At 861 oC the equilibrium constant for the reaction: 2 IBr(g) I2(g) + Br2(g) is KP = 1.86. If the initial pressure of IBr is 0.00743 atm, what are the equilibrium partial pressures of IBr, I2, and Br2? p(IBr) = p(I2) = p(Br2) =

At 861 oC the equilibrium constant for the reaction: 2 IBr(g) I2(g) + Br2(g) is KP = 1.86. If the initial pressure of IBr is 0.00743 atm, what are the equilibrium partial pressures of IBr, I2, and Br2? p(IBr) = p(I2) = p(Br2) =

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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Question

At 861 ^oC the equilibrium constant for the reaction:

2 IBr(g) I₂(g) + Br₂(g)

is K_P = 1.86. If the initial pressure of IBr is 0.00743 atm, what are the equilibrium partial pressures of IBr, I₂, and Br₂?

p(IBr) =

p(I₂) =

p(Br₂) =

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