The reaction N2(g) + O2(g) ⇄ 2 NO(g) contributes to air pollution whenever a fuel is...
The reaction
N2(g) + O2(g) ⇄ 2 NO(g)
contributes to air pollution whenever a fuel is burned in air at a high temperature, as in a gasoline engine. At 1500 K, Kc = 1.0×10-3. Suppose a sample of air has [N2] = 0.70 mol/L and [O2] = 0.20 mol/L before any reaction occurs. Calculate the equilibrium concentrations of reactants and products after the mixture has been heated to 1500 K.
[N2] = M
[O2] = M
[NO] = M
Homework Answers
FIRST CONSTRUCT THE ICE TABLE AND THEN SUBSTITUTE THE
VALUES IN KC EXPRESSION AND YOU CAN GET THE X VALUE FROM THIS
CALCULATE THE EQUILIBRIUM CONCENTRATIONS
N2 + O2
------------------------> 2 NO
I 0.70 0.20 0
C -X -X +2X
E (0.70-X) (0.20-X) 2X
Kc = [NO]2 / [N2][O2]
1.0*10-3 = [2X]2 / [0.70-X][0.20-X]
1.0*10-3 * [0.70-X][0.20-X] = [2X]2
solving for X => 0.0058 M
at equilibrium [N2] = (0.70-X) =(0.70-0.0058) = 0.6942 M
[O2] = (0.40-X) = (0.40-0.0058) = 0.3942 M
[NO] = 2X = 2*0.0058 = 0.0116 M
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