Calculate the half life of a first order reaction from their rate constants given below:
(a) $200 s^{- 1}$ ; (b) $2 m i n^{- 1}$ ; (c) $4 y e a r^{- 1}$ .

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Solution

(a) $t_{1 / 2} = \frac{0.693}{K} = \frac{0.693}{200} = 3.465 \times 10^{- 3} sec$
(b) $t_{1 / 2} = \frac{0.693}{K} = \frac{0.693}{2} = 3.465 \times 10^{- 1} m i n$
(c) $t_{1 / 2} = \frac{0.693}{K} = \frac{0.693}{4} = 1.733 \times 10^{- 1} y r$ .

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