AP Chemistry
7.4 Calculating the Equilibrium Constant
7.3 Reaction Quotient and Equilibrium Constant
A student introduces sulfur dioxide and oxygen into a rigid vessel maintained at a constant temperature. The system reaches equilibrium according to the equation
\(2\text{SO}_2\text{(g)}+\text{O}_2\text{(g)}\rightleftharpoons2\text{SO}_3\text{(g)}\)
The measured equilibrium partial pressures are shown below.
What is the value of \(K_p\) for the reaction at this temperature?
\(2\text{SO}_2\text{(g)}+\text{O}_2\text{(g)}\rightleftharpoons2\text{SO}_3\text{(g)}\)
The measured equilibrium partial pressures are shown below.
| Gas | Equilibrium partial pressure (atm) |
|---|---|
| \(\text{SO}_2\) | \(0.50\) |
| \(\text{O}_2\) | \(0.40\) |
| \(\text{SO}_3\) | \(0.20\) |
What is the value of \(K_p\) for the reaction at this temperature?
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