At a particular temperature, Kp = 0.460 for the reaction

N2O4(g) = 2NO2(g)
a)A flask containing only NO2(g) at an initial pressure of 7.00 atm is allowed to reach equilibrium. Calculate the total pressure in this flask at equilibrium.

b)With no change in the amount of material in the flask, the volume of the container in question is increased to 9.000 times the original. Assuming constant temperature, calculate the (new) total pressure, at equilibrium.

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1. .....................N2O4(g) = 2NO2(g)
I......................0..................7.00
C...................+p..................-2p
E....................p...................7.00-2p
Kp = (7.00-2p)^2/(p) = 0.460
Solve for p, evaluate p and 7.00-2p, then add to obtain total P. You will need to solve a quadratic equation.
2. Take the values you find for p and 7.00-2p in problem 1, divide by 9 for each (since the volume is increased by 9 you know the concentration will be decreased by 9) and substitute these new values for N2O4 and NO2 into the equation for line I (initial) and recalculate.
Post your work if you get stuck.

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