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Four experiments were conducted to discover how the initial rate of consumption of BrO3- ions in...

Four experiments were conducted to discover how the initial rate of consumption of BrO3- ions in the reaction BrO3-(aq) + 5Br-(aq) + 6H+(aq) à 3Br2(aq) + 3H2O(l) varies as the concentration of the reactants are changed. Use the data given below to determine the average rate constant and write the rate law for this reaction.

Experiment

[BrO3-] (M)

[Br-] (M)

[H+] (M)

Initial rate (M/s)

1

0.10

0.10

0.10

0.0012

2

0.20

0.10

0.10

0.0024

3

0.10

0.30

0.10

0.0035

4

0.20

0.10

0.15

0.0054

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Answer #1

in experiment 1 and 3 , the concentration of BrO3^-1 but the conentration of Br- is increased 3 times. rate is also increased three times. So the reaction is 1st order with respect to Br-.

In experiment 1 and 2 the concentration of BrO3^-1 is doubled and consequently the rate is also doubled. So, the reaction is ist order with respect to BrO3^-1.

rate = k [BrO3^-1][Br-]

This is the rate law

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to find out the averate rate constant consider experiment 1

rate = k [BrO3^-1][Br-]

k=rate/ [BrO3^-1][Br-]

   = 0.0012 M/s/[0.1][0.1]= 0.12 M-1s-1

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