AP Chemistry
7.7 Calculating Equilibrium Concentrations
7.4 Calculating the Equilibrium Constant
A student introduces only \(\text{N}_2\text{O}_4\text{(g)}\) into an evacuated rigid container at a particular temperature. The system reaches equilibrium according to the following equation.
\(\text{N}_2\text{O}_4\text{(g)} \rightleftharpoons 2\text{NO}_2\text{(g)}\)
What is the value of \(K_c\) at this temperature for the reaction \(2\text{NO}_2\text{(g)} \rightleftharpoons \text{N}_2\text{O}_4\text{(g)}\)?
\(\text{N}_2\text{O}_4\text{(g)} \rightleftharpoons 2\text{NO}_2\text{(g)}\)
| Stage | \([\text{N}_2\text{O}_4]\) (M) | \([\text{NO}_2]\) (M) |
|---|---|---|
| Initial | \(0.375\) | \(0\) |
| Equilibrium | — | \(0.500\) |
What is the value of \(K_c\) at this temperature for the reaction \(2\text{NO}_2\text{(g)} \rightleftharpoons \text{N}_2\text{O}_4\text{(g)}\)?
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