The reaction : 2NO + H_2 → H_2 + 2H_2O has been assigned to follow the followingmechanism. I . NO + NO ⇌ N_2O_2 (fast) II. N_2O_2 + H_2 → N_2O + H_2O (slow) III. N_2O + H_2 → N_2 + H_2O (fast) The rate constant of step II is 1.2 × 10^{-4} l mole^{-1}min^{-1} 1while equilibrium constant ofstep I is 1.4 × 10^{-2} L mole^{-1} What is the rate of reaction when concentration of NO and H_2 each is 0.5 mole L^{-1}

Question

The reaction : 2NO + H_2  → H_2 + 2H_2O  has been assigned to follow the followingmechanism. I . NO + NO ⇌ N_2O_2 (fast) II. N_2O_2 + H_2 → N_2O + H_2O (slow) III. N_2O + H_2 → N_2 + H_2O (fast) The rate constant of step II is 1.2 × 10^{-4} l mole^{-1}min^{-1}  1while equilibrium constant ofstep I is 1.4 × 10^{-2}  L mole^{-1} What is the rate of reaction when concentration of NO and H_2 each is 0.5 mole L^{-1}

Examsnet · Accepted Answer

Correct Answer is : 2.1 × 10−7 mole L−1 min−1

JEE Advanced Model Paper 9 with solutions for online practice