Solution Found!
The equilibrium constant (kp) for the reaction is 1.4 ×
Chapter 20, Problem 76P(choose chapter or problem)
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?
Questions & Answers
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.