1. Clicker Questions Chapters 13, 14, 15
Dana and Michelle Chatellier
University of Delaware

2. molecular weights shapes intermolecular attractive forces d. densities
The rule of “like dissolves like” refers to similarities between _______ of miscible liquids.
molecular weights
shapes
intermolecular attractive forces
d. densities
Answer: c

3. Which of the following compounds is miscible with water?
CH3OH
CH4
C6H6
d. CH3CH2OCH2CH3
Answer: a

4. Which of the compounds below is the LEAST miscible with water?
CH3OH
CH3CH2OH
CH3CH2CH2OH
d. CH3CH2CH2CH2OH
Answer: d

5. Boyle’s Charles’s Henry’s d. Raoult’s
_______ Law says that the solubility of a gas in a liquid increases as the pressure of the gas increases.
Boyle’s
Charles’s
Henry’s
d. Raoult’s
Answer: c

6. Boyle’s Charles’s Henry’s d. Raoult’s
_______ Law says that the vapor pressure of a solution is proportional to the mole fraction of the solvent.
Boyle’s
Charles’s
Henry’s
d. Raoult’s
Answer: d

7. The molality of a solution is defined as the amount of solute (in moles) divided by the
volume of the solution (in liters).
mass of the solvent (in kilograms).
mass of the solution (in kilograms).
d. total number of moles.
Answer: b

8. increases. decreases. remains unchanged. d. varies from gas to gas.
In general, as the temperature of a solution increases, the solubility of a gaseous solute
increases.
decreases.
remains unchanged.
d. varies from gas to gas.
Answer: b

9. –3.72 degrees C –1.86 degrees C +1.86 degrees C d. +3.72 degrees C
What is the freezing point of a 2.00 m aqueous solution of sucrose? The value of Kf for water is 1.86 degrees C/molal.
–3.72 degrees C
–1.86 degrees C
+1.86 degrees C
d degrees C
Answer: a

10. What is the vapor pressure of a solution containing 0
What is the vapor pressure of a solution containing mol of glucose and mol of water at 29 degrees C?
29°C =
30.04 torr
30.0 Torr
27.3 Torr
25.0 Torr
d Torr
Answer: b

11. A 0.100 molal solution of which compound below will have the lowest freezing point?
NaCl
CaCl2 KI
d. LiNO3
Answer: b

12. 180 g/mole b. 360 g/mole c. 720 g/mole d. 1800 g/mole
What is the molecular weight of adrenaline if 0.64 grams of adrenaline dissolved in 36.0 g of CCl4 raises the boiling point by 0.49 degrees Celsius?
Kb=
4.95 °C/m
Answer: a
180 g/mole b g/mole
c g/mole d g/mole

13. Tyndall Raoult Hall d. Meissner
Light scattering by colloidally dispersed particles is an example of the _______ effect.
Tyndall
Raoult
Hall
d. Meissner
Answer: a

14. The rate of a reaction can be increased by
increasing reactant concentrations.
increasing the temperature.
adding a suitable catalyst.
d. All of the above
Answer: d

15. Over time, the rate of most chemical reactions tends to _______.
increase
decrease
remain constant
d. oscillate
Answer: b

16. zeroth first second d. third
If tripling the concentration of reactant A multiplies the rate by a factor of nine, the reaction is _______ order in A.
zeroth
first
second
d. third
Answer: c

17. first. second. third. d. fourth.
Reaction: A + B  C + D Rate = k[A][B] The overall order of this reaction is
first.
second.
third.
d. fourth.
Answer: b

18. zeroth. first. second. d. third.
Reaction: W + X  Y + Z Rate = k[W] The order of this reaction with respect to X is
zeroth.
first.
second.
d. third.
Answer: a

19. The time required for the concentration of a reactant to be reduced to half of its initial value is called the
midpoint of the reaction.
equivalence point of the reaction.
half-rate of the reaction.
d. half-life of the reaction.
Answer: d

20. If k is the rate constant of a first-order reaction, the half-life of the reaction is:
d. 2k
Answer: a

21. 10 seconds 69 seconds 100 seconds d. 690 seconds
The value of the rate constant (k) for a first-order reaction is sec–1. What is the half-life of this reaction?
10 seconds
69 seconds
100 seconds
d. 690 seconds
Answer: b

22. 69 seconds 138 seconds 460 seconds d. 690 seconds
A + B  products, Rate = k[A], k = sec–1, Initial [A] = .100 M, Final [A] = M How long will this take?
69 seconds
138 seconds
460 seconds
d. 690 seconds
Answer: c

