Ch17 Equilibrium The Extent Of Test Questions & Answers

Chapter 17 Test Bank

Equilibrium: The Extent of Chemical Reactions

1. An equilibrium is established in which both the forward (fwd) and the reverse (rev) reactions are elementary. If the equilibrium constant K_c = 1.6 × 10^–2 and the rate constant k_fwd = 8.0 × 10^–7 s^–1 what is the value of k_rev?

A. 1.3 × 10^–8 s^–1

B. 7.8 × 10⁷ s^–1

C. 2 × 10⁴ s^–1

D. 5.0 × 10^–5 s^–1

E. None of these choices are correct.

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

2. Consider the equilibrium reaction shown below.

B2(g) 2B(g)

If the rate constants are: k_fwd = 7.00 × 10^–5s^–1 and k_rev = 2.00 × 10^–5 L mol^–1 s^–1, what is the value of K_c under these conditions?

A. 1.75 × 10⁵

B. 3.50

C. 0.286

D. 5.71 × 10^–6

E. 1.40 × 10^–10

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

3. When a chemical system is at equilibrium,

A. the concentrations of the reactants are equal to the concentrations of the products.

B. the concentrations of the reactants and products have reached constant values.

C. the forward and reverse reactions have stopped.

D. the reaction quotient, , has reached a maximum.

E. the reaction quotient, , has reached a minimum.

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

4. A chemical reaction has an equilibrium constant of 2 × 10⁶. If this reaction is at equilibrium, select the one correct conclusion that can be made about the reaction.

A. The forward and back reactions have stopped.

B. The limiting reactant has been used up.

C. The forward and reverse rate constants are equal.

D. The forward and reverse reaction rates are equal.

E. None of these choices are correct.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

5. Which of the following has an effect on the magnitude of the equilibrium constant?

A. removing products as they are formed

B. adding more of a reactant

C. adding a catalyst

D. increasing the pressure, in a gas-phase reaction

E. change in temperature

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

6. In order to write the correct mass-action expression for a reaction one must

A. know the kinetic rate law for the reaction.

B. know the mechanism for the reaction.

C. have a properly balanced chemical equation.

D. have values for the concentrations of the reactants.

E. know the limiting reactant.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

7. The two equilibrium constants for the same reaction, K_c and K_p, will always equal one another when

A. all of the reactants and products are gases.

B. in the reaction equation, the number of moles of gaseous products equals the number of moles of gaseous reactants.

C. in the reaction equation, the number of moles of gaseous products is greater than the number of moles of gaseous reactants.

D. in the reaction equation, the number of moles of gaseous products is smaller than the number of moles of gaseous reactants.

E. in the reaction equation, the total number of moles of reactants equals that of the products.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Easy

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

8. The reaction quotient for a gas phase reaction has a value of 2000. If the number of moles of reactants in the reaction equation is equal to that of the products, which of the following statements is definitely true?

A. The reaction must proceed to the left to establish equilibrium.

B. The reaction must proceed to the right to establish equilibrium.

C. When the system is at equilibrium, the concentrations of the products will be much larger than the concentrations of the reactants.

D. The concentrations of the products are generally larger than the concentrations of the reactants.

E. None of these choices are correct.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

9. The reaction quotient, _c, for a reaction has a value of 75 while the equilibrium constant, K_c, has a value of 195. Which of the following statements is accurate?

A. The reaction must proceed to the left to establish equilibrium.

B. The reaction must proceed to the right to establish equilibrium.

C. The concentrations of the products will be much smaller than the concentrations of the reactants when the system is at equilibrium.

D. The concentrations of the products will be about the same as the concentrations of the reactants when the system is at equilibrium.

E. None of these choices are correct.

Bloom's: 2. Understand

Difficulty: Easy

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

10. Carbon monoxide and chlorine combine in an equilibrium reaction to produce the highly toxic product, phosgene (COCl₂)

CO(g) + Cl₂(g) COCl₂(g)

If the equilibrium constant for this reaction is K_c = 248, predict, if possible, what will happen when the reactants and product are combined with the concentrations shown.

[CO] = [Cl₂] = 0.010 M; [COCl₂] = 0.070 M

A. The reaction will proceed to the right.

B. The reaction will proceed to the left.

C. The reaction is at equilibrium, and no change in concentrations will occur.

D. The container volume needs to be specified before a prediction can be made.

E. The temperature needs to be specified before a prediction can be made.

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

11. Carbon monoxide and chlorine combine in an equilibrium reaction to produce the highly toxic product, phosgene (COCl₂)

CO(g) + Cl₂(g)COCl₂(g)

If the equilibrium constant for this reaction is Kc = 248, predict, if possible, what will happen when the reactants and product are combined with the concentrations shown.

