Posted by **Frank** on Thursday, April 22, 2010 at 2:38am.

Given: N2O4 (g) « 2NO2 (g) @ 25 degrees celcius, Kc is 5.84 x 10^-3.

(A) Calculate the equilibrium concentrations of both gases when 4.00 grams of N2O4 is placed in a 2.00 L flask at 25 degrees celcius.

(B) What will be the new equilibrium concentrations if the volume of the system is suddenly increased to 3.00 L at 25 degrees celcius.

(C) What effect would increasing the pressure at 25 degrees celcius have on the equilibrium?

- CHEMISTRY HELP NEEDED A.S.A.P -
**Dr Russ**, Thursday, April 22, 2010 at 4:33am
You have not shown the units for Kc, but let us assume that the units are moles/L

1. Calculate the number of moles of N2O4 and hence the concentration (C) in moles/L.

2. At equilibrium let the concentration of NO2=x

Thus Kc=[NO2]^2/[N2O4]

Kc=(x)^2/(C-x)= 5.84x10^-3

we know C so solve for x

for part B repeat the calculation using the new volume.

for part C by Le Chateliers Principle the equilibrium will move in the direction to accommodate the change so will move to smaller volume, which is the N2O4 side.

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