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Question

For a first-order reaction X product, the concentration of X changes from 0.2 M to 0.05 M in 40 minutes, find the rate of reaction of X when its concentration is 0.02 M.

A
1.73×104Mmin1
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B
6.93×104Mmin1
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C
1.73×105Mmin1
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D
3.47×105Mmin1
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Solution

The correct option is C 6.93×104Mmin1
For a first order reaction we use:
ln(AoA)=kt (Integrated Rate Law)

Using Ao=0.2M A=0.05M we get

k=2ln(2)40min1

Rate of the reaction, dAdt=k[A]=2ln(2)40min1×0.02M

=6.93×104Mmin1
Option B is correct.

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