The reactionN₂O4(g)2NO₂(g)has a Kp = 0.140 at 25 °C. In a reaction vessel containing the gases in equilibrium at that temperature, the partial pressure of N₂O4was 0.344 atm.(a) What was the partial pressure of NO2 in the reaction mixture?pressure of NO₂ =atm(b) What was the total pressure of the mixture of gases?total pressure =atm

Given -> N2O4(g) <-----> 2NO2(g) Kp = 0.140 T = 25°C = 25 + 273 = 298 K Partial pressure…

The reaction N2O4(8) 2NO₂(g) has a Kp = 0.140 at 25 °C. In a reaction vessel containing the gases in equilibrium at that temperature, the partial pressure of N2O4 was 0.344 atm. (a) What was the partial pressure of NO2 in the reaction mixture? pressure of NO₂ = i atm (b) What was the total pressure of the mixture of gases? total pressure = atm

The reaction N2O4(8) 2NO₂(g) has a Kp = 0.140 at 25 °C. In a reaction vessel containing the gases in equilibrium at that temperature, the partial pressure of N2O4 was 0.344 atm. (a) What was the partial pressure of NO2 in the reaction mixture? pressure of NO₂ = i atm (b) What was the total pressure of the mixture of gases? total pressure = atm

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.79PAE

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