[CO] = [Cl₂] = 0.0200 M; [COCl₂] = 0.0992 M

A. The reaction will proceed to the right.

B. The reaction will proceed to the left.

C. The reaction is at equilibrium, and no change in concentrations will occur.

D. The container volume needs to be specified before a prediction can be made.

E. The temperature needs to be specified before a prediction can be made.

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

12. Write the mass-action expression, _c, for the following chemical reaction equation.

2C₆H₆(g) + 15O₂(g) 12CO₂(g) + 6H₂O(g)

A.

B.

C.

D.

E.

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

13. What is the mass-action expression, p, for the following reaction?

SbF₅(g) + 4Cl₂(g)SbCl₃(g) + 5ClF(g)

A.

B.

C.

D.

E. None of these choices are correct.

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

14. Write the mass-action expression, c, for the following chemical reaction.

NO(g) + ½Br₂(g) NOBr(g)

A.

B.

C.

D.

E.

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

15. Write the mass-action expression, c, for the following chemical reaction.

3ClO₂^–(aq) 2ClO₃^–(aq) + Cl^–(aq)

A.

B.

C.

D.

E.

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

16. What is the mass-action expression, c, for the following chemical reaction?

Cu₂₊(aq) + 4NH₃(aq)Cu(NH₃)₄²⁺(aq)

A.

B.

C.

D.

E. None of these choices are correct.

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

17. Write the mass-action expression, c, for the following chemical reaction.

2Cu₂₊(aq) + 4I^–(aq) 2CuI(s) + I₂(aq)

A.

B.

C.

D.

E.

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

18. Write the mass-action expression, c, for the following chemical reaction.

Zn(s) + 2Ag⁺(aq)Zn²⁺(aq) + 2Ag(s)

A.

B.

C.

D.

E.

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

19. Write the mass-action expression, c, for the following chemical reaction.

Fe³⁺(aq) + 3OH^–(aq) Fe(OH)₃(s)

A.

B.

C.

D.

E.

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

20. What is the mass-action expression, c, for the following chemical reaction?

PbO(s) + CO(g) Pb(l) + CO₂(g)

A.

B.

C.

D.

E. None of these choices are correct.

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

21. What is the mass-action expression, c, for the following chemical reaction?

4H₃O⁺(aq) + 2Cl^–(aq) + MnO₂(s) Mn²⁺(aq) + 6H₂O(l) + Cl₂(g)

A.

B.

C.

D.

E. None of these choices are correct.

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

22. Write the mass-action expression, c, for the following chemical reaction.

MgO(s) + SO₂(g) + ½O₂(g) MgSO₄(s)

A.

B.

C.

D.

E. None of these choices are correct.

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

23. Write the mass-action expression, c, for the following chemical reaction.

Sn²⁺(aq) + ½O₂(g) + 3H₂O(l) SnO₂(s) + 2H₃O⁺(aq)

A.

B.

C.

D.

E. None of these choices are correct.

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

24. Consider the reactions of cadmium with the thiosulfate anion.

Cd²⁺(aq) + S₂O₃^2–(aq) Cd(S₂O₃)(aq) K₁ = 8.3 × 10³

Cd(S₂O₃)(aq) + S₂O₃^2–(aq) Cd(S₂O₃)₂^2–(aq) K₂ = 2.5 × 10²

What is the value for the equilibrium constant for the following reaction?

Cd²⁺(aq) + 2S₂O₃^2–(aq) Cd(S₂O₃)₂^2–(aq)

A. 0.030

B. 33

C. 8.1 × 10³

D. 8.6 × 10³

E. 2.1 × 10⁶

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

25. N₂(g) + O₂(g) 2NO(g) K_c = 4.8 × 10^–31

2NOBr(g) 2NO(g) + Br₂(g) K_c = 0.50

Given the above equilibrium constant data at 25°C, what is the value of K_c at this temperature for the reaction

2NOBr(g) N₂(g) + O₂(g) + Br₂(g)?

A. 2.4 × 10^–31

B. 9.6 × 10^–31

C. 1.0 × 10³⁰

D. 4.2 × 10³⁰

E. None of these choices are correct.

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

26. H₂SO₃(aq) HSO₃(aq) + H⁺(aq) K_c = 1.4 × 10^–2

H₂SO₃(aq) SO₃^2–(aq) + 2H⁺(aq) K_c = 9.1 × 10^–10

Given the above equilibrium constant data at 25°C, what is the value of K_c at this temperature for the reaction

HSO₃^–(aq) SO₃^2–(aq) + H⁺(aq)?

