Consider the equilibrium system: N2O4 (g) = 2 NO2 (g) for which the Kp = 0.1134 at 25 C and deltaH rx is 58.03 kJ/mol. Assume that 1 mole of N2O4 and 2 moles of NO2 are introduced into a 5 L contains. What will be the equilibrium value of [N204]? A) 0.358 M
B) 0.042 M
C) 0.0822 M
D) 0.928 M
E) 0.379 M

The equilibrium value of is 0.379 M

Explanation:

Equilibrium constant is the ratio of the concentration of products to the concentration of reactants each term raised to its stochiometric coefficients.

Using ideal gas equation :

P = pressure of gas

V = volume of gas

n = no of moles

R = gas constant

T = Temperature

pressure of =

pressure of =

at t= 0    5 atm                                10 atm

at eqm    (5-x) atm                          (10+2x) atm

pressure of at equilibrium = (5-(-4.48))= 9.48 atm

pressure of =

9.48 =

Thus the equilibrium value of is 0.379 M

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