AP Chemistry
7.7 Calculating Equilibrium Concentrations
7.4 Calculating the Equilibrium Constant
7.3 Reaction Quotient and Equilibrium Constant
A sample of \(\text{N}_2\text{O}_4\text{(g)}\) is placed into a rigid, evacuated container at a constant temperature. The system reaches equilibrium according to the following equation:
\[ \text{N}_2\text{O}_4\text{(g)} \rightleftharpoons 2\text{NO}_2\text{(g)} \]
The initial and equilibrium concentrations of the species are shown in the table below.
Based on the data in the table, what is the value of the equilibrium constant, \(K_c\), for the reaction at this temperature?
\[ \text{N}_2\text{O}_4\text{(g)} \rightleftharpoons 2\text{NO}_2\text{(g)} \]
The initial and equilibrium concentrations of the species are shown in the table below.
| Substance | Initial concentration (M) | Equilibrium concentration (M) |
|---|---|---|
| \(\text{N}_2\text{O}_4\text{(g)}\) | \(0.50\) | ? |
| \(\text{NO}_2\text{(g)}\) | \(0.00\) | \(0.20\) |
Based on the data in the table, what is the value of the equilibrium constant, \(K_c\), for the reaction at this temperature?
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