---
title: "The dissociation of dinitrogen tetroxide gas is represented by the following equation:  \\[ \\text{N}_2\\text{O}_4\\text{(g)} \\rightleftharpoons 2\\,\\text{NO}_2\\text{(g)} \\quad \\Delta G^	circ_{298} = +4.8\\text{ kJ/mol}_{\\text{rxn}} \\]  At \\(298\\text{ K}\\), the equilibrium constant \\(K_p\\) for the reaction is approximately \\(0.14\\). A rigid, evacuated reaction vessel at \\(298\\text{ K}\\) is charged with \\(\\text{N}_2\\text{O}_4\\text{(g)}\\) at a partial pressure of \\(1.0\\text{ atm}\\) and \\(\\text{NO}_2\\text{(g)}\\) at a partial pressure of \\(0.010\\text{ atm}\\).  Which of the following statements best describes the initial thermodynamic favorability of the forward reaction and provides the correct justification?"
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url: "https://nerd-notes.com/ubq/120335/"
date_modified: "2026-08-23T04:23:12+00:00"
---

# The dissociation of dinitrogen tetroxide gas is represented by the following equation:

\[ \text{N}_2\text{O}_4\text{(g)} \rightleftharpoons 2\,\text{NO}_2\text{(g)} \quad \Delta G^	circ_{298} = +4.8\text{ kJ/mol}_{\text{rxn}} \]

At \(298\text{ K}\), the equilibrium constant \(K_p\) for the reaction is approximately \(0.14\). A rigid, evacuated reaction vessel at \(298\text{ K}\) is charged with \(\text{N}_2\text{O}_4\text{(g)}\) at a partial pressure of \(1.0\text{ atm}\) and \(\text{NO}_2\text{(g)}\) at a partial pressure of \(0.010\text{ atm}\).

Which of the following statements best describes the initial thermodynamic favorability of the forward reaction and provides the correct justification?

The dissociation of dinitrogen tetroxide gas is represented by the following equation:

\[ \text{N}_2\text{O}_4\text{(g)} \rightleftharpoons 2\,\text{NO}_2\text{(g)} \quad \Delta G^	circ_{298} = +4.8\text{ kJ/mol}_{\text{rxn}} \]

At \(298\text{ K}\), the equilibrium constant \(K_p\) for the reaction is approximately \(0.14\). A rigid, evacuated reaction vessel at \(298\text{ K}\) is charged with \(\text{N}_2\text{O}_4\text{(g)}\) at a partial pressure of \(1.0\text{ atm}\) and \(\text{NO}_2\text{(g)}\) at a partial pressure of \(0.010\text{ atm}\).

Which of the following statements best describes the initial thermodynamic favorability of the forward reaction and provides the correct justification?

- **A.** The forward reaction is not thermodynamically favorable because \(\Delta G^\circ > 0\), which indicates that the reaction cannot proceed spontaneously in the forward direction under any set of partial pressures.
- **B.** The forward reaction is not thermodynamically favorable because \(Q_p < K_p\), which requires the consumption of products to shift the reaction toward reactants to reach equilibrium.
- **C.** The forward reaction is thermodynamically favorable because \(\Delta G^\circ > 0\) ensures that the reaction quotient \(Q_p\) must increase until it reaches a value of \(1.0\).
- **D.** The forward reaction is thermodynamically favorable because \(Q_p < K_p\), which results in \(\Delta G < 0\) and drives the net conversion of reactants to products until equilibrium is reached.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/120335/*