AP Chemistry
7.7 Calculating Equilibrium Concentrations
7.4 Calculating the Equilibrium Constant
At a constant temperature, the dimerization of nitrogen dioxide gas is represented by the following equation.
\[ 2\text{NO}_2\text{(g)} \rightleftharpoons \text{N}_2\text{O}_4\text{(g)} \quad K_p = 0.50 \]
A sample of pure \(\text{NO}_2\text{(g)}\) is placed in a rigid, evacuated container at an initial partial pressure of \(2.0\text{ atm}\). Which of the following is the partial pressure of \(\text{N}_2\text{O}_4\text{(g)}\) after the system reaches equilibrium?
\[ 2\text{NO}_2\text{(g)} \rightleftharpoons \text{N}_2\text{O}_4\text{(g)} \quad K_p = 0.50 \]
A sample of pure \(\text{NO}_2\text{(g)}\) is placed in a rigid, evacuated container at an initial partial pressure of \(2.0\text{ atm}\). Which of the following is the partial pressure of \(\text{N}_2\text{O}_4\text{(g)}\) after the system reaches equilibrium?
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