04-09-2018, 03:58 PM

Hello, I'd like some help solving a gaseous equilibrium-type problem.

My new chemistry professor isn't a native English speaker and i'm pulling my hair out trying to understand his accent and prolixity; It makes everything so much more difficult. The following problem was presented in his lecture and taken out of a textbook.

Given reaction:

N2O4 (g) ::equil:: 2NO2 (g)

Problem:

Given that the partial pressures of those two gasses at equilibrium is .34ATMN2O4, and 1.20ATMNO2, calculate the equilbrium partial pressures of the two gasses when the volume of the container has been doubled.

what I've tried so far: according to Le Chatelier's Principle, if the volume of the container is increased, the reaction will shift to the right side of the above equation.

.236Kp = (.17-x)/(.6+2x)2

.17-x represents the equilibrium partial pressure of the N2O4 gas, and .6+2x represents the equilibrium partial pressure of the NO2 gas.

x= .0526

[NO2] = .494M

[N2O4]= .117M

My mental notes:

-The resulting Kp value is approximately twice of the original Kp calculated from the given partial pressures.

Any input would be so much appreciated.

My new chemistry professor isn't a native English speaker and i'm pulling my hair out trying to understand his accent and prolixity; It makes everything so much more difficult. The following problem was presented in his lecture and taken out of a textbook.

Given reaction:

N2O4 (g) ::equil:: 2NO2 (g)

Problem:

Given that the partial pressures of those two gasses at equilibrium is .34ATMN2O4, and 1.20ATMNO2, calculate the equilbrium partial pressures of the two gasses when the volume of the container has been doubled.

what I've tried so far: according to Le Chatelier's Principle, if the volume of the container is increased, the reaction will shift to the right side of the above equation.

.236Kp = (.17-x)/(.6+2x)2

.17-x represents the equilibrium partial pressure of the N2O4 gas, and .6+2x represents the equilibrium partial pressure of the NO2 gas.

x= .0526

[NO2] = .494M

[N2O4]= .117M

My mental notes:

-The resulting Kp value is approximately twice of the original Kp calculated from the given partial pressures.

Any input would be so much appreciated.