Consider the reaction between NO2 and N2O4 in a closed
Chapter 15, Problem 121AP(choose chapter or problem)
Consider the reaction between \(\mathrm{NO}_2\) and \(\mathrm{N}_2 \mathrm{O}_4\) in a closed container:
\(\mathrm{N}_2 \mathrm{O}_4(\mathrm{~g}) \rightleftarrows 2 \mathrm{NO}_2(\mathrm{~g})\)
Initially, 1 mole of \(\mathrm{N}_2 \mathrm{O}_4\) is present. At equilibrium, x mole of \(\mathrm{N}_2 \mathrm{O}_4\) has dissociated to form \(\mathrm{NO}_2\).
(a) Derive an expression for \(K_P\) in terms of x and P, the total pressure.
(b) How does the expression in part (a) help you predict the shift in equilibrium due to an increase in P? Does your prediction agree with Le Châtelier's principle?
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