Problem: The initial rate for the oxidation of iron(II) by cerium(IV)Ce4+ + Fe2+   ------->  Ce3+ + Fe3+ Is measured at several different initial concentrations of the two reactants     Experiment        [Ce+4]                            [Fe2+]                          Initial Rate (M/s)1                     1.10 x10-5                       1.80 x10-5                          2.00 x10-72                     1.10 x10-5                       2.80 x10-5                          3.10 x10-73                     3.40 x10-5                       2.80 x10-5                          9.50 x10-7a) Write the rate law for this reaction.

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We’re being asked to calculate the rate law based on the data given.

     Experiment        [Ce+4]                            [Fe2+]                          Initial Rate (M/s)

1                     1.10 x10-5                       1.80 x10-5                          2.00 x10-7
2                     1.10 x10-5                       2.80 x10-5                          3.10 x10-7

3                     3.40 x10-5                       2.80 x10-5                          9.50 x10-7


Recall that the rate law only focuses on the reactant concentrations and has a general form of:

rate law=kAxBy

k = rate constant
A & B = reactants
x & y = reactant orders


We’re going to calculate the rate law and the rate constant using the following steps:


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Problem Details

The initial rate for the oxidation of iron(II) by cerium(IV)

Ce4+ + Fe2+   ------->  Ce3+ + Fe3+ 

Is measured at several different initial concentrations of the two reactants


     Experiment        [Ce+4]                            [Fe2+]                          Initial Rate (M/s)

1                     1.10 x10-5                       1.80 x10-5                          2.00 x10-7
2                     1.10 x10-5                       2.80 x10-5                          3.10 x10-7
3                     3.40 x10-5                       2.80 x10-5                          9.50 x10-7

a) Write the rate law for this reaction.

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