23. 69 seconds 138 seconds 460 seconds d. 690 seconds
Rate = k[A]2, Initial [A] = M, k = M–1 sec–1 What is the half-life of this second-order reaction?
69 seconds
138 seconds
460 seconds
d. 690 seconds
Answer: c

24. Rate = k[A]2, Initial [A] = 0. 100 M, k = 0. 0214 M–1 sec–1 After 1
Rate = k[A]2, Initial [A] = M, k = M–1 sec–1 After 1.00 hour, what is the concentration of reactant A? M M M
d M
Answer: d

25. The minimum energy that a collision between molecules must have for a reaction to occur is called the
initial energy.
internal energy.
external energy.
d. energy of activation.
Answer: d

26. 100 kJ/mole. 310 kJ/mole. 690 kJ/mole. d. 1000 kJ/mole.
At 298 K, k = 1.36  10–7 sec–1. At 323 K, k = 2.72  10–6 sec–1. The energy of activation for this reaction is
100 kJ/mole.
310 kJ/mole.
690 kJ/mole.
d kJ/mole.
Answer: a

27. The rate-determining step is the _______ step in a reaction mechanism.
first
last
c. fastest
d. slowest
Answer: d

28. Adding a catalyst increases the rate of a chemical reaction because the presence of the catalyst
increases molecular velocities.
increases molecular collisions.
decreases energy of activation.
d. All of the above
Answer: c

29. equal to slower than faster than d. the reverse of
At equilibrium, the rate of the forward reaction is _______ the rate of the reverse reaction.
equal to
slower than
faster than
d. the reverse of
Answer: a

30. The reaction quotient Q is usually represented by
[reactants] / [products].
[products] / [reactants].
[reactants]  [products].
d. [reactants] + [products].
Answer: b

31. reactants products catalysts d. shrapnel
If the value of the equilibrium constant is large, then _______ will mostly be present at equilibrium.
reactants
products
catalysts
d. shrapnel
Answer: b

32. reactants products catalysts d. shrapnel
If the value of the equilibrium constant is small, then _______ will mostly be present at equilibrium.
reactants
products
catalysts
d. shrapnel
Answer: a

33. Q = the reaction quotient K = the equilibrium constant At equilibrium, which is true?
Q > K
Q < K
Q = K
d. Q2 = K
Answer: c

34. Equilibrium constants typically have units of
d. None of the above
Answer: d

35. pure liquids. pure solids. Both of the above d. Neither of the above
Reaction quotients for heterogeneous equilibria do not include concentrations of
pure liquids.
pure solids.
Both of the above
d. Neither of the above
Answer: c

36. HA ⇋ H+ + A– [HA] = 1. 65  10–2 M and [H+] = [A–] = 5
HA ⇋ H+ + A– [HA] = 1.65  10–2 M and [H+] = [A–] = 5.44  10–4 M at equilibrium. Kc = _______.
1.79  10–2
1.79  10–3
1.79  10–4
d  10–5
Answer: d

37. KP = KC when the reaction is at equilibrium.
the reaction is exothermic.
all of the gases present are at the same pressure.
d. the number of moles of gas on both sides of the balanced equation is the same.
Answer: d

38. increase. decrease. remain unchanged. d. disappear.
CO2 + H2 ⇋ CO + H2O If all species are gases and H2 is added, the concentration of CO at equilibrium will
increase.
decrease.
remain unchanged.
d. disappear.
Answer: a

39. CO2 + H2 ⇋ CO + H2O If all species are gases and H2O is added, the equilibrium concentration of CO
will increase.
will decrease.
will remain unchanged.
d. will disappear.
Answer: b

40. increase. decrease. remain unchanged. d. disappear.
CO2 + H2 ⇋ CO + H2O If all species are gases and CO2 is removed, the [CO] at equilibrium will
increase.
decrease.
remain unchanged.
d. disappear.
Answer: b

41. increase decrease not change d. eradicate
CO2 + H2 ⇋ CO + H2O Increasing the temperature of this endothermic reaction will _______ [CO] at equilibrium.
increase
decrease
not change
d. eradicate
Answer: a

42. increase. decrease. remain unchanged. d. vanish.
CO2 + H2 ⇋ CO + H2O If all species are gases and the container is compressed, the amount of CO will
increase.
decrease.
remain unchanged.
d. vanish.
Answer: c

43. increase. decrease. remain unchanged. d. cease to exist.
CO2 + H2 ⇋ CO + H2O Adding a catalyst to this reaction will cause the [CO] at equilibrium to
increase.
decrease.
remain unchanged.
d. cease to exist.
Answer: c