The triple bond in the N2 molecule is very strong, but at high enough temperatures even it breaks down. At 5000 K, when the total pressure exerted by a sample of nitrogen is 1.00 atm, N2(g) is 0.65% dissociated at equilibrium: N2(g) 2 2 N(g) At 6000 K with the same total pressure, the proportion of N,(g) dissociated at equilibrium rises to 11.6%. Use the van't Hoff equation to estimate the AH of this reaction.

The triple bond in the N2 molecule is very strong, but at high enough temperatures even it breaks down. At 5000 K, when the total pressure exerted by a sample of nitrogen is 1.00 atm, N2(g) is 0.65% dissociated at equilibrium: N2(g) 2 2 N(g) At 6000 K with the same total pressure, the proportion of N,(g) dissociated at equilibrium rises to 11.6%. Use the van't Hoff equation to estimate the AH of this reaction.

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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