Question

The rate of a first order reaction is $0.69\times {10}^{-2}mi{n}^{-1}$and the initial concentration is 0.5 mol/L. The half life period is

• A. 3000 s
• B. 0.33 s
• C. 50 s
• D. 100 s

Answer 1

The correct option is A 3000 s

$Rate=k\left[C\right]0.69X{10}^{-2}=k\left[0.5\right]or,k=\frac{0.69\times {10}^{-2}}{0.5}{t}_{\frac{1}{2}}=\frac{0.693}{K}=\frac{0.693\times 0.5}{0.69\times {10}^{-2}}{t}_{\frac{1}{2}}=50min=3000sec$