Verified Test Bank Chemical Equilibrium Ch15 - MCQ Test Bank | Introductory Chemistry - 2nd Edition by Burdge and Driessen by Julia Burdge, Michelle Driessen. DOCX document preview.
Student name:__________
TRUE/FALSE - Write 'T' if the statement is true and 'F' if the statement is false.
1) Ethanol (C2H5–OH) will have a greater viscosity than ethylene glycol (HO–CH2CH2–OH) at the same temperature.
⊚ true
⊚ false
MULTIPLE CHOICE - Choose the one alternative that best completes the statement or answers the question.
2) Which state of matter is described as taking on the shape and volume of its container?
A) solid
B) liquid
C) gas
D) solution
E) mixture
3) Which state of matter is described as having a definite shape and volume?
A) solid
B) liquid
C) gas
D) solution
E) mixture
4) Which state of matter is described as taking on the shape of its container, but having a specific volume?
A) solid
B) liquid
C) gas
D) solution
E) mixture
5) Which one of the following crystallizes in a metallic lattice?
A) C
B) NaMnO 4
C) K
D) LiClO 4
E) K2Cr2O7
6) If liquid bromine is cooled to form a solid, which type of solid does it form?
A) atomic
B) metallic
C) molecular
D) ionic
E) covalent
7) For the solid forms of the following elements, which one is most likely to be of the molecular type?
A) Cs
B) C
C) Pb
D) S
E) Cr
8) Which of the following lacks a regular three-dimensional arrangement of atoms?
A) crystalline solids
B) ionic crystals
C) solids
D) amorphous solids
E) molecular solids
9) Which of the substances would form an ionic solid?
A) NCl3
B) NH4Cl
C) Ag
D) He
E) OF2
10) Which of the substances would form a metallic solid?
A) NCl3
B) KCl
C) Ni
D) Ar
E) MgF2
11) Ammonia's unusually high melting point is the result of
A) dipole-dipole forces.
B) London dispersion forces.
C) hydrogen bonding.
D) covalent bonding.
E) ionic bonding.
12) Place the substances in order of increasing melting point.CS2 KCl NF3
A) CS2 < NF3 < KCl
B) KCl < NF3 < CS2
C) NF3 < CS2 < KCl
D) CS2 < KCl < NF3
E) NF3 < KCl < CS2
13) Place the substances in order of increasing melting point.CH4 C3H8 C2H4
A) C3H8 < C2H4 < CH4
B) C2H4 < CH4 < C3H8
C) C3H8 < CH4 < C2H4
D) CH4 < C2H4 < C3H8
E) C2H4 < C3H8 < CH4
14) Place the substances in order of increasing melting point.CO2 CH4 OF2
A) OF2 < CO2 < CH4
B) CH4 < CO2 < OF2
C) OF2 < CH4 < CO2
D) CO2 < CH4 < OF2
E) CO2 < OF2 < CH4
15) The energy required to increase the surface of a liquid per unit area is called the
A) capillary action.
B) surface tension.
C) viscosity.
D) cohesion.
E) specific elasticity.
16) Which has the highest surface tension at room temperature?
A) CH 4
B) CF 4
C) CCl 4
D) CBr 4
E) CI4
17) Which has the highest surface tension at a given temperature?
A)
B)
C)
D)
E)
18) What is determined by the magnitude of intermolecular forces in a liquid and is a measure of a fluid's resistance to flow?
A) surface tension
B) adhesion
C) polarity
D) viscosity
E) cohesion
19) Which of the following terms refers to the resistance of a liquid to flow?
A) surface tension
B) capillary action
C) viscosity
D) adhesion
E) cohesion
20) Which of the following statements is true?
A) The higher the viscosity, the faster a liquid flows.
B) The viscosity increases with increasing temperature.
C) The stronger the intermolecular forces, the higher the viscosity.
D) Hydrogen bonding in water gives rise to its unusually low viscosity.
E) The viscosity of gases is larger than the viscosity of liquids.
