What is the rate law for the reaction? C_2 H_6 O_2 + 2Br_2 rightarrow C_3 H_4 Br

Question

What is the rate law for the reaction? C_2 H_6 O_2 + 2Br_2 rightarrow C_3 H_4 Br_2O_2 + 2HBr (A) rate = k[C_3H_6O_2] (B) rate = k[C_3H_6O_2]^2 (C) rate = k[C_3 H_6O_2] [Br_2] (D) rate = k[C_3H_6O_2] [Br_2]^2 The main reason that reaction rates normally decrease as the temperature is decreased is that the (A) equilibrium constant increases as the temperature decreases. (B) activation energy increases as the temperature decreases. (C) energy of molecular collisions decreases as the temperature decreases. (D) all of the above. Which diagram represents a forward reaction with Delta H^compositefunction + 10.0 kJ and E_ = + 35.0 kJ? Which rate law corresponds to the proposed mechanism for the decomposition of N_2O? (A) Rate = k [N_2 O]^2 (B) Rate = k [N_2 O] (C) Rate = k [N_2 O] [O] (D) Rate = k [N_2 O]^2 [O]

Explanation / Answer

48. For a reaction: A + 2B----> Products

As the rate of a reaction is directly proportional to the reactant concentrations, thus the rate of reaction may be expressed as

                      Rate [A]1[B]2

                       Rate = k [A]1 [B]2

Similarly for a given reaction

C3H6O2 + 2Br2    ----> C3H4Br2O2 + 2HBr

So the rate = k [C3H6O2] [Br2]2

But according to the Law of mass action, in the above reaction the rate is found to be proportional to [Br2] although the quotient of Br2 in the equation is 2.

Thus the rate = k [C3H6O2] [Br2]. So option C is the correct answer

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