19) Dinitrogen tetroxide partially decomposes according to the following equilibrium: N204 (g) 2NO2 (g) Initially, a 1.000-L flask is charged with 3.20 x 10-2 mol of N204. At equilibrium, 2.54 x 10-2 mol of N204 remains. Keq for this reaction is.
19) Dinitrogen tetroxide partially decomposes according to the following equilibrium: N204 (g) 2NO2 (g) Initially, a 1.000-L flask is charged with 3.20 x 10-2 mol of N204. At equilibrium, 2.54 x 10-2 mol of N204 remains. Keq for this reaction is.
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![**Equilibrium of Dinitrogen Tetroxide Decomposition**
Dinitrogen tetroxide \((\text{N}_2\text{O}_4)\) partially decomposes in a gas-phase equilibrium reaction as follows:
\[
\text{N}_2\text{O}_4(g) \rightleftharpoons 2\text{NO}_2(g)
\]
**Initial Conditions:**
- A 1.000-L flask is initially charged with \(3.20 \times 10^{-2} \text{ mol}\) of \(\text{N}_2\text{O}_4\).
**Equilibrium Conditions:**
- At equilibrium, \(2.54 \times 10^{-2} \text{ mol}\) of \(\text{N}_2\text{O}_4\) remains.
**Objective:**
- Determine the equilibrium constant, \(\text{K}_{eq}\), for the reaction.
**Options:**
A) \(6.86 \times 10^{-3}\)
B) \(1.72 \times 10^{-3}\)
C) 0.260
D) 0.520
E) 1.66
Select the correct \(\text{K}_{eq}\) value from the options provided based on the information given.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F04b28093-4f77-4d69-adb9-9e4a8e9f1bf0%2Ff35f7994-a3db-4327-a865-35674b58a267%2Fhn5gzg6_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Equilibrium of Dinitrogen Tetroxide Decomposition**
Dinitrogen tetroxide \((\text{N}_2\text{O}_4)\) partially decomposes in a gas-phase equilibrium reaction as follows:
\[
\text{N}_2\text{O}_4(g) \rightleftharpoons 2\text{NO}_2(g)
\]
**Initial Conditions:**
- A 1.000-L flask is initially charged with \(3.20 \times 10^{-2} \text{ mol}\) of \(\text{N}_2\text{O}_4\).
**Equilibrium Conditions:**
- At equilibrium, \(2.54 \times 10^{-2} \text{ mol}\) of \(\text{N}_2\text{O}_4\) remains.
**Objective:**
- Determine the equilibrium constant, \(\text{K}_{eq}\), for the reaction.
**Options:**
A) \(6.86 \times 10^{-3}\)
B) \(1.72 \times 10^{-3}\)
C) 0.260
D) 0.520
E) 1.66
Select the correct \(\text{K}_{eq}\) value from the options provided based on the information given.
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