Question

Suppose a 500.mL flask is filled with 1.0mol of O2 and 1.8mol of NO . The following reaction becomes possible: N2g+O2g =2NOg The equilibrium constant K for this reaction is 0.461 at the temperature of the flask. Calculate the equilibrium molarity of N2 . Round your answer to two decimal places.

Final answer in molarity M 2 decimal places

Answer 1

Molarity of O2 = 1 / 0.5 = 2

Molarity of NO = 1.8 / 0.5 = 3.6 M

N2   +    O2    ------------> 2 NO

0          2                           3.6

x             2+x                    3.6 - 2x

K = (3.6-2x)^2 / (2+x)(x)

0.461 = (3.6-2x)^2 / (2+x)(x)

x = 1.15

Equlibrium Molarity of N2 = 1.15 M