Calculate Kp and ΔG for each of the followingreactions:(a) N2(g) + 3 H2(g)---->2 NH3(g)PN2 = 2.6 atm, PH2 = 5.9 atm, PNH3 = 1.2 atm(b) 2 N2H4(g) + 2 NO2(g)--->3 N2(g) + 4 H2OvPN2H4 = PNO2 = 5.0 x10-2 atm,PN2 = 0.5 atm, PH2O = 0.3 atm(c) N2H4(g)---->N2(g) + 2 H2(g)PN2H4 = 0.5 atm, PN2 = 1.5 atm, PH2 = 2.5 atm

Kp is equilibrium constant and ΔG is Change in Gibbs free energy ΔG= -RTlnKp

Answered: Calculate Kp and ΔG for each of the…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter17: Chemcial Thermodynamics

Section: Chapter Questions

Problem 17.75QE

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Calculate Kp and ΔG for each of the following
reactions:
(a) N₂(g) + 3 H₂(g)---->2 NH₃(g)
P_N2 = 2.6 atm, P_H2 = 5.9 atm, P_NH3 = 1.2 atm
(b) 2 N₂H₄(g) + 2 NO₂(g)--->3 N₂(g) + 4 H₂Ov
P_N2H4 = P_NO2 = 5.0 x10^-2 atm,
P_N2 = 0.5 atm, P_H2O = 0.3 atm
(c) N₂H₄(g)---->N₂(g) + 2 H₂(g)
P_N2H4 = 0.5 atm, P_N2 = 1.5 atm, P_H2 = 2.5 atm

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