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Answer to Question #21243 in Physical Chemistry for nidhi mehra

Question #21243
the reaction N2+O2=2NO2 contributes to air pollution. whenever a fuel is burnt in air at high temp. At 1500 K equilibrium constant K for it is 1.0*10^-5. suppose in a case [N2]=0.80 mol per litre and [O2]= 0.20 mol per litre before any reaction occurs. Calculate the equillibrium concerntrations of the reactants and the products after the mixture has been heated to 1500 K.
Expert's answer
Equilibrium constant can be calculated by next equation:

K = [products]/[reactants]

K = [NO2]2/[O2][N2]

Concentration after reaction would be: (where x is that part
of reactants that would be converted in product)

0.8-x 0.2-x 2x
N2 + O2 = 2NO2
In the moment at equilibrium equilibrium constant would be:

K = [2x]2/[0.8-x][0.2-x]

1.0*10^-5 * (0.8-x)*( 0.2-x) = 4x2

1.0*10^-5 * (0.6-0.8x-0.2x+x^2) = 4x2

6.0*10^-6 - 6.0*10^-6 x + 1.0*10^-5x^2 - 4x^2 = 0

x = 0.001224 M so concentration of product NO2 m = 2*0.001224 = 0.002448 M

concentration of O2 = 0.2-0.001224 = 0.198776 and concentration of N2 = 0.798776 M

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