The equilibrium constant, K, for the following reaction is 8.93 at 739 K.2NH3(g) N2(g) + 3H2(g)In order to Calculate Kc at this temperature for the following reaction:1/2N2(g) + 3/2H2(g) NH3(g)The original Kc value will need to be multiplied by 1/2.TrueFalse

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Answered: The equilibrium constant, K, for the…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 56QRT

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Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?
Consider the equation G = G + RT ln(Q). What is the value of G for a reaction at equilibrium? What does Q equal at equilibrium? At equilibrium, the previous equation reduces to G = RT ln(K). When G 0, what does it indicate about K? When G 0, what does it indicate about K? When t G = 0, what does it indicate about K? G predicts spontaneity for a reaction, whereas G predicts the equilibrium position. Explain what this statement means. Under what conditions can you use G to determine the spontaneity of a reaction?
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The equilibrium constant, K, for the following reaction is 8.93 at 739 K. 2NH3(g) N2(g) + 3H2(g) In order to Calculate Kc at this temperature for the following reaction: 1/2N2(g) + 3/2H2(g) NH3(g) The original Kc value will need to be multiplied by 1/2. True False