A. 6.5 ×10^–8

B. 1.3 × 10^–11

C. 7.8 × 10¹⁰

D. 1.5 × 10⁷

E. None of these choices are correct.

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

27. Hydrogen sulfide will react with water as shown in the following reactions.

H₂S(g) + H₂O(l) H₃O⁺(aq) + HS^–(aq) K₁ = 1.0 × 10^–7

HS^–(aq) + H₂O(l) H₃O⁺(aq) + S^2–(aq) K₂ = ?

H₂S(g) + 2H₂O(l) 2H₃O⁺(aq) + S^2–(aq) K₃ = 1.3 × 10^–20

What is the value of K₂?

A. 1.3 × 10^–27

B. 2.3 × 10^–7

C. 1.3 × 10^–13

D. 7.7 × 10¹²

E. 7.7 × 10²⁶

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

28. At 500°C the equilibrium constant, K_p, is 4.00 × 10^–4 for the equilibrium:

2HCN(g) H₂(g) + C₂N₂(g)

What is Kp for the following reaction?

H₂(g) + C₂N₂(g) 2HCN(g)

A. 2.00 × 10^–4

B. –4.00 × 10^–4

C. 1.25 × 10³

D. 2.50 × 10³

E. 4.00 × 10⁴

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

29. About half of the sodium carbonate produced is used in making glass products because it lowers the melting point of sand, the major component of glass. When sodium carbonate is added to water it hydrolyses according to the following reactions.

CO₃^2–(aq) + H₂O(l) HCO₃^–(aq) + OH^–(aq) K₁

HCO₃(aq) + H₂O(l) H₂CO₃(aq) + OH^–(aq) K₂

These can be combined to yield

CO₃^2–(aq) + 2H₂O(l) H₂CO₃(aq) + 2OH^–(aq) K₃

What is the value of K₃?

A. K₁ × K₂

B. K₁ ÷ K₂

C. K₁ + K₂

D. K₁ – K₂

E. (K₁K₂)²

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

30. The equilibrium constant, K_c, for the decomposition of COBr₂

COBr₂(g) CO(g) + Br₂(g)

is 0.190. What is K_c for the following reaction?

2CO(g) + 2Br₂(g) 2COBr₂(g)

A. 0.0361

B. 2.63

C. 5.62

D. 10.5

E. 27.7

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

31. The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature.

Br₂(g) + Cl₂(g) 2BrCl(g)

What is the equilibrium constant for the following reaction?

BrCl(g) ½Br₂(g) + ½Cl₂(g)

A. 2.97 × 10^–4

B. 1.72 × 10^–2

C. 3.45 × 10^–2

D. 1.31 × 10^–1

E. > 1.00

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

32. Consider the following two equilibria and their respective equilibrium constants:

(1) NO(g) + ½O2(g) NO2(g)

(2) 2NO₂(g) 2NO(g) + O₂(g)

Which one of the following is the correct relationship between the equilibrium constants K₁ and K₂?

A. K₂ = 2/K₁

B. K₂ = (1/K₁)²

C. K₂ = –K₁/2

D. K₂ = 1/(2K₁)

E. K₂ = 1/(2K₁)²

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

33. The equilibrium constant for reaction (1) below is 276. Under the same conditions, what is the equilibrium constant of reaction (2)?

(1) ½X₂(g) + ½Y₂(g) XY(g)

(2) 2XY(g) X₂(g) + Y₂(g)

A. 6.02 × 10^–2

B. 7.25 × 10^–3

C. 3.62 × 10^–3

D. 1.31 × 10^–5

E. None of these choices are correct.

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

34. In water, the following equilibrium exists:

H⁺(aq) + OH^–(aq) H₂O(l)

In pure water at 25°C, the concentration of H+ ions is 1.00 × 10^–7 mol/L. Calculate the value of the equilibrium constant for the reaction as written above.

A. 1.00 × 10¹⁴

B. 1.00 × 10¹²

C. 1.00 × 10^–14

D. 1.00 × 10^–12

E. 5.55 × 10¹⁵

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

35. Consider the equilibrium reaction: N₂O₄(g) 2NO₂(g)

Which of the following correctly describes the relationship between K_c and K_p for the reaction?

A. K_p = K_c

B. K_p = RT × K_c

C. K_p = (RT × K_c)^–1

D. K_p = K_c / RT

E. K_p = RT / K_c

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

36. Consider the equilibrium reaction: H₂(g) + Br₂(g) 2HBr(g)

Which of the following correctly describes the relationship between K_c and K_p for the reaction?

A. K_p = K_c

B. K_p = (RT)K_c

C. K_p = (RT)2K_c

D. K_p = K_c / RT

E. K_p = K_c / (RT)²

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

37. The equilibrium constant, K_p, has a value of 6.5 × 10^–4 at 308 K for the reaction of nitrogen monoxide with chlorine.

2NO(g) + Cl₂(g) 2NOCl(g)

What is the value of K_c?

