a) Two reactants, A and B, were mixed and allowed to react. The concentration of

Question

a) Two reactants, A and B, were mixed and allowed to react. The concentration of A was in large excess. The concentration of B was measured and t0.9 values (time required to reach 0.9 times an initial concentration) were calculated. When log(t0.9) was plotted vs. log{[B]o}, the slope was found to be +1.49. What is the order of the reaction with respect to B?

b) This has nothing to do with part a). Here is an overall reaction: Fe3+ + V3+ Fe2+ + V4+

Here is its rate law: rate = k{[Fe3+][V4+][V3+]}/[Fe2+] Give a possible rate determining step.

Explanation / Answer

A log-log plot of rate versus concentration gives a straight line which gives a slope which gives the order of the species which is the used as the concentration term on the axis.

So the order of the reaction with respect to B is 1.49.

b) Fe3+ + V3+ Fe2+ + V4+

If the rate = k{[Fe3+][V4+][V3+]}/[Fe2+]

then the rate determining step is

one where both Fe3+ and V3+ is present in the slow step.

which means the slop step is the actual reaction.

Fe3+ + V3+ Fe2+ + V4+

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