Edexcel A-Level Chemistry A2 13.9 Apply Knowledge of the Value of Equilibrium Constants to Predict the Extent to Which a Reaction Takes Place Questions

Describe very large K as equilibrium far to products and very small K as far to reactants, while treating moderate values as mixtures rather than complete conversion.

Exam points

Use a very large K value to justify that equilibrium lies far toward products.
Interpret a moderate K as appreciable reactant and product amounts rather than completion.

[Maximum number: 2]

This question is about the reaction between nitrogen monoxide and oxygen.

\mathrm{NO}(\mathrm{~g})+1 / 2 \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{NO}_{2}(\mathrm{~g})

The equilibrium constant, $K_{p}$ , for the reaction at 298 K is $1.55 \times 10^{6} \mathrm{~atm}^{-1 / 2}$ .

State what this value of the equilibrium constant indicates about the position of the equilibrium. Justify your answer.

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Edexcel A-Level Chemistry A2 13.9 Apply Knowledge of the Value of Equilibrium Constants to Predict the Extent to Which a Reaction Takes Place Questions question 1