All a snowbound skier had to cat were walnuts! He was carrying a bag holding 12 dozen nuts. With his mittened hands, he cracked open the shells. Each nut that was opened resulted in one kernel and two shell halves. When he tired of the cracking and got ready to do some eating, he discovered he had 194 total pieces (whole nuts, shell halves, and kernels). What is the $K_{\text {eq }}$ for this reaction?

At a certain temperature, $K_{\text {eq }}$ is $2.2 \times 10^{-3}$ for the reaction $2 \mathrm{~ICl}(g) \rightleftharpoons \mathrm{I}_2(g)+\mathrm{Cl}_2(g)$ Now calculate the $K_{\text {eq }}$ value for the reaction

$$\mathrm{I}_2(g)+\mathrm{Cl}_2(g) \rightleftharpoons 2 \mathrm{~ICl}(g)$$

Reactants $\mathrm{A}$ and $\mathrm{B}$ are mixed, cach initially at a concentration of $1.0~M$. They react to produce $\mathrm{C}$ according to this cquation:

$$2 \mathrm{~A}+\mathrm{B} \rightleftharpoons \mathrm{C}$$

When equilibrium is established, the concentration of $\mathrm{C}$ is found to be $0.30~M$. Calculate the value of $K_{\text {eq }}$.

For the following equations, tell in which direction, left or right, the equilibrium will shift when these changes are made: The temperature is increased, the pressure is increased by decreasing the volume of the reaction vessel, and a catalyst is added.

(a) $2 \mathrm{~SO}_3(g)+197 \mathrm{~kJ} \rightleftharpoons 2 \mathrm{~SO}_2(g)+\mathrm{O}_2(g)$
(b) $4 \mathrm{~NH}_3(g)+3 \mathrm{~O}_2(g) \rightleftharpoons 2 \mathrm{~N}_2(g)+6 \mathrm{~H}_2 \mathrm{O}(g)+1531 \mathrm{~kJ}$
(c) $\mathrm{OF}_2(g)+\mathrm{H}_2 \mathrm{O}(g) \rightleftharpoons \mathrm{O}_2(g)+2 \mathrm{~HF}(g)+318 \mathrm{~kJ}$

Determine the $\mathrm{pH}$ for the following solutions:

(a) $5.0 \times 10^{-5}~M\mathrm{~HNO}_3$
(b) $2.0 \times 10^{-6}~M\mathrm{~KOH}$

Write the equilibrium constant expressions for these reactions:

(a) $3 \mathrm{O}_2(g) \rightleftharpoons 2 \mathrm{O}_3(g)$
(b) $\mathrm{H}_2 \mathrm{O}(g) \rightleftharpoons \mathrm{H}_2 \mathrm{O}(l)$
(c) $\mathrm{MgCO}_3(s) \rightleftharpoons \mathrm{MgO}(s)+\mathrm{CO}_2(g)$
(d) $2 \mathrm{~Bi}^{3+}(a q)+3 \mathrm{~H}_2 \mathrm{~S}(a q) \rightleftharpoons \mathrm{Bi}_2 \mathrm{S}_3(s)+6 \mathrm{~H}^{+}(a q)$

For the reaction $\mathrm{CO}(\mathrm{g})+\mathrm{H}_2 \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{CO}_2(\mathrm{~g})+\mathrm{H}_2(\mathrm{~g})$ at a certain temperature, $K_{\text {eq }}$ is 1 . At cquilibrium would you cxpect to find

(a) only $\mathrm{CO}$ and $\mathrm{H}_2$
(b) mostly $\mathrm{CO}_2$ and $\mathrm{H}_2$
(c) about equal concentrations of $\mathrm{CO}$ and $\mathrm{H}_2 \mathrm{O}$, compared to $\mathrm{CO}_2$ and $\mathrm{H}_2$
(d) mostly $\mathrm{CO}$ and $\mathrm{H}_2 \mathrm{O}$ (e) only $\mathrm{CO}$ and $\mathrm{H}_2 \mathrm{O}$ Explain your answer briefly.

One day in a laboratory, some water spilled on a table. In just a few minutes the water had evaporated. Some days later, a similar amount of water spilled again. This time, the water remained on the table after 7 or 8 hours. Name three conditions that could have changed in the lab to cause this difference.

Under certain circumstances, when oxygen gas is heated, it can be converted into ozone according to the following reaction equation:

$$3 \mathrm{O}_2(g)+\text { heat } \rightleftharpoons 2 \mathrm{~O}_3(g)$$

Name three different ways that you could increase the production of the ozone.

The solubility of $\mathrm{Hg}_2 \mathrm{I}_2$ in $\mathrm{H}_2 \mathrm{O}$ is $3.04 \times 10^{-7} \mathrm{~g} / \mathrm{L}$. The reaction $\mathrm{Hg}_2 \mathrm{I}_2 \rightleftharpoons \mathrm{Hg}_2^{2+}+2 \mathrm{~I}^{-}$represents the equilibrium. Calculate the $K_{\text {sp }}$.

The $K_{s p}$ of $\mathrm{SrSO}_4$ is $7.6 \times 10^{-7}$. Should precipitation occur when $25.0 \mathrm{~mL}$ of $1.0 \times 10^{-3} \mathrm{M} \mathrm{SrCl}_2$ solution are mixed with $15.0 \mathrm{~mL}$ of $2.0 \times 10^{-3}~M\mathrm{~Na}_2 \mathrm{SO}_4$ ? Show proof.

The $K_{\text {eq }}$ for the formation of ammonia gas from its elements is 4.0. If the equilibrium concentrations of nitrogen gas and hydrogen gas are both $2.0~M$, what is the equilibrium concentration of the ammonia gas?

If it takes $0.048 \mathrm{~g} \mathrm{~BaF}_2$ to saturate $15.0 \mathrm{~mL}$ of water, what is the $K_{s p}$ of $\mathrm{BaF}_2$ ?

Of the acids listed in Table 16.2, which ones are stronger than acetic acid and which are weaker?