AP Chemistry
7.10 Reaction Quotient and Le Châtelier’s Principle
7.3 Reaction Quotient and Equilibrium Constant
A student introduces \(\text{N}_2\text{O}_4\text{(g)}\) and \(\text{NO}_2\text{(g)}\) into a rigid, evacuated \(1.0 \text{ L}\) container at \(298 \text{ K}\). The reaction and its equilibrium constant at \(298 \text{ K}\) are represented below.
\[\text{N}_2\text{O}_4\text{(g)} \rightleftharpoons 2\text{ NO}_2\text{(g)} \quad K_c = 4.0 \times 10^{-2}\]
The initial concentration of \(\text{N}_2\text{O}_4\text{(g)}\) is \(0.10 \text{ M}\) and the initial concentration of \(\text{NO}_2\text{(g)}\) is \(0.20 \text{ M}\). Which of the following best predicts the direction in which the reaction will proceed to reach equilibrium, and provides the correct justification?
\[\text{N}_2\text{O}_4\text{(g)} \rightleftharpoons 2\text{ NO}_2\text{(g)} \quad K_c = 4.0 \times 10^{-2}\]
The initial concentration of \(\text{N}_2\text{O}_4\text{(g)}\) is \(0.10 \text{ M}\) and the initial concentration of \(\text{NO}_2\text{(g)}\) is \(0.20 \text{ M}\). Which of the following best predicts the direction in which the reaction will proceed to reach equilibrium, and provides the correct justification?
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