Half life period of a first order reaction, A → product is 6.93 hour. What is the value of rate constant ?

Question

Half life period of a first order reaction, A → product is 6.93 hour. What is the value of rate constant ? (A) 1.596 h-1 (B) 0.1 h-1 (C) 4.802 h-1 (D) 10 h-1

Tardigrade Admin · Accepted Answer

We have the formula for half-life of a first order reaction, t1 / 2=(0.693/k) where, k= rate constant ∴ 6.93 h =(0.693/k) ⇒ k=(0.693/6.93 h ) k =0.1 h -1

Q. Half life period of a first order reaction, $A$ $\to$ product is $6.93$ hour. What is the value of rate constant ?

$1.596 h^{- 1}$

$0.1 h^{- 1}$

$4.802 h^{- 1}$

$10 h^{- 1}$

We have the formula for half-life of a first order reaction,

$t_{1/2} = \frac{0.693}{k}$

where, $k =$ rate constant

$∴ 6.93 h = \frac{0.693}{k}$

$\Rightarrow k = \frac{0.693}{6.93 h}$

$k = 0.1 h^{- 1}$

Q. Half life period of a first order reaction, A → product is 6.93 hour. What is the value of rate constant ?

1.596h−1

0.1h−1

4.802h−1

10h−1