21) Place the substances in order of increasing viscosity.CH3OH C2H6 HO-CH2CH2-OH
A) C2H6 < HO-CH2CH2-OH < CH3OH
B) CH3OH< C2H6 < HO-CH2CH2-OH
C) HO-CH2CH2-OH< C2H6 < CH3OH
D) CH3OH < HO-CH2CH2-OH < C2H6
E) C2H6 < CH3OH < HO-CH2CH2-OH
22) Place the substances in order of increasing viscosity.CH3CH2CH2CH3 H2NCH2CH2NH2 CH3CH2CH2NH2
A) CH3CH2CH2CH3 < CH3CH2CH2NH2 < H2NCH2CH2NH2
B) H2NCH2CH2NH2 < CH3CH2CH2NH2 < CH3CH2CH2CH3
C) H2NCH2CH2NH2 < CH3CH2CH2CH3 < CH3CH2CH2NH2
D) CH3CH2CH2CH3 < H2NCH2CH2NH2 < CH3CH2CH2NH2
E) CH3CH2CH2NH2 < H2NCH2CH2NH2 < CH3CH2CH2CH3
23) Which statement concerning the vapor pressures of water and methanol (CH3OH) is true?
A) At 25ºC, methanol has a higher vapor pressure than water because methanol has a lower normal boiling point than water.
B) At 25ºC, methanol has a higher vapor pressure than water because methanol is a poorer solvent than water.
C) At 25ºC, methanol has a higher vapor pressure than water because methanol is a less viscous liquid than water.
D) At 25ºC, methanol has a higher vapor pressure than water because the density of methanol is less than the density of water.
E) At 25ºC, methanol has a higher vapor pressure than water because methanol has weaker intermolecular forces than water.
24) Which of the following properties indicates the presence of strong intermolecular forces in a liquid?
A) a low heat of vaporization
B) a low critical temperature
C) a low vapor pressure
D) a low boiling point
E) a low melting point
25) Which corresponds to the temperature-dependent partial pressure above the surface of a liquid?
A) surface tension
B) vapor pressure
C) boiling point
D) viscosity
E) capillary action
26) If a molecule at the surface of a liquid has enough kinetic energy to escape the liquid phase and enter the gas phase, then which of the following terms is used to describe this phenomenon?
A) boiling point
B) condensation
C) vaporization
D) sublimation
E) gasification
27) Select the pair of substances in which the one with the higher vapor pressure at a given temperature is listed first.
A) C7H16, C5H12
B) CCl 4, CBr 4
C) H2O, H2S
D) CH3CH2OH, CH3–O–CH3
E) Xe, Kr
28) Which substance has the highest vapor pressure at room temperature?
A) HF
B) HCl
C) HBr
D) HI
E) All of these substances have the same vapor pressure at room temperature.
29) Which substance has the lowest vapor pressure at room temperature?
A) HF
B) HCl
C) HBr
D) HI
E) H 2
30) Select the pair of substances in which the one with the lower vapor pressure at a given temperature is listed first.
A)
B) PH3, NH3
C) CF4, CBr4
D) C3H8, C4H10
E) F2, Cl2
31) Place the substances in order of decreasing boiling point.CO2 CH4 OF2
A) OF2 > CO2 > CH4
B) CH4 > CO2 > OF2
C) OF2 > CH4 > CO2
D) CO2 > CH4 > OF2
E) CO2 > OF2 > CH4
32) Place the substances in order of decreasing boiling point.BeCl2 CBr4 BeBr2
A) BeCl2 > CBr4 > BeBr2
B) BeCl2 > BeBr2 > CBr4
C) CBr4 > BeBr2 > BeCl2
D) BeBr2 > BeCl2 > CBr4
33) Place the substances in order of increasing boiling point.BF3 NF3 BeF2
A) NF3 < BF3 < BeF2
B) BF3 < NF3 < BeF2
C) NF3 < BeF2 < BF3
D) BeF2 < NF3 < BF3
E) BeF2 < BF3 < NF3
34) Place the substances in order of increasing boiling point.BeF2 SF2 Ar
A) BeF2 < SF2 < Ar
B) Ar < BeF2 < SF2
C) SF2 < Ar < BeF2
D) SF2 < BeF2 < Ar
E) Ar < SF2 < BeF2
35) What is the process in which molecules undergo a phase change directly from the solid phase to the gas phase?
