5 Steps to a 5 AP Chemistry 2019

Take a Diagnostic Exam ‹ 23

51. The critical point on a phase diagram represents:

(A) the highest temperature and pressure where

a substance can sublime

(B) the highest temperature and pressure where

the substance may exist as discrete solid and

gas phases

(C) the temperature and pressure where the sub-

stance exists in equilibrium as solid, liquid,

and gas phases

(D) the highest temperature and pressure where

the substance may exist as discrete liquid

and gas phases

52. This explains why copper is ductile.

(A) London dispersion forces

(B) covalent bonding

(C) hydrogen bonding

(D) metallic bonding

53. This is why acetic acid, CH 3 COOH, molecules
    exist as dimers in the gaseous phase.
    (A) London dispersion forces
    (B) covalent bonding
    (C) hydrogen bonding
    (D) metallic bonding


54. For the following, pick the answer that most
    likely represents their relative solubilities in water.
    (A) CH 3 CH 2 CH 2 OH < HOCH 2 CH 2 OH
    < CH 3 CH 2 CH 2 CH 3
    (B) CH 3 CH 2 CH 2 CH 3 < HOCH 2 CH 2 OH
    < CH 3 CH 2 CH 2 OH
    (C) CH 3 CH 2 CH 2 CH 3 < CH 3 CH 2 CH 2 OH
    < HOCH 2 CH 2 OH
    (D) CH 3 CH 2 CH 2 OH < CH 3 CH 2 CH 2 CH 3
    < HOCH 2 CH 2 OH

Time

TemperatureA

B

C

D

E

55. The above diagram represents the heating curve
    for a pure crystalline substance. The solid is the
    only phase present up to point:
    (A) C
    (B) B
    (C) E
    (D) A


56. For all one-component phase diagrams, choose
    the correct statement from the following list.
    (A) The line separating the gas from the liquid
    phase may have a positive or negative slope.
    (B) The line separating the solid from the liquid
    phase may have a positive or negative slope.
    (C) The line separating the solid from the liquid
    phase has a positive slope.
    (D) The temperature at the triple point is the
    same as at the freezing point.

Chapter 13

57. A solution is prepared by dissolving 0.500 mol of
    NaCl in 500.0 g of water. Which of the follow-
    ing would be the best procedure to determine the
    molarity of the solution?
    (A) Measure the volume of the solution.
    (B) Titrate the solution with standard silver
    nitrate solution.
    (C) Determine the freezing point of the solution.
    (D) Determine the osmotic pressure of the
    solution.