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The equilibrium constant (kp) for the reaction is 1.4 ×

Chapter 20, Problem 76P

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QUESTION:

The equilibrium constant \(\left(\mathrm{K}_{p}\right)\) for the reaction

              \(2\mathrm{CO}(g)+\mathrm{O}_2(g)\ \rightleftharpoons\ 2\mathrm{CO}_2(g)\)

is \(1.4 \times 10^{90}\) at \(25^{\circ} \mathrm{C}\). Given this enormous value, why doesn't CO convert totally to \(\mathrm{CO}_{2}\) in the troposphere?

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QUESTION:

The equilibrium constant \(\left(\mathrm{K}_{p}\right)\) for the reaction

              \(2\mathrm{CO}(g)+\mathrm{O}_2(g)\ \rightleftharpoons\ 2\mathrm{CO}_2(g)\)

is \(1.4 \times 10^{90}\) at \(25^{\circ} \mathrm{C}\). Given this enormous value, why doesn't CO convert totally to \(\mathrm{CO}_{2}\) in the troposphere?

ANSWER:

Step 1 of 2

Given reaction

The equilibrium constant  for the reaction is

We need to explain the reason for carbon monoxide not converting totally to carbon dioxide.

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