The equilibrium constant, \( K \), for the following reaction is \( 1.20 \times 10^{-2} \) at 500 K.\[ \text{PCl}_5(g) \rightleftharpoons \text{PCl}_3(g) + \text{Cl}_2(g) \]An equilibrium mixture of the three gases in a 1.00 L flask at 500 K contains 0.269 M \(\text{PCl}_5\), \(5.68 \times 10^{-2}\) M \(\text{PCl}_3\), and \(5.68 \times 10^{-2}\) M \(\text{Cl}_2\). What will be the concentrations of the three gases once equilibrium has been reestablished, if \(5.09 \times 10^{-2}\) mol of \(\text{PCl}_3(g)\) is added to the flask?\[ [\text{PCl}_5] = \text{M} \]\[ [\text{PCl}_3] = \text{M} \]\[ [\text{Cl}_2] = \text{M} \]

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The equilibrium constant, K, for the following reaction is 1.20x10-2 at 500 K. PCI5(9) =PC13(g) + Cl₂(9) An equilibrium mixture of the three gases in a 1.00 L flask at 500 K contains 0.269 M PCI5, 5.68x10-2 M PCI3 and 5.68x10-2 M Cl₂. What will be the concentrations of the three gases once equilibrium has been reestablished, if 5.09x10-2 mol of PCI3(g) is added to the flask? [PCI5] = [PCI3] = [Cl₂] = ΣΣΣ

The equilibrium constant, K, for the following reaction is 1.20x10-2 at 500 K. PCI5(9) =PC13(g) + Cl₂(9) An equilibrium mixture of the three gases in a 1.00 L flask at 500 K contains 0.269 M PCI5, 5.68x10-2 M PCI3 and 5.68x10-2 M Cl₂. What will be the concentrations of the three gases once equilibrium has been reestablished, if 5.09x10-2 mol of PCI3(g) is added to the flask? [PCI5] = [PCI3] = [Cl₂] = ΣΣΣ

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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