A. 2.5 × 10^–7

B. 6.5 × 10^–4

C. 1.6 × 10^–2

D. 1.7

E. None of these choices are correct.

Bloom's: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

38. The reaction of nitrogen with oxygen to form nitrogen monoxide can be represented by the following equation.

N₂(g) + O₂(g) 2NO(g)

At 2000°C, the equilibrium constant, K_c, has a value of 4.10 × 10^–4. What is the value of K_p?

A. 2.17 × 10^–8

B. 4.10 × 10^–4

C. 7.65 × 10^–2

D. 7.75

E. None of these choices are correct.

Bloom's: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

39. Nitrogen dioxide decomposes according to the reaction

2NO₂(g) 2NO(g) + O₂(g)

where K_p = 4.48 × 10^–13 at 25°C. What is the value for K_c?

A. 1.81 × 10^–16

B. 1.83 × 10^–14

C. 4.48 × 10^–13

D. 1.10 × 10^–11

E. 1.11 × 10^–9

Bloom's: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

40. The equilibrium constant, Kp, for the reaction

H₂(g) + I₂(g) 2HI(g)

is 55.2 at 425°C. A rigid cylinder at that temperature contains 0.127 atm of hydrogen, 0.134 atm of iodine, and 1.055 atm of hydrogen iodide. Is the system at equilibrium?

A. Yes.

B. No, the forward reaction must proceed to establish equilibrium.

C. No, the reverse reaction must proceed to establish equilibrium.

D. Need to know the volume of the container before deciding.

E. Need to know the starting concentrations of all substances before deciding.

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

41. The equilibrium constant, Kp, for the reaction

CO(g) + H₂O(g) CO₂(g) + H₂(g)

at 986°C is 0.63. A rigid cylinder at that temperature contains 1.2 atm of carbon monoxide, 0.20 atm of water vapor, 0.30 atm of carbon dioxide, and 0.27 atm of hydrogen. Is the system at equilibrium?

A. Yes.

B. No, the forward reaction must proceed to establish equilibrium.

C. No, the reverse reaction must proceed to establish equilibrium.

D. Need to know the volume of the container before deciding.

E. Need to know the starting concentrations of all substances before deciding.

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

42. Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached

P_NO = 0.526 atm, = 1.59 atm, and P_NOBr = 7.68 atm. Calculate K_p for the reaction.

2NO(g) + Br₂(g) 2NOBr(g)

A. 7.45 × 10^–3

B. 0.109

C. 9.18

D. 91.8

E. 134

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

43. Compounds A, B, and C react according to the following equation.

3A(g) + 2B(g) 2C(g)

At 100°C a mixture of these gases at equilibrium showed that [A] = 0.855 M, [B] = 1.23 M, and [C] = 1.75 M. What is the value of K_c for this reaction?

A. 0.309

B. 0.601

C. 1.66

D. 3.24

E. > 10

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

44. Consider the reversible reaction: 2NO₂(g) N₂O₄(g)

If the concentrations of both NO₂ and N₂O₄ are 0.016 mol L^–1, what is the value of _c?

A. 0.016

B. 0.50

C. 1.0

D. 2.0

E. 63

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

45. 10.0 mL of a 0.100 mol L^–1 solution of a metal ion M²⁺ is mixed with 10.0 mL of a 0.100 mol L^–1 solution of a substance L. The following equilibrium is established:

M²⁺(aq) + 2L(aq) ML₂²⁺(aq)

At equilibrium the concentration of L is found to be 0.0100 mol L^–1. What is the equilibrium concentration of ML₂²⁺, in mol L^–1?

A. 0.100 mol L^–1

B. 0.050 mol L^–1

C. 0.025 mol L^–1

D. 0.0200 mol L^–1

E. 0.0100 mol L^–1

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Calculating Equilibrium Concentration

Topic: Chemical Equilibrium

46. Hydrogen iodide, HI, is formed in an equilibrium reaction when gaseous hydrogen and iodine gas are heated together. If 20.0 g of hydrogen and 20.0 g of iodine are heated, forming 10.0 g of hydrogen iodide, what mass of hydrogen remains unreacted?

A. 10.0 g hydrogen remains

B. 10.9 g hydrogen remains

C. 15.0 g hydrogen remains

D. 19.9 g hydrogen remains

E. Need to know the equilibrium constant in order to calculate the answer.

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Calculating Equilibrium Concentration

Topic: Chemical Equilibrium

47. SO₂ reacts with O₂ to produce SO₃. If 86.0 g of SO₂ is placed in a reaction vessel along with excess oxygen gas, how many moles of SO₂ remain when 50.0 g of SO₃ have been formed?

