**Chemical Equilibrium Problem**Consider the reaction:\[ \text{N}_2(g) + \text{O}_2(g) \rightleftharpoons 2\text{NO}(g) \]If the equilibrium partial pressures of \(\text{N}_2\), \(\text{O}_2\), and \(\text{NO}\) are 0.16 atm, 0.20 atm, and 0.045 atm, respectively, at 2200°C, what is \(K_p\)?**Solution:**To find the equilibrium constant (\(K_p\)), use the expression:\[ K_p = \frac{(P_{NO})^2}{(P_{N_2})(P_{O_2})} \]Where:- \(P_{NO} = 0.045 \, \text{atm}\)- \(P_{N_2} = 0.16 \, \text{atm}\)- \(P_{O_2} = 0.20 \, \text{atm}\)Substitute the given values into the equation to find \(K_p\).

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Answered: Consider the reaction N2(g) + O2(g)…

Consider the reaction N2(g) + O2(g) 2NO(g) If the equilibrium partial pressures of N2, O2, and NO are 0.16, 0.20, and 0.045 atm, respectively, at 2200°C, what is Kp?

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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