Consider the simple one-step reaction: A(g) = B(g) Since the reaction occurs in a single step, the forward reaction has a rate of kjoe[A] and the reverse reaction has a rate of kgev[B]. What happens to the rate of the forward reaction when we in- crease the concentration of A? How does this explain the reason behind Le Châtelier's principle?

Consider the simple one-step reaction: A(g) = B(g) Since the reaction occurs in a single step, the forward reaction has a rate of kjoe[A] and the reverse reaction has a rate of kgev[B]. What happens to the rate of the forward reaction when we in- crease the concentration of A? How does this explain the reason behind Le Châtelier's principle?

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

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 120CP: The equilibrium constant for a certain reaction decreases from 8.84 to 3.25 102 when the...

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