A. 0.56 mol

B. 0.62 mol

C. 0.72 mol

D. 0.78 mol

E. 1.34 mol

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Calculating Equilibrium Concentration

Topic: Chemical Equilibrium

48. At high temperatures, carbon reacts with O₂ to produce CO as follows:

C(s) + O₂(g) 2CO(g).

When 0.350 mol of O₂ and excess carbon were placed in a 5.00-L container and heated, the equilibrium concentration of CO was found to be 0.060 M. What is the equilibrium constant, K_c, for this reaction?

A. 0.010

B. 0.072

C. 0.090

D. 0.17

E. 1.2

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Calculating Equilibrium Concentration

Topic: Chemical Equilibrium

49. A mixture of 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid

1.00-L container and the system was allowed to come to equilibrium. The equilibrium

concentration of COBr₂ was 0.233 M. What is the value of Kc for this reaction?

CO(g) + Br₂(g) COBr₂(g)

A. 5.23

B. 1.22

C. 1.165

D. 0.858

E. 0.191

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Calculating Equilibrium Concentration

Topic: Chemical Equilibrium

50. A mixture of 0.600 mol of bromine and 1.600 mol of iodine is placed into a rigid 1.000-L container at 350°C.

Br₂(g) + I₂(g) 2IBr(g)

When the mixture has come to equilibrium, the concentration of iodine monobromide is 1.190 M. What is the equilibrium constant for this reaction at 350°C?

A. 3.55 × 10^–3

B. 1.24

C. 1.47

D. 282

E. 325

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Calculating Equilibrium Concentration

Topic: Chemical Equilibrium

51. The equilibrium constant Kc for the reaction

PCl₃(g) + Cl₂(g) PCl₅(g)

is 49 at 230°C. If 0.70 mol of PCl₃ is added to 0.70 mol of Cl₂ in a 1.00-L reaction vessel at 230°C, what is the concentration of PCl₃ when equilibrium has been established?

A. 0.049 M

B. 0.11 M

C. 0.30 M

D. 0.59 M

E. 0.83 M

Bloom's: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Calculating Equilibrium Concentration

Topic: Chemical Equilibrium

52. The equilibrium constant Kc for the reaction

A(g) + B(g) C(g)

is 0.76 at 150°C. If 0.800 mol of A is added to 0.600 mol of B in a 1.00-L container at 150°C, what will be the equilibrium concentration of C?

A. 0.19 M

B. 0.29 M

C. 0.36 M

D. 0.41 M

E. 0.51 M

Bloom's: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Calculating Equilibrium Concentration

Topic: Chemical Equilibrium

53. Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures.

N₂(g) + O₂(g) 2NO(g)

The equilibrium constant K_p for the reaction is 0.0025 at 2127°C. If a container is charged with 8.00 atm of nitrogen and 5.00 atm of oxygen and the mixture is allowed to reach equilibrium, what will be the equilibrium partial pressure of nitrogen?

A. 0.16 atm

B. 0.31 atm

C. 3.1 atm

D. 7.7 atm

E. 7.8 atm

Bloom's: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Calculating Equilibrium Concentration

Topic: Chemical Equilibrium

54. The following reaction, in CCl4 solvent, has been studied at 25°C.

2BrClBr₂ + Cl₂

The equilibrium constant Kc is known to be 0.141. If the initial concentration of chlorine is 0.0300 M and of bromine monochloride is 0.0200 M, what is the equilibrium concentration of bromine?

A. 1.35 × 10^–3 M

B. 2.70 × 10^–3 M

C. 8.82 × 10^–3 M

D. 9.70 × 10^–2 M

E. None of these choices are correct.

Bloom's: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Calculating Equilibrium Concentration

Topic: Chemical Equilibrium

55. At 25°C, the equilibrium constant Kc for the reaction

2A(aq) B(aq) + C(aq)

is 65. If 2.50 mol of A is added to enough water to prepare 1.00 L of solution, what will the equilibrium concentration of A be?

A. 0.038 M

B. 0.14 M

C. 0.28 M

D. 1.18 M

E. 2.4 M

Bloom's: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Calculating Equilibrium Concentration

Topic: Chemical Equilibrium

56. At a certain temperature the reaction

CO₂(g) + H₂(g) CO(g) + H₂O(g)₂

has K_c = 2.50. If 2.00 mol of carbon dioxide and 1.5 mol of hydrogen are placed in a 5.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide?

A. 0.091 M

B. 0.191 M

C. 0.209 M

D. 0.913 M

E. 1.05 M

Bloom's: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Calculating Equilibrium Concentration

Topic: Chemical Equilibrium

57. At 25°C, the equilibrium constant K_c for the reaction

2A(g) B(g) + C(g)

is 0.035. A mixture of 8.00 moles of B and 12.00 moles of C in a 20.0 L container is allowed to come to equilibrium. What is the equilibrium concentration of A?

