Question 6. Inside a rigid container, initially filled with 2.5 kPa CO2 at 383.08K. Then excessive amount of NHCOONH4(S) is added inside and the volume of the solid is negligible Assume the only reaction inside the system is: NH2COONH4(S) 2 NH3 (g) + CO2 (g). After equilibrium, the total pressure of the system is 6.39 kPa. (a) At this temperature if Fe catalyst is added, the NH3 can decompose as: 2NH3 = N2 + 3H2 At 298K, this reaction A, G = -33kJ /mol, A,H = -92.4kJ/mol Assume A, H is constant and there was some other inert gas to keep the pressure at 100 kpa Calculate the partial pressure of N2, H2 and CO2 at equilibrium

Question 6. Inside a rigid container, initially filled with 2.5 kPa CO2 at 383.08K. Then excessive amount of NHCOONH4(S) is added inside and the volume of the solid is negligible Assume the only reaction inside the system is: NH2COONH4(S) 2 NH3 (g) + CO2 (g). After equilibrium, the total pressure of the system is 6.39 kPa. (a) At this temperature if Fe catalyst is added, the NH3 can decompose as: 2NH3 = N2 + 3H2 At 298K, this reaction A, G = -33kJ /mol, A,H = -92.4kJ/mol Assume A, H is constant and there was some other inert gas to keep the pressure at 100 kpa Calculate the partial pressure of N2, H2 and CO2 at equilibrium

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 89AP

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