Consider the equilibrium NO2(g) = NO(g) + 1/2 O2(g). One mole of NO2(g) is placed in a vessel and allowed to come to equilibrium at. a total pressure of 1 bar. An analysis of the contents of the vessel gives the following results: 700 K 800 K PNo/PNO2 0.872 2.5 a. Calculate Kp at( 700 K)=, b. Calculate AG'R and AH"R for this reaction at 298,15 K, using only the data in the problem. Assume that AH R is independent of ,and (800 K) = temperature. AG R(KJ mol") = c. Calculate AG'R and AH'R using the following data. AH'R(kJ mol')- Data: AH"(KJ mol") for NO(g): 91.3, NO2(9): 33.2. and AH'R(kJ mol')=
Consider the equilibrium NO2(g) = NO(g) + 1/2 O2(g). One mole of NO2(g) is placed in a vessel and allowed to come to equilibrium at. a total pressure of 1 bar. An analysis of the contents of the vessel gives the following results: 700 K 800 K PNo/PNO2 0.872 2.5 a. Calculate Kp at( 700 K)=, b. Calculate AG'R and AH"R for this reaction at 298,15 K, using only the data in the problem. Assume that AH R is independent of ,and (800 K) = temperature. AG R(KJ mol") = c. Calculate AG'R and AH'R using the following data. AH'R(kJ mol')- Data: AH"(KJ mol") for NO(g): 91.3, NO2(9): 33.2. and AH'R(kJ mol')=
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter8: Thermochemistry
Section: Chapter Questions
Problem 90QAP: Consider a metal ion A2+ and its nitrate salt, In an experiment, 35.00 mL of a 0.217 M solution of...
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