Molecular hydrogen can be made from methane gas by the reaction below. How is th

Question

Molecular hydrogen can be made from methane gas by the reaction below. How is the rate of disappearance of CH_4 related to the rate of appearance of H_2? Delta [CH_4]/Delta t = ? CH_4 (g) + H_2O(l) rightarrow CO(g) + 3H_2(g) A) + 1Delta [H_2]/3 Delta t B) +3 Delta [H_2]/Delta) + Delta [H_2]/Delta t D) none of these For a reaction that follow, the general rate law, Rate = k[A]([B]^2, what will happen to the rate of reaction if the concentration of A is increased by a factor of 3.00? The rate will A) decrease by a factor of 1/900. B) decrease by a factor of 1/3.00. C) increase by a factor of 9.00 D) increase by a factor of 3.00 What is the overall reaction order for the reaction that has the rate law: Rate - k[H_2][NO]^2? A) zero order B)first order C) second order D) third order The following set of data was obtained by the method of initial rates for the fraction: (H_3C_3CBr + OH^- rightarrow (H_3C)_3COH + Br^- What is the order of reaction with respect to ion OH^-? A) zero B) first C) second D) none of these Which statement below regarding the half life of a zeroth order reactions is true? A) Each half life is four times as long as the preceding half life. B) The half-life remains unchanged throughout the course of the reaction. C) Each half life is half as long as the preceding half life. D) Each halt-life is twice as long at the preceding half life For a particular first order reaction, it takes 2880 seconds for the concentration of the reactant to decrease from 2.0 M to .50 M. What is the value for rate constant in g^-1 for the reaction? A) 2.9 times 10^-2 g^-1 B) 1.0 times 10^-4 g^-1 C) 6.0 times 10^-3 g^-1 D) 4.8 times 10^-4 g^-1 The rate constant k, for a first order reaction is equal to 4.2 times 10^-4 g^-1. What is the half life for the reaction. A) 2.0 times 10^-4 s B) 1.7 times 10^3 s C) 1.2 times 10^3 s D) 2.4 times 10^3 s

Explanation / Answer

When concentration of OH- is doubled from 0.25M to 0.5M by keeping keeping concentraion of (CH3)3CBr at 0.5M, the rate of the reaction remains constant at 2.2 x 10^-4.

So the rate of reaction is independent of concentartion of OH-

order with respect to OH- is zero

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