Chapter 14

Write the equilibrium law for each of the following gas phase reactions in terms of molar concentrations. (a) \(3 \mathrm{Cl}_{2}(g)+\mathrm{NH}_{3}(g) \rightleftharpoons \mathrm{NCl}_{3}(g)+3 \mathrm{HCl}(g)\) (b) \(\mathrm{PCl}_{3}(g)+\mathrm{PBr}_{3}(g) \rightleftharpoons \mathrm{PCl}_{2} \operatorname{Br}(g)+\mathrm{PClBr}_{2}(g)\) (c) \(\mathrm{NO}(g)+\mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons 2 \mathrm{HNO}_{2}(g)\) (d) \(\mathrm{H}_{2} \mathrm{O}(g)+\mathrm{Cl}_{2} \mathrm{O}(g) \rightleftharpoons 2 \mathrm{HOCl}(g)\) (e) \(\mathrm{Br}_{2}(g)+5 \mathrm{~F}_{2}(g) \rightleftharpoons 2 \mathrm{BrF}_{5}(g)\)

Write the equilibrium law for the following reactions in aqueous solution. (a) \(\mathrm{Ag}^{+}(a q)+2 \mathrm{NH}_{3}(a q) \rightleftharpoons \mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}(a q)\) (b) \(\mathrm{Cd}^{2+}(a q)+4 \mathrm{SCN}^{-}(a q) \rightleftharpoons \mathrm{Cd}(\mathrm{SCN})_{4}^{2-}(a q)\)

Write the equilibrium law for the following reactions in aqueous solution. $$ \begin{array}{l} \text { (a) } \mathrm{HClO}(a q)+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{3} \mathrm{O}+(a q)^{+} \mathrm{ClO}^{-}(a q) \\ \text { (b) } \mathrm{CO}_{3}^{2-}(a q)+\mathrm{HSO}^{-}(a q) \rightleftharpoons \\ \mathrm{HCO}_{3}^{-}(a q)+\mathrm{SO}_{4}^{2-}(a q) \end{array} $$

Use the following equilibria $$ \begin{aligned} 2 \mathrm{CH}_{4}(g) & \rightleftharpoons \mathrm{C}_{2} \mathrm{H}_{6}(g)+\mathrm{H}_{2}(g) & K_{\mathrm{c}} &=9.5 \times 10^{-13} \\ \mathrm{CH}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(g) & \rightleftharpoons \mathrm{CH}_{3} \mathrm{OH}(g)+\mathrm{H}_{2}(g) K_{\mathrm{c}} &=2.8 \times 10^{-21} \end{aligned} $$ to calculate \(K_{\mathrm{c}}\) for the reaction $$ 2 \mathrm{CH}_{3} \mathrm{OH}(g)+\mathrm{H}_{2}(g) \rightleftharpoons \mathrm{C}_{2} \mathrm{H}_{6}(g)+2 \mathrm{H}_{2} \mathrm{O}(g) $$

Write the equilibrium law for each of the following reactions in terms of molar concentrations: (a) \(\mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons 2 \mathrm{HCl}(g)\) (b) \(\frac{1}{2} \mathrm{H}_{2}(g)+\frac{1}{2} \mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{HCl}(g)\) How does \(K_{\mathrm{c}}\) for reaction (a) compare with \(K_{\mathrm{c}}\) for reaction (b)?

A \(345 \mathrm{~mL}\) vessel contains \(\mathrm{NH}_{3}\) at a pressure of 745 torr and a temperature of \(45^{\circ} \mathrm{C}\). What is the molar concentration of ammonia in the container?

For which of the following reactions does \(K_{\mathrm{P}}=K_{\mathrm{c}}\) ? (a) \(2 \mathrm{H}_{2}(g)+\mathrm{C}_{2} \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{C}_{2} \mathrm{H}_{6}(g)\) (b) \(\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g)\) (c) \(2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g)\)

Calculate the molar concentration of water in (a) \(18.0 \mathrm{~mL}\) of \(\mathrm{H}_{2} \mathrm{O}(l),\) (b) \(100.0 \mathrm{~mL}\) of \(\mathrm{H}_{2} \mathrm{O}(l),\) and \(\mathbf{( c )} 1.00 \mathrm{~L}\) of \(\mathrm{H}_{2} \mathrm{O}(l)\). Assume that the density of water is \(1.00 \mathrm{~g} / \mathrm{mL}\)

The density of sodium chloride is \(2.164 \mathrm{~g} \mathrm{~cm}^{-3}\). What is the molar concentration of \(\mathrm{NaCl}\) in a \(12.0 \mathrm{~cm}^{3}\) sample of pure \(\mathrm{NaCl}\) ? What is the molar concentration of \(\mathrm{NaCl}\) in a \(25.0 \mathrm{~g}\) sample of pure \(\mathrm{NaCl}\) ?

Write the equilibrium law corresponding to \(K_{c}\) for each of the following heterogeneous reactions. (a) \(2 \mathrm{C}(s)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{CO}(g)\) (b) \(2 \mathrm{NaHSO}_{3}(s) \rightleftharpoons \mathrm{Na}_{2} \mathrm{SO}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(g)+\mathrm{SO}_{2}(g)\) (c) \(2 \mathrm{C}(s)+2 \mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{CH}_{4}(g)+\mathrm{CO}_{2}(g)\) (d) \(\mathrm{CaCO}_{3}(s)+2 \mathrm{HF}(g) \rightleftharpoons \mathrm{C}_{2}(g)+\mathrm{CaF}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(g)\) (e) \(\mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O}(s) \rightleftharpoons \mathrm{CuSO}_{4}(s)+5 \mathrm{H}_{2} \mathrm{O}(g)\)