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Question
The half life of the homogeneous gaseous reaction \[\ce{SO2Cl2 -> SO2 + Cl2}\] which obeys first order kinetics is 8.0 minutes. How long will it take for the concentration of SO2Cl2 to be reduced to 1% of the initial value?
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Solution
We know that, k = `0.693/"t"_(1/2)`
k = `0.693/8.0` minutes = 0.087 minutes−1
For a first order reaction,
t = `2.303/"k" log (["A"_0])/(["A"])`
t = `2.303/(0.087 "min"^-1) log (100/1)`
t = 52.93 min
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