AP Chemistry
7.7 Calculating Equilibrium Concentrations
A student models a high-temperature gas-processing system using a rigid container maintained at constant temperature. The gases react according to the equation
\(2\text{SO}_3\text{(g)} \rightleftharpoons 2\text{SO}_2\text{(g)} + \text{O}_2\text{(g)}\)
Before appreciable reaction occurs, the partial pressures are \(0.80\text{ atm}\) for \(\text{SO}_3\text{(g)}\), \(0.10\text{ atm}\) for \(\text{O}_2\text{(g)}\), and \(0\text{ atm}\) for \(\text{SO}_2\text{(g)}\). At equilibrium, the total pressure in the container is \(1.10\text{ atm}\). What is the equilibrium partial pressure of \(\text{SO}_2\text{(g)}\)?
\(2\text{SO}_3\text{(g)} \rightleftharpoons 2\text{SO}_2\text{(g)} + \text{O}_2\text{(g)}\)
Before appreciable reaction occurs, the partial pressures are \(0.80\text{ atm}\) for \(\text{SO}_3\text{(g)}\), \(0.10\text{ atm}\) for \(\text{O}_2\text{(g)}\), and \(0\text{ atm}\) for \(\text{SO}_2\text{(g)}\). At equilibrium, the total pressure in the container is \(1.10\text{ atm}\). What is the equilibrium partial pressure of \(\text{SO}_2\text{(g)}\)?
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