Question
For the chemical system shown below, it was found that[N2] = [O2] = 0.70 mol/L and [NO] =0.22mol/L, at equilibrium. Suppose that enough N2 wasadded to increase its concentration temporarily to 1.00 equilibriumconcentrations of N2, O2, and NO? N2 + O2(g) <-> 2NO(g) Thanks! For the chemical system shown below, it was found that[N2] = [O2] = 0.70 mol/L and [NO] =0.22mol/L, at equilibrium. Suppose that enough N2 wasadded to increase its concentration temporarily to 1.00 equilibriumconcentrations of N2, O2, and NO? N2 + O2(g) <-> 2NO(g) Thanks!
Explanation / Answer
The given reaction N2 (g) +O2 (g) ------> 2NO(g) But at the euilibrium the concentration of N2 and O2 areequal. [N2]= [O2] =0.70 mol/L and [NO] =0.22mol/L Rate constant Kc = [NO]2 / [N2][O2] =(0.22)2 /(0.70) (0.70) = 0.0484/0.49 = 0.0987 If N2 concentration as increased to 1.00 then there is nochange the other two concentrationof NO,O2 But the final rate is changed at equilibrium.