Question

The half life period of a first order reaction is $100$ seconds. Its rate constant is:

• A. $0.693se{c}^{-1}$
• B. $6.93\times {10}^{-3}se{c}^{-1}$
• C. $6.93\times {10}^{-2}se{c}^{-1}$
• D. None of these
  

Answer 1

Answer: (B)

$6.93\times {10}^{-3}se{c}^{-1}$

For the first order reaction, the rate constant $k=\frac{0.693}{t_{1/2}}=\frac{0.693}{100s}=6.93\times {10}^{-3}se{c}^{-1}$

Hence, the correct option is $\text{B}$