Question 1

Which of the following compounds is most likely to be insoluble in water?

Accepted Answer

BaSO\_4

Question 2

When solutions of AgNO\_3 and NaCl are mixed, what is the precipitate formed?

Accepted Answer

AgCl

Question 3

Given the solubility product constant $$K_{sp}$$ for CaF\_2 is $$4.0 	imes 10$$^{-11}$$, what is the molar solubility of CaF\_2 in pure water?

Accepted Answer

$$2.5 	imes 10$$^{-6}$$ M

Question 4

A solution is prepared by dissolving PbCl\_2 in water. If the $$K_{sp} of $$PbCl\_2 is $$1.7 	imes 10$$^{-5}$$, what is the concentration of Cl\^- ions at equilibrium?

Accepted Answer

$$2x$$ where $$x = \sqrt{K_{sp}/2}$$

Question 5

Which of the following actions will increase the solubility of Fe(OH)\_3 in water?

Accepted Answer

Adding HCl

Question 6

If solutions of Ba(NO\_3)\_2 and Na\_2SO\_4 are mixed, will a precipitate form? Why?

Accepted Answer

Yes, because BaSO\_4 is insoluble.

Question 7

Which of the following is a spontaneous process?

Accepted Answer

Iron rusting in moist air

Question 8

Which statement best explains the connection between disorder (randomness) and spontaneity?

Accepted Answer

Spontaneous processes tend to increase the disorder of the universe.

Question 9

Which phase change results in the greatest increase in entropy?

Accepted Answer

Sublimation of dry ice (CO\_2(s) to CO\_2(g))

Question 10

Consider the reaction: $$2H_2O_2 \rightarrow 2H_2O + O_2$. What is the qualitative change in entropy ($$\Delta S$$)?

Accepted Answer

$$\Delta S$$ increases because a gas is produced.

Question 11

State the Second Law of Thermodynamics and its importance.

Accepted Answer

The entropy of the universe always increases in a spontaneous process.

Question 12

What is a 'microstate' in thermodynamics?

Accepted Answer

A single possible arrangement of the positions and energies of the particles in a system.

Question 13

How does $$\Delta S_{sys}$$ and $$\Delta S_{surr}$$ depend on temperature?

Accepted Answer

$$\Delta S_{surr} is $$inversely proportional to temperature.

Question 14

Given $$\Delta H = -100 kJ $$and $$\Delta S = -200 J/K$$, at what temperature is the reaction spontaneous?

Accepted Answer

At low temperatures

Question 15

Calculate $$\Delta S^\circ$$ for the reaction: $$N_2(g) + 3H_2(g$$) \rightarrow 2NH_3(g)$$ given S$$^\circ($$N_2) = 192$ J/mol·K, S$$^\circ($$H_2) = 130$ J/mol·K, S$$^\circ($$NH_3) = 206$ J/mol·K.

Accepted Answer

$$\Delta S^\circ = -198 J/$$mol·K

Question 16

State the Third Law of Thermodynamics and its significance.

Accepted Answer

The entropy of a perfect crystal at absolute zero is zero.

Question 17

Given $$\Delta G^\circ = -30 kJ/$$mol, what is the equilibrium constant $$K_{eq} at 298 K$$? (Use $$\Delta G^\circ = -RT \ln K_{eq}$$, $$R = 8.314 J/$$mol·K)

Accepted Answer

$$K_{eq} \approx 1 	imes 10^5$

Question 18

Which of the following is an example of oxidation?

Accepted Answer

Zn losing electrons to become Zn\^{2+}

Question 19

Assign the oxidation number to sulfur in $$SO_4$$^{2-}$$.

Accepted Answer

+6

Question 20

Which metal will react with HCl to produce hydrogen gas?

Accepted Answer

Zinc (Zn)

Solubility, Thermodynamics, and Electrochemistry: Study Guide

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