AP Chemistry
7.9 Introduction to Le Châtelier’s Principle
7.4 Calculating the Equilibrium Constant
7.3 Reaction Quotient and Equilibrium Constant
A sample of \(\text{N}_2\text{O}_4(g)\) is placed in a rigid, sealed container and allowed to decompose according to the equation below.
\[ \text{N}_2\text{O}_4(g) \rightleftharpoons 2\,\text{NO}_2(g) \]
The reaction is allowed to reach equilibrium at two different temperatures. The equilibrium partial pressures of each gas at both temperatures are recorded in the table below.
Based on the data, which of the following correctly identifies the sign of \(\Delta H^\circ\) for the forward reaction and provides the correct justification using the equilibrium constant, \(K_p\)?
\[ \text{N}_2\text{O}_4(g) \rightleftharpoons 2\,\text{NO}_2(g) \]
The reaction is allowed to reach equilibrium at two different temperatures. The equilibrium partial pressures of each gas at both temperatures are recorded in the table below.
| Temperature | \(P_{\text{N}_2\text{O}_4}\) (atm) | \(P_{\text{NO}_2}\) (atm) |
|---|---|---|
| \(300\text{ K}\) | \(4.0\) | \(2.0\) |
| \(400\text{ K}\) | \(0.50\) | \(4.0\) |
Based on the data, which of the following correctly identifies the sign of \(\Delta H^\circ\) for the forward reaction and provides the correct justification using the equilibrium constant, \(K_p\)?
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