# Problem: The initial rate for the oxidation of iron(II) by cerium(IV)Ce4+ + Fe2+   -------&gt;  Ce3+ + Fe3+ Is measured at several different initial concentrations of the two reactantsThe rate law for the reaction is:rate law = k[Ce4+][Fe2+]The rate constant is k = 1010.1 M-1•s-1  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 x10-7d) Predict the initial reaction rate for a solution in which [Ce4+] is 2.6 x 10-5 M and [Fe2+] is 1.3 x 10-5 M.

###### FREE Expert Solution

We are asked to calculate the initial reaction rate for a solution in which [Ce4+] is 2.6 x 10-5 M and [Fe2+] is 1.3 x 10-5 M.

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

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

The rate law for the reaction is:

rate = k[Ce4+][Fe2+]

100% (437 ratings)
###### 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

The rate law for the reaction is:

rate law = k[Ce4+][Fe2+]

The rate constant is k = 1010.1 M-1•s-1

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

d) Predict the initial reaction rate for a solution in which [Ce4+] is 2.6 x 10-5 M and [Fe2+] is 1.3 x 10-5 M.