AP Chemistry
7.7 Calculating Equilibrium Concentrations
At \(700\text{ K}\), the equilibrium constant \(K_p\) for the reaction represented below is \(64\).
\[\text{H}_2\text{(g)} + \text{I}_2\text{(g)} \rightleftharpoons 2\,\text{HI(g)}\]
A rigid reaction vessel is initially charged with \(\text{H}_2\text{(g)}\) and \(\text{I}_2\text{(g)}\), each at a partial pressure of \(1.0\text{ atm}\), with no \(\text{HI(g)}\) present. The mixture is allowed to reach equilibrium at \(700\text{ K}\). What is the equilibrium partial pressure of \(\text{H}_2\text{(g)}\)?
\[\text{H}_2\text{(g)} + \text{I}_2\text{(g)} \rightleftharpoons 2\,\text{HI(g)}\]
A rigid reaction vessel is initially charged with \(\text{H}_2\text{(g)}\) and \(\text{I}_2\text{(g)}\), each at a partial pressure of \(1.0\text{ atm}\), with no \(\text{HI(g)}\) present. The mixture is allowed to reach equilibrium at \(700\text{ K}\). What is the equilibrium partial pressure of \(\text{H}_2\text{(g)}\)?
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