Questions 9 through 12 are based upon following mechanism proposed for the decom
ID: 518455 • Letter: Q
Question
Questions 9 through 12 are based upon following mechanism proposed for the decomposition of hydrogen the peroxide using potassium bromide. A. H2O2 B (aq) + Be^- (aq) H2O(aq) + OBr^-(aq) Slow. B. H2O2(aq) + OBr^- (aq) H@O(aq) + Br^- (aq) + O2(g) Fast The overall reaction is: A. H_2O_2(aq) + OBr(aq) = H_2O(aq) + Br'(aq) + O_2(g) B. H_2O_2(aq) + Br'(aq) = H_2O(aq) + OBr'(aq) C. 2H_2O_2(aq) + Br^'(aq) = 2H_2O(aq) + OBr'(aq) + O_2(g) D. 2H_2O_2 (aq) = 2H_2O(aq) + O_2(g) E. 2H_2O_2(aq) + Br^(aq) = 2H_2O(aq) + Br'(aq) + O_2(g) The rate law for this reaction is: A. Rate = k[H_2O_2][OBr^] B. Rate = k[H_2O_2]^2 C. Rate = k[H_2O_2]^2[Br] D. Rate = k[H_2O_2][Br] E. Rate = k[H_2O_2][OBr]^2 Which of the following are reaction intermediates: A. H_2O B. Br' C. OBr ' D. None are reaction intermediates E. Both (B) and (C) are reaction intermediates.Explanation / Answer
Q.No -9 -----(B)
We know slow step is rate determining step, hence slow step is overall the reaction.
Q.No-10. ------(D)
Rate law of the reaction
Rate = K[H2O2][Br-]
Where K is rate constant of the reaction
Q.No-11 -----(C)
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