Question

a first order reaction is 30% completed in 50 minutes at 300k calculate half life ?



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Answer 1

Explanation:

HEY MATE ......

$\frac{t1}{2} = \frac{0.693}{k} \\ \\ k = \frac{0.693}{ \frac{t1}{2} } \\ \\ therefore \\ \\ k1 = \frac{0.693}{50 \: min \: } = 0.01386 {min}^{ - 1} \\ \\ k2 = \frac{0.693}{10} = 0.693 {min}^{ - 1} \\ \\ \\ according \: to \: arrhenius \: eqn \: \\ \\ we \: get \: \\ \\ log \frac{k2}{k1} = \frac{e(a)}{2.303} \\ \\ ( \frac{1}{t1} - \frac{1}{t2)} \\ \\ k1 = 0.01386 \\ \\ k2 = 0.693 {min}^{ - 1} \\ \\ t1 = \frac{log(0.693 {min}^{ - 1} }{0.01386 {min}^{ - 1} } \\ \\ = \frac{e(a)}{2.303 \times (8.314)j \: mol} \\ \\ ( \frac{1}{300} k - \frac{1}{320} k)$

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