Under the same reaction conditions, initial concentration of 1.386 $m o l d m^{- 3}$ of a substance becomes half in 40 s amd 20 s through first order and zero order kinetics respectively. Ratio $(\frac{k_{1}}{k_{0}})$ of the rate constants for first order $(k_{1})$ and zero order $(k_{0})$ of the reaction is:

$0.5 m o l^{- 1} d m^{3}$

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

$1.0 m o l d m^{- 3}$

No worries! We‘ve got your back. Try BYJU‘S free classes today!

$1.5 m o l d m^{- 3}$

No worries! We‘ve got your back. Try BYJU‘S free classes today!

$2.0 m o l^{- 1} d m^{3}$

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is A
$0.5 m o l^{- 1} d m^{3}$

For first order reaction $t_{1 / 2} = \frac{I n 2}{k_{1}} = 40 s$ $\dots (i)$
For zero order reaction $t_{1 / 2} = \frac{[A]_{0}}{2 k_{0}} = 20 s$ $\dots (i i)$
$\Rightarrow E q . (i i) / (i) = \frac{1}{2} = \frac{[A]_{0}}{2 k_{0}} \times \frac{k_{1}}{I n 2}$
$\Rightarrow \frac{k_{1}}{k_{0}} = \frac{I n 2}{[A]_{0}} = \frac{0.693}{1.386} = 0.5$

Suggest Corrections

Similar questions

Under the same reaction conditions, initial concentration of 1.386 $m o l d m^{- 3}$ of a substance becomes half in 40 s amd 20 s through first order and zero order kinetics respectively. Ratio $(\frac{k_{1}}{k_{0}})$ of the rate constants for first order $(k_{1})$ and zero order $(k_{0})$ of the reaction is:

Q. Under the same reaction conditions, initial concentration of

1.386

m o l

{d m}^{- 3}

of a substance becomes half in

40

seconds and

20

seconds through first order and zero order kinetics respectivley. Ratio

(\frac{k_{1}}{k_{0}})

of the rate constant for first order

(k_{1})

and zero order

(k_{0})

of the reaction is:

Under the same reaction conditions, the initial concentration of 1.386 mol $d m^{- 3}$ of a substance becomes half in 40 seconds and 20 seconds through first order and zero order kinetics, respectively.

The ratio $(k_{1} / k_{0}$ ) of the rate constants for first order $(k_{1})$ and zero order $(k_{0})$ of the reaction is

Under the same reaction conditions, the initial concentration of 1.386 mol $d m^{- 3}$ of a substance becomes half in 40 s and 20 s through first order and zero order kinetics, respectively.

The ratio $(k_{1} / k_{0}$ of the rate constants for first order $(k_{1})$ and zero order $(k_{0})$ of the reaction is

Join BYJU'S Learning Program

Under the same reaction conditions, initial concentration of 1.386 mol dm−3 of a substance becomes half in 40 s amd 20 s through first order and zero order kinetics respectively. Ratio (k1k0) of the rate constants for first order (k1) and zero order (k0) of the reaction is:

The correct option is A 0.5 mol−1 dm3 For first order reaction t1/2=In 2k1=40 s ⋯(i) For zero order reaction t1/2=[A]02k0=20 s ⋯(ii) ⇒Eq.(ii)/(i)=12=[A]02k0×k1In 2 ⇒k1k0=In 2[A]0=0.6931.386=0.5