The oxidation of2-butanone (CH3COC2H5) by the cerium(IV) ion in aqueous solution

Question

The oxidation of2-butanone (CH3COC2H5) by the cerium(IV) ion in aqueous solution to form acetic acid (CH3CO2H) occurs according to the following balanced equation: CH3COC2H5(aq) + 6Ce4+(aq) + 3h2O(l) rightarrow 2CH3CO2H(aq) + 6Ce3+(aq) + 6H+(aq) If acetic acid appears at an average rate of 5.5 times 10-8M/s what is delta[H+] / delta t during the same time interval? Express your answer to two significant figures and include the appropriate units. What is the average rate of consumption of Ce4+ during the same time interval? Express your answer to two significant figures and include the appropriate units.

Explanation / Answer

since H+ ion is produced thrice as acetic acid,
the H+/t=3*5.5*10^-8

=16.5*10^-8 M/s

the number of moles of H+ produced is same as that of Ce4+ used,

the rate of consumption of Ce4+=16.5*10^-8 m/s

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