3 Consider the following reaction N2O4 g 2 NO2g K036 at 100C

3. Consider the following reaction: N2O4 (g) 2 NO2(g) K.-0.36 at 100°C A reaction mixture at 100 °C initially contains [NO2] 0.100M. The reaction is allowed to reach equilibrium. What are the concentrations of NO2 and N204 at this temperature? a) (2pt) What is the molarity of NO2 at equilibrium? b) (2pt) What is the molarity of N204 at equilibrium?

Solution

Answer

a) Molarity of NO2 at equillibrium = 0.07156M

b) Molarity of N2O4 at equillibrium = 0.01422M

Explanation

N2O4(g) <-------> 2NO2(g)

Kc = [NO2]²/[N2O4]= 0.36

At equillibrium

[N2O4] = - x

[NO2] = 0.100 + 2x

Therefore,

- ((0.100+ 2x)²/x) = 0.36

solving for x

x = - 0.01422

Therefore, at equillibrium

[N2O4] = - (-0.01422) = 0.01422M

[NO2] = 0.10 + (2× - 0.01422) = 0.07156M