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.\[ K_c = \boxed{} \]

The number of moles of SO2 and O2 introduced to container is 6.86×10-2 mol and 8.48×10-2 mol,…

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. =

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. =

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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