Consider the following reaction: 2NO2(g)⇌N2O4(g) Calculate the partial pressures of NO2(g) andN2O4 at equilibrium in atm, if the total pressure in the system at equilibrium was 1.304 atm and Kp=7.00
Consider the following reaction: 2NO2(g)⇌N2O4(g) Calculate the partial pressures of NO2(g) andN2O4 at equilibrium in atm, if the total pressure in the system at equilibrium was 1.304 atm and Kp=7.00
Chemistry by OpenStax (2015-05-04)
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Chapter16: Thermodynamics
Section: Chapter Questions
Problem 50E: Consider the decomposition of CaCO3(s) into CaO(s) and Co2(g). What is the equilibrium partial...
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Consider the following reaction: 2NO2(g)⇌N2O4(g)
Calculate the partial pressures of NO2(g) andN2O4 at equilibrium in atm, if the total pressure in the system at equilibrium was 1.304 atm and Kp=7.00
Hint: PN2O4+PNO2=Ptotal
Group of answer choices
PNO2 =0.100; PN2O4=1.204
PNO2 =0.51; PN2O4=0.79
PNO2 =0.200; PN2O4=0.110
PNO2 =0.250; PN2O4=1.09
PNO2 =0.366; PN2O4=0.938
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