Calculate the half-life of a first order reaction from their rate constants given below: (i) `200 s^(–1) (ii) 2 min^(–1) (iii) 4 years^(–1)`

Answer

`a. 3.47xx10^(-3)s`
`b . 0.35 mi n`
`c.` `0.173 years`

Explanation

For the first order reaction `, t_(1//2)=(0.693)/(k)`
`a.` `k=200s^(-1)`
`:. T_(1//2)=(0.693)/(200s)`
`=3.465xx10^(-3)s=3.47xx10^(-3)s`
`b. K=2 mi n^(-1)`
`t_(1//2)=(0.693)/(2 mi n)=0.3465mi n=0.35mi n`
`c. k=4 year^(-1)`
`t_(1//2)=(0.693)/(4)=0.173 years`