A student ran the following reaction in the laboratory at 1197 K: 2502(g) + O2(g) = 2503(g) When she introduced 6.86x10-2 moles of SO2(g) and S.48x102 moles of O,(g) into a 1.00 liter container, she found the equilibrium concentration of SO3(g) to be 3.49×102 M. Calculate the equilibrium constant, K, she obtained for this reaction. K. =

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A student ran the following reaction in the laboratory at 1197 K:

\[ 2\text{SO}_2(\text{g}) + \text{O}_2(\text{g}) \rightleftharpoons 2\text{SO}_3(\text{g}) \]

When she introduced \( 6.86 \times 10^{-2} \) moles of \(\text{SO}_2(\text{g})\) and \( 8.48 \times 10^{-2} \) moles of \(\text{O}_2(\text{g})\) into a 1.00 liter container, she found the equilibrium concentration of \(\text{SO}_3(\text{g})\) to be \( 3.49 \times 10^{-2} \) M.

Calculate the equilibrium constant, \( K_c \), she obtained for this reaction.

\[ K_c = \boxed{} \]
Transcribed Image Text:A student ran the following reaction in the laboratory at 1197 K: \[ 2\text{SO}_2(\text{g}) + \text{O}_2(\text{g}) \rightleftharpoons 2\text{SO}_3(\text{g}) \] When she introduced \( 6.86 \times 10^{-2} \) moles of \(\text{SO}_2(\text{g})\) and \( 8.48 \times 10^{-2} \) moles of \(\text{O}_2(\text{g})\) into a 1.00 liter container, she found the equilibrium concentration of \(\text{SO}_3(\text{g})\) to be \( 3.49 \times 10^{-2} \) M. Calculate the equilibrium constant, \( K_c \), she obtained for this reaction. \[ K_c = \boxed{} \]
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