1. Tardigrade
  2. Question
  3. Chemistry
  4. 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 -

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Q. 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 $\left(\frac{k_{1}}{k_{0}}\right)$ of the rate constant for first order $\left(k_{1}\right)$ and zero order $\left(k_{0}\right)$ of the reaction is -

Chemical Kinetics

Solution:

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