16.4 Exercise 10

Calculate ΔG° for each of the following reactions from the equilibrium constant at the temperature given.

(a) $\text{N}_{2} \left(g\right) + \text{O}_{2} \left(g\right) \rightarrow \text{2NO} \left(g\right) \text{T} = 2000 °\text{C} K_{p} = 4.1 \times 10^{−\text{4}}$

(b) $\text{H}_{2} \left(g\right) + \text{I}_{2} \left(g\right) \rightarrow \text{2HI} \left(g\right) \text{T} = 400 °\text{C} K_{p} = 50.0$

(c) $\text{CO}_{2} \left(g\right) + \text{H}_{2} \left(g\right) \rightarrow \text{CO} \left(g\right) + \text{H}_{2} \text{O} \left(g\right) \text{T} = 980 °\text{C} K_{p} = 1.67$

(d) $\text{CaCO}_{3} \left(s\right) \rightarrow \text{CaO} \left(s\right) + \text{CO}_{2} \left(g\right) \text{T} = 900 °\text{C} K_{p} = 1.04$

(e) $\text{HF} \left(a q\right) + \text{H}_{2} \text{O} \left(l\right) \rightarrow \text{H}_{3} \text{O}^{+} \left(a q\right) + \text{F}^{−} \left(a q\right) \text{T} = 25 °\text{C} K_{a} = 7.2 \times 10^{−\text{4}}$

(f) $\text{AgBr} \left(s\right) \rightarrow \text{Ag}^{+} \left(a q\right) + \text{Br}^{−} \left(a q\right) \text{T} = 25 °\text{C} K_{sp} = 3.3 \times 10^{−\text{13}}$