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Consider the following reaction, 2H2(g) + 2NO(g) N2(g) + 2H2O(g) which follows the mechanism given below: 2NO(g) k-1 k1 N2O2(g) (fast equlibrium) N2O2(g) + H2(g) k2 N2O(g) + H2O(g) (slow reaction) N2O(g) + H2(g) k3 N2(g) + H2O(g) (fast reaction) The order of the reaction is .
Answer
3
Solution
Rate is decided by the slow step: rate = k2[N2O2][H2].
From the fast equilibrium: K = k1k-1 = [N2O2][NO]2 [N2O2] = K[NO]2.
Rate = k2K[NO]2[H2]
Order = 2 + 1 = 3
Answer: 3
JEE Advanced 2024 Paper 1