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Question

The reaction X products follows first order kinetics. In 40 minutes, the concentration of X changes from 0.1 M to 0.025 M. The rate of reaction when concentration of X is 0.01 M is:
  1. 1.73×104M min1
  2. 3.47×105M min1
  3. 3.47×104M min1
  4. 1.73×105M min1


Solution

The correct option is C 3.47×104M min1
Explanation :

k=2.303t log aax

=2.303(40 min)log(0.1 M)(0.025 M)

=2.303×0.6021(40~min)=0.03467 min1

Rate = k[x]

=(0.03467, min1)×(0.01 M)

=3.47×104M min1

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