A) deposition
B) sublimation
C) freezing
D) condensation
E) melting
36) What is the process in which molecules undergo a phase change directly from the gas phase to the solid phase?
A) deposition
B) sublimation
C) freezing
D) condensation
E) melting
37) What is the process in which molecules undergo a phase change from the liquid phase to the gas phase?
A) vaporization
B) condensation
C) freezing
D) melting
E) sublimation
38) What is the process in which molecules undergo a phase change from the gas phase to the liquid phase?
A) vaporization
B) condensation
C) freezing
D) melting
E) sublimation
39) What is the process in which molecules undergo a phase change from the liquid phase to the solid phase?
A) vaporization
B) condensation
C) freezing
D) melting
E) sublimation
40) What is the process in which molecules undergo a phase change from the solid phase to the liquid phase?
A) vaporization
B) condensation
C) freezing
D) melting
E) sublimation
41) The specific heat (capacity) is
A) amount of energy needed to change 1 g of a substance by 1°C.
B) amount of energy needed to change 1 mol of a substance by 1°C
C) amount of energy required to melt 1 g of substance.
D) amount of substance that is heated by 1°C.
E) the temperature increase, in K, associated with heating 1 g of a substance for 1 minute.
42) What is q if 28.6 g of water is heated from 22.0°C to 78.3°C?The specific heat of water is 4.184 J/g·°C.
A) 2.60 J
B) 2.63 kJ
C) 6.74 kJ
D) 9.37 kJ
E) 3.94×104 kJ
43) If, as a pioneer, you wished to warm your room by taking an object heated on top of a pot-bellied stove to it, which of the following 15-pound objects, each heated to 100°C, would be the best choice? The specific heat capacity (in J/g·°C) for each substance is given in parentheses. Iron (0.450), copper (0.387), granite (0.79), gold (0.129), water (4.184).
A) iron
B) copper
C) granite
D) gold
E) H2O
44) Ethylene glycol, used as a coolant in automotive engines, has a specific heat capacity of 2.42 J/g·°C. Calculate q when 3.65 kg of ethylene glycol is cooled from 132°C to 85°C.
A) −1900 kJ
B) −420 kJ
C) −99 kJ
D) −0.42 kJ
E) −4.2 × 10−6 kJ
45) If 75.4 J of energy is absorbed by 0.25 mol of CCl4 at constant pressure, what is the change in temperature? The specific heat of CCl4 is 0.861 J/g·°C.
A) 17.8°C
B) 21.9°C
C) 2.3°C
D) 9.1°C
E) 44.6°C
46) A 275-g sample of nickel at l00.0°C is placed in 100.0 g of water at 22.0°C. What is the final temperature of the water? Assume no heat transfer with the surroundings. The specific heat of nickel is 0.444 J/g·°C and the specific heat of water is 4.184 J/g·°C.
A) 39.6°C
B) 40.8°C
C) 61.0°C
D) 79.2°C
E) 82.4°C
47) Benzene is a starting material in the synthesis of nylon fibers and polystyrene (styrofoam). Its specific heat capacity is 1.74 J/g·°C. If 16.7 kJ of energy is absorbed by a 225-g sample of benzene at 20.0°C, what is its final temperature?
A) −22.7°C
B) 37.7°C
C) 42.7°C
D) 62.7°C
E) 80.1°C
48) When Karl Kaveman adds chilled grog to his new granite mug, he removes 10.9 kJ of energy from the mug. If it has a mass of 625 g and was at 25°C, what is its new temperature? Specific heat capacity of granite = 0.79 J/g·°C.
A) 3°C
B) 14°C
C) 22°C
D) 47°C
E) None of the answers is correct.
49) How much heat is required to raise the temperature of 22.8 g of copper from 20.0°C to 875.0°C? The specific heat of copper is 0.385 J/g·°C.
