?A mixture of 0.2000 mol of \(\mathrm{CO}_{2}\), 0.1000 mol of \(\mathrm{H}_{2}\), and

Chapter 15, Problem 15.37

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A mixture of 0.2000 mol of \(\mathrm{CO}_{2}\), 0.1000 mol of \(\mathrm{H}_{2}\), and 0.1600 mol  of \(\mathrm{H}_{2} \mathrm{O}\) is placed in a 2.000-L vessel. The following equilibrium is established at 500 K:

\(\mathrm{CO}_{2}(g)+\mathrm{H}_{2}(g) \rightleftharpoons \mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g)\)

(a) Calculate the initial partial pressures of \(\mathrm{CO}_{2}, \mathrm{H}_{2}\), and \(\mathrm{H}_{2} \mathrm{O}\).

(b) At equilibrium \(P_{\mathrm{H}_{2} \mathrm{O}}=3.51\) atm. Calculate the equilibrium partial pressures of \(\mathrm{CO}_{2}, \mathrm{H}_{2}\), and \(\mathrm{CO}\).

(c) Calculate \(K_{p}\) for the reaction.

(d) Calculate \(K_{c}\) for the reaction.

Text Transcription:

CO_2

H_2

H_2O

CO_2(g) + H2(g) \rightleftharpoons CO(g) + H_2O(g)

P_H2O = 3.51

K_p