A. < 0.100 M

B. 0.339 M

C. 0.678 M

D. 6.78 M

E. 13.56 M

Bloom's: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Calculating Equilibrium Concentration

Topic: Chemical Equilibrium

58. At 850°C, the equilibrium constant Kp for the reaction

C(s) + CO₂(g) 2CO(g)

has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide?

A. 0.362 atm

B. 0.489 atm

C. 0.667 atm

D. 0.915 atm

E. 0.921 atm

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Calculating Equilibrium Concentration

Topic: Chemical Equilibrium

59. Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide.

NH₄I(s) NH₃(g) + HI(g)

At 400°C, K_p = 0.215. Calculate the partial pressure of ammonia at equilibrium when a sufficient quantity of ammonium iodide is heated to 400°C.

A. 0.103 atm

B. 0.215 atm

C. 0.232 atm

D. 0.464 atm

E. 2.00 atm

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Calculating Equilibrium Concentration

Topic: Chemical Equilibrium

60. The reaction system

POCl₃(g) POCl(g) + Cl₂(g)

is at equilibrium. Which of the following statements describes the behavior of the system if POCl is added to the container?

A. The forward reaction will proceed to establish equilibrium.

B. The reverse reaction will proceed to establish equilibrium.

C. The partial pressures of POCl₃ and POCl will remain steady while the partial pressure of chlorine increases.

D. The partial pressure of chlorine remains steady while the partial pressures of POCl₃ and POCl increase.

E. The partial pressure of chlorine will increase while the partial pressure of POCl decreases.

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

61. The reaction system

POCl₃(g) POCl(g) + Cl₂(g)

is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of chlorine is reduced by 50%?

A. POCl₃ will be consumed as equilibrium is established.

B. POCl will be consumed as equilibrium is established.

C. Chlorine will be consumed as equilibrium is established.

D. The partial pressure of POCl will decrease while the partial pressure of Cl₂ increases as equilibrium is established.

E. The volume will have to decrease before equilibrium can be reestablished.

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

62. The reaction system

CS₂(g) + 4H₂(g) CH₄(g) + 2H₂S(g)

is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of hydrogen is doubled?

A. As equilibrium is reestablished, the partial pressure of carbon disulfide increases.

B. As equilibrium is reestablished, the partial pressure of methane, CH₄, decreases.

C. As equilibrium is reestablished, the partial pressure of hydrogen decreases.

D. As equilibrium is reestablished, the partial pressure of hydrogen sulfide decreases.

E. As equilibrium is reestablished, all the partial pressures will decrease.

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

63. The reaction system

CS₂(g) + 4H₂(g) CH₄(g) + 2H₂S(g)

is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of carbon disulfide is reduced?

A. As equilibrium is reestablished, the partial pressure of carbon disulfide increases.

B. As equilibrium is reestablished, the partial pressure of hydrogen decreases.

C. As equilibrium is reestablished, the partial pressure of methane, CH₄, increases.

D. As equilibrium is reestablished, the partial pressures of hydrogen and hydrogen sulfide decrease.

E. As equilibrium is reestablished, all the partial pressures will increase.

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

64. Magnesium hydroxide is used in several antacid formulations. When it is added to water it dissociates into magnesium and hydroxide ions.

Mg(OH)₂(s) Mg²⁺(aq) + 2OH^–(aq)

The equilibrium constant at 25°C is 8.9 × 10^–12. One hundred grams of magnesium hydroxide is added to 1.00 L of water and equilibrium is established. What happens to the solution if another 10 grams of Mg(OH)₂ are now added to the mixture?

A. The hydroxide ion concentration will decrease.

B. The hydroxide ion concentration will increase.

C. The hydroxide ion concentration will be unchanged.

D. The solution will become supersaturated.

E. None of these choices are correct.

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

65. Sodium hydrogen carbonate decomposes above 110°C to form sodium carbonate, water, and carbon dioxide.

2NaHCO₃(s) Na₂CO₃(s) + H₂O(g) + CO₂(g)

One thousand grams of sodium hydrogen carbonate are added to a reaction vessel, the temperature is increased to 200°C, and the system comes to equilibrium. What happens in this system if another 50 g of sodium carbonate are now added?

A. The partial pressure of carbon dioxide will increase.

B. The partial pressure of carbon dioxide will decrease.

C. The partial pressure of carbon dioxide will be unchanged.

D. The amounts of all products will be greater when equilibrium is reestablished.

E. None of these choices are correct.

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

66. Methanol can be synthesized by combining carbon monoxide and hydrogen.

CO(g) + 2H₂(g) CH₃OH(g)

A reaction vessel contains the three gases at equilibrium with a total pressure of 1.00 atm. What will happen to the partial pressure of hydrogen if enough argon is added to raise the total pressure to 1.4 atm?

