-198 kJ, and K = 34.5, at 1.15 × 10³ K:Consider the following system at equilibrium where AH° = -198 kJ, and Ke2SO2(g) + O2(g)=2SO3 (9)If the temperature on the equilibrium system is suddenly decreased:The value of KO increasesO decreasesOremains the sameThe value of QcO is less than KcO is greater than KcO is equal to KThe reaction mustOrun in the forward direction to reestablish equilibriumOrun in the reverse direction to reestablish equilibriumO remain in the current position, since it is already at equilibriumThe concentration of O2 willO increaseOdecreaseO remain the samePreviousNext

For the given reaction2SO2(g)+O2(g)⇌2SO3(g) The value of ΔH0 = -198 KJ.The negative value of ΔH0…

Answered: -198 kJ, and K = 34.5, at 1.15 × 10³ 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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Consider the following system at equilibrium where AH° = -87.9 kJ/mol, and K. = 83.3 , at 500 K. PCI3 (g) + Cl2 (g) = PCI5 (g) When 0.22 moles of PCI3 (g) are removed from the equilibrium system at constant temperature: The value of Ke increase. decrease. remain the same. The value of Qc K.. is greater than is equal to is less than The reaction must Orun in the forward direction to restablish equilibrium. Orun in the reverse direction to restablish equilibrium. Oremain the same. It is already at equilibrium. The concentration of Cl, will increase. decrease. remain the same.
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