A) 14.4 J
B) 176 J
C) 7.51 kJ
D) 7.68 kJ
E) 9.90 kJ
50) How much heat is required to raise the temperature of 12.0 g of water from 15.4°C to 93.0°C? The specific heat of water is 4.184 J/g·°C.
A) 223 J
B) 773 J
C) 503 J
D) 4.67 ×103 J
E) 3.90 ×103 J
51) How much heat is required to raise the temperature of 1500 g of water from 25°C to 52°C? The specific heat of water is 4.184 J/g·°C.
A) 1500 kJ
B) 170 kJ
C) 6.3 kJ
D) 41 J
E) 41 kJ
52) What is the change in temperature if a 25.0-g block of aluminum absorbs 10.0 kJ of heat? The specific heat of aluminum is 0.900 J/g·°C.
A) 0.44°C
B) 22.5°C
C) 225°C
D) 360°C
E) 444°C
53) If 325 g of water at 4.2°C absorbs 12.28 kJ, what is the final temperature of the water? The specific heat of water is 4.184 J/g·°C.
A) 4.21°C
B) 4.8°C
C) 9.0°C
D) 13.2°C
E) 2938°C
54) A glass containing 200.0 g of H2O at 20.0°C was placed in a refrigerator. The water loses 11.7 kJ as it cools to a constant temperature. What is its new temperature? The specific heat of water is 4.184 J/g·°C.
A) 0.0°C
B) 4.0°C
C) 6.0°C
D) 14.0°C
E) 34.0°C
55) A piece of copper with a mass of 218 g has a heat capacity of 83.9 J/°C. What is the specific heat of copper?
A) 0.385 J/g·°C
B) 1.83 × 104 J/g·°C
C) 2.60 J/g·°C
D) 1.32 J/g·°C
E) 24.5 J/g·°C
56) What is the energy in kJ/mol required to melt 1 mole of a solid?
A) molar heat of freezing
B) molar heat of fission
C) molar heat of vaporization
D) molar heat of fusion
E) molar heat of condensation
57) What quantity of heat is required to melt 2.00 kg of iron at its melting point (1809 K)? For iron, ΔHfus = 13.80 kJ/mol.
A) 0.385 kJ
B) 6.90 kJ
C) 27.6 kJ
D) 494 kJ
E) 771 kJ
58)
What mass of water would need to evaporate from your skin in order to dissipate 1.70 ×105 J of heat from the surface of your body? |
H2O(l)→ H2O(g) ΔHvap = 40.7 kJ/mol |
A) 2.26 g
B) 4.18 g
C) 75.2 g
D) 4.18 ×103 g
E) 4.07 × 104 g
59) What amount of energy (heat) is required to warm a 65.0-g sample of liquid water from 25.0ºC to 96.5ºC? The specific heat capacity of water is 4.184 J/gºC.
A) 4.60 J
B) 1.11 × 103 J
C) 2.62 × 104 J
D) 1.94 ×104 J
E) 1.61 J
60) What amount of energy (heat) is required to warm a 73.5-g sample of liquid ethanol from 15.0ºC to 29.5ºC? The specific heat capacity of ethanol is 2.46 J/gºC.
A) 0.485 J
B) 433 J
C) 2.62 × 103 J
D) 5.33 × 103 J
E) 238 J
61) The temperature of an 86.4-g piece of an unknown metal increases by 29.4ºC when 1.94 kJ of heat energy is added. Determine the specific heat capacity of the metal.
A) 4.93 J/gºC
B) 1.31 J/gºC
C) 0.764 J/gºC
D) 0.491 J/gºC
E) 0.131 J/gºC
62) The temperature of a 159-g piece of an unknown metal increases by 43.4ºC when 6.88 kJ of heat energy is added.Determine the specific heat capacity of the metal.
A) 10.0 J/gºC
B) 4.75 J/gºC
C) 0.338 J/gºC
D) 0.211 J/gºC
E) 0.997 J/gºC
Document Information
Connected Book
MCQ Test Bank | Introductory Chemistry - 2nd Edition by Burdge and Driessen
By Julia Burdge, Michelle Driessen