A. The partial pressure of hydrogen will decrease.

B. The partial pressure of hydrogen will increase.

C. The partial pressure of hydrogen will be unchanged.

D. K_p needs to be known before a prediction can be made.

E. Both K_p and the temperature need to be known before a prediction can be made.

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

67. At 450°C, tert-butyl alcohol decomposes into water and isobutene.

(CH₃)₃COH(g) (CH₃)₂CCH₂(g) + H₂O(g)

A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature?

A. The forward reaction will proceed to reestablish equilibrium.

B. The reverse reaction will proceed to reestablish equilibrium.

C. No change occurs.

D. The equilibrium constant will increase.

E. The equilibrium constant will decrease.

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

68. A container was charged with hydrogen, nitrogen, and ammonia gases at 120°C and the system was allowed to reach equilibrium. What will happen if the volume of the container is increased at constant temperature?

3H₂(g) + N₂(g) 2NH₃(g)

A. There will be no effect.

B. More ammonia will be produced at the expense of hydrogen and nitrogen.

C. Hydrogen and nitrogen will be produced at the expense of ammonia.

D. The equilibrium constant will increase.

E. The equilibrium constant will decrease.

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

69. Magnesium carbonate dissociates to magnesium oxide and carbon dioxide at elevated temperatures.

MgCO₃(s) MgO(s) + CO₂(g)

A reaction vessel contains these compounds in equilibrium at 300°C. What will happen if the volume of the container is reduced by 25% at 300°C?

A. The partial pressure of carbon dioxide present at equilibrium will increase.

B. The partial pressure of carbon dioxide present at equilibrium will decrease.

C. The partial pressure of carbon dioxide at equilibrium will be unchanged.

D. The equilibrium constant will have to decrease to compensate for the decrease in volume.

E. More information is needed in order to make a valid judgment.

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

70. The reaction of nitric oxide to form dinitrogen oxide and nitrogen dioxide is exothermic.

3NO(g) N₂O(g) + NO₂(g) + heat

What effect will be seen if the temperature of the system at equilibrium is raised by 25°C?

A. The partial pressure of NO will increase.

B. The partial pressure of NO will decrease.

C. The partial pressure of NO₂ will increase.

D. The partial pressures of NO and N₂O will increase.

E. All three partial pressures will increase.

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

71. Methanol can be synthesized by combining carbon monoxide and hydrogen.

CO(g) + 2H₂(g) CH₃OH(g) ΔH°_rxn = –90.7 kJ

A reaction vessel contains these compounds at equilibrium. What effect will be seen when equilibrium is re-established after decreasing the temperature by 45°C?

A. All the partial pressures will decrease.

B. The partial pressure of methanol will decrease.

C. The partial pressures of hydrogen and methanol will decrease.

D. The partial pressure of hydrogen will increase.

E. The partial pressure of carbon monoxide will decrease.

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

72. Hydrogen bromide will dissociate into hydrogen and bromine gases.

2HBr(g) H₂(g) + Br₂(g) ΔH°_rxn = 68 kJ

What effect will a temperature increase of 50°C have on this system at equilibrium?

A. The partial pressure of hydrogen bromide will increase.

B. The partial pressure of hydrogen will increase.

C. The partial pressure of hydrogen bromide and bromine will increase.

D. There will be no effect on the partial pressure of any of the gases.

E. Need to know the initial pressure, volume, and temperature before any of the above predictions can be made.

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

73. Ethane can be formed by reacting acetylene with hydrogen.

C₂H₂(g) + 2H₂(g) C₂H₆(g) ΔH°_rxn = –311 kJ

Under which reaction conditions would you expect to have the greatest equilibrium yield of ethane?

A. high temperature, high pressure

B. low temperature, high pressure

C. high temperature, low pressure

D. low temperature, low pressure

E. None of these choices are correct.

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

74. Nitrogen dioxide can dissociate to nitric oxide and oxygen.

2NO₂(g)2NO(g) + O₂(g) ΔH°_rxn = +114 kJ

Under which reaction conditions would you expect to produce the largest amount of oxygen?

A. high temperature, high pressure

B. low temperature, high pressure

C. high temperature, low pressure

D. low temperature, low pressure

E. None of these choices are correct.

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

75. The following reaction is at equilibrium at one atmosphere, in a closed container.

NaOH(s) + CO₂(g) NaHCO₃(s)

Which, if any, of the following actions will decrease the total amount of CO₂ gas present at equilibrium?

