At 1000 k, a sample of pure no2 gas decomposes. 2 no2(g) equilibrium reaction arrow 2 no(g) + o2(g) the equilibrium constant kp is 158. analysis shows that the partial pressure of o2 is 0.29 atm at equilibrium. calculate the pressure of no and no2 in the mixture.

The pressure of NO and in the mixture is 0.58 atm and 0.024 atm respectively.

Explanation:

We are given:

Equilibrium partial pressure of = 0.29 atm

For the given chemical equation:

Initial:              a

At eqllm:        a-2x          2x          x

Calculating for the value of 'x'

Equilibrium partial pressure of NO = 2x = 2(0.29) = 0.58 atm

Equilibrium partial pressure of = a - 2x = a - 2(0.29) = a - 0.58

The expression of for above equation follows:

We are given:

Putting values in above expression, we get:

Neglecting the value of a = 0.555 because it cannot be less than the equilibrium concentration.

So,

Equilibrium partial pressure of = (a - 0.58) = (0.604 - 0.58) = 0.024 atm

Hence, the pressure of NO and in the mixture is 0.58 atm and 0.024 atm respectively.