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Be sure to answer all parts. thallium(i) is oxidized by cerium(iv) as follows: tl+(aq) + 2ce4+(aq) → tl3+(aq) + 2ce3+(aq) the elementary steps, in the presence of aqueous mn(ii), are as follows: step 1: ce4+ + mn2+ → ce3+ + mn3+ step 2: ce4+ + mn3+ → ce3+ + mn4+ step 3: tl+ + mn4+ → tl3+ + mn2+ the rate law is given by the equation: rate = k[ce4+][mn2+] identify the catalyst: tl+ tl3+ ce3+ ce4+ mn2+ mn3+ mn4+ identify the intermediates: tl+ tl3+ ce3+ ce4+ mn2+ mn3+ mn4+ identify the rate-determining step

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W0lf93
Best Answer: Mn(ii) is catalyst Stetep-1 is slow step Steps-2,3 are fast steps intermediates are Mn(iii)and Mn(iv) since step -1 is slow rate depends on Ce(iv) and Mn(ii) only not on Tl(i) as it is involved in fast step-3

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