We're being asked to determine the rate law for the reaction given the following initial rate data:
BrO3-(aq) + 5 Br-(aq) + 6 H+(aq) → 3 Br2(aq) + 3 H2O(l).
Expt [BrO3-] (M) [Br-] (M) [H+] (M) Rate (M/s)
1 0.10 0.10 0.10 8.0x10-4
2 0.20 0.10 0.10 1.6x10-3
3 0.20 0.15 0.10 2.4x10-3
4 0.10 0.10 0.25 5.0x10-3
Recall that the rate law only focuses on the reactant concentrations and has a general form of:
k = rate constant
A, B, and C = reactants
x, y, & z = reactant orders
To calculate the order of the reaction with respect to each reactant, we will use the experimental data given.
• BrO3-
Look for the experimental data where the concentration of BrO3- changes while the concentration of the other reactants remains the same.
The following set of data was obtained by the method of initial rates for the reaction:
BrO3-(aq) + 5 Br-(aq) + 6 H+(aq) → 3 Br2(aq) + 3 H2O(l).
What is the rate law for the reaction?
Expt [BrO3-] (M) [Br-] (M) [H+] (M) Rate (M/s)
1 0.10 0.10 0.10 8.0x10-4
2 0.20 0.10 0.10 1.6x10-3
3 0.20 0.15 0.10 2.4x10-3
4 0.10 0.10 0.25 5.0x10-3
a. rate = k[BrO3-][Br-][H+]
b. rate = k[H+]2
c. rate = k[BrO3-][Br-][H+]2
d. rate = k[BrO3-][Br-]
e. rate = k[BrO3-]2[Br-]2[H+]2
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