Under the same reaction conditions, initial concentration of 1.386 mol / dm 3 of a substance becomes half in 40 seconds and 20 seconds through first order and zero order kinetics, respectively. Ratio ((k1/k0)) of the rate constant for first order (k1) and zero order (k0) of the reaction is -

Question

Under the same reaction conditions, initial concentration of 1.386 mol / dm 3 of a substance becomes half in 40 seconds and 20 seconds through first order and zero order kinetics, respectively. Ratio ((k1/k0)) of the rate constant for first order (k1) and zero order (k0) of the reaction is - (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

K 1=(0.693/40) K 0=(1.386/2 × 20) ∴ ( K 1/ K 0)=(0.693/1.386)=(1/2)=0.5 ∴ 0.5

K1​=400.693​ K0​=2×201.386​ ∴K0​K1​​=1.3860.693​=21​=0.5 ∴0.5

$K_{1} = \frac{0.693}{40}$
$K_{0} = \frac{1.386}{2 \times 20}$
$∴ \frac{K _{1}}{K _{0}} = \frac{0.693}{1.386} = \frac{1}{2} = 0.5$
$∴ 0.5$