A. adding N₂ gas to double the pressure

B. adding more solid NaOH

C. decreasing the volume of the container

D. removing half of the solid NaHCO₃

E. None of these choices are correct.

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

76. The following reaction is at equilibrium at a pressure of 1 atm, in a closed container.

NaOH(s) + CO₂(g) NaHCO₃(s) ΔH°_rxn < 0

Which, if any, of the following actions will decrease the concentration of CO₂ gas present at equilibrium?

A. adding N₂ gas to double the pressure

B. adding more solid NaOH

C. increasing the volume of the container

D. lowering the temperature

E. None of these choices are correct.

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

77. The following reaction is at equilibrium in a closed container.

CuSO₄.5H₂O(s) CuSO₄(s) + 5H₂O(g)

Which, if any, of the following actions will lead to an increase in the pressure of H₂O present at equilibrium?

A. increasing the volume of the container

B. decreasing the volume of the container

C. adding a catalyst

D. removing some solid CuSO₄

E. None of these choices are correct.

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

78. The following reaction is at equilibrium in a sealed container.

N₂(g) + 3H₂(g) 2NH₃(g) ΔH°_rxn < 0

Which, if any, of the following actions will increase the value of the equilibrium constant, K_c?

A. adding a catalyst

B. adding more N₂

C. increasing the pressure

D. lowering the temperature

E. None of these choices are correct.

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

79. Stearic acid, nature's most common fatty acid, dimerizes when dissolved in hexane:

2C₁₇H₃₅COOH (C₁₇H₃₅COOH)₂ ΔH°_rxn = –172 kJ

The equilibrium constant for this reaction at 28°C is 2900. Estimate the equilibrium constant at 38°C.

A. 4.7 × 10⁵

B. 2.6 × 10⁴

C. 1.9 × 10³

D. 3.2 × 10²

E. 18

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

80. Hydrogen sulfide can be formed in the following reaction:

H₂(g) + ½S₂(g) H₂S(g) ΔH°rxn = –92 kJ

The equilibrium constant K_p = 106 at 1023 K. Estimate the value of K_p at 1218 K.

A. 5.05

B. 18.8

C. 34.7

D. 88.9

E. 598

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

81. Although a system may be at equilibrium, the rate constants of the forward and reverse reactions will in general be different.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

82. When a reaction system reaches equilibrium, the forward and reverse reactions stop.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

83. Once a reaction system reaches equilibrium, the concentrations of reactions and products no longer change.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

84. A chemical reaction will reach equilibrium when the limiting reactant is used up.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

85. Increasing the initial amount of the limiting reactant in a reaction will increase the value of the equilibrium constant, K_c.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

86. In a chemical reaction, if the starting concentrations of reactants are increased, then the equilibrium constant K_c will also increase.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

87. There is a direct correlation between the speed of a reaction and its equilibrium constant.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

88. If all of the coefficients in the balanced equation for an equilibrium reaction are doubled, then the value of the equilibrium constant, K_c, will also be doubled.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

89. For a gas-phase equilibrium, a change in the pressure of any single reactant or product will change K_p.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

90. If all the reactants and products in an equilibrium reaction are in the gas phase, then K_p = K_c.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Easy

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

91. For a gas-phase equilibrium, a change in the pressure of any single reactant or product will affect the amounts of other substances involved in the equilibrium.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Easy

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

92. For a solution equilibrium, a change in concentration of a reactant or product does not change K_c.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

93. For some gas-phase reactions, K_p = K_c.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

94. If > K, more products need to be formed as the reaction proceeds to equilibrium.

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

95. Changing the amount of a solid reactant or product in an equilibrium reaction will not affect the amounts of the other reactants and products present at equilibrium.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

96. Unless ΔH°_rxn = 0, a change in temperature will affect the value of the equilibrium constant K_c.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume)

Topic: Chemical Equilibrium

97. A good catalyst for a reaction will speed up the forward reaction and slow down the reverse reaction.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Catalysis

Topic: Chemical Kinetics (Reaction Rates)

98. Chemical reactions generally reach equilibrium because one of the reactants is used up.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Equilibrium Constant and Reaction Quotient

Topic: Chemical Equilibrium

Category # of Questions

Accessibility: Keyboard Navigation 25

Bloom's: 1. Remember 19

Bloom's: 2. Understand 7

Bloom's: 3. Apply 72

Difficulty: Easy 38

Difficulty: Hard 10

Difficulty: Medium 50

Gradable: automatic 98

Subtopic: Calculating Equilibrium Concentration 15

Subtopic: Catalysis 1

Subtopic: Equilibrium Constant and Reaction Quotient 57

Subtopic: Le Châtelier's Principle (Effect of Temperature (van't Hoff Eq.), Pressure, Volume) 25

Topic: Chemical Equilibrium 97

Topic: Chemical Kinetics (Reaction Rates) 1