c. In a different equilibrium mixture, under different conditions, the partial pressures of thegases are shown in the table:GasPartial pressure / kPaN21.20 x 102H21.50 x 102NH31.10 x 103Calculate the value of the equilibrium constant (Kp) for this reaction and give its units.d. The enthalpy change for the reaction is -92 kJ mol-1State the effect, if any, of an increase in temperature on the value of Kp for this reaction.Explain your answer.3. a. Name the catalyst used in the Haber process.b. Explain why a catalyst does not change the yield of ammonia produced.c. Sketch a Maxwell Boltzmann distribution curve (with labelled axes) and use it to explain whya catalyst will increase the rate of reaction.

Answered: Image /qna-images/answer/aad6dc9c-97c9-4134-bda5-79134cc8c3e3.jpg

c. In a different equilibrium mixture, under different conditions, the partial pressures of gases are shown in the table: Gas Partial pressure / kPa N2 1.20 x 10? H2 1.50 x 102 NH3 1.10 x 103 Calculate the value of the equilibrium constant (Kp) for this reaction and give its units.

c. In a different equilibrium mixture, under different conditions, the partial pressures of gases are shown in the table: Gas Partial pressure / kPa N2 1.20 x 10? H2 1.50 x 102 NH3 1.10 x 103 Calculate the value of the equilibrium constant (Kp) for this reaction and give its units.

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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