A reactant with initial concentration 1.386 mol $l i t r e^{- 1}$ showing first order change takes 40 minutes to become half. If it shows zero-order change taking 20 minutes to becomes half under the similar conditions, the ratio, $\frac{K_{1}}{K_{0}}$ for the first order and zero order kinetics will be:

1.0 m o l l i t r e

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

0.5 m o l^{- 1} l i t r e

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

1.5 m o l l i t r e

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

None of these

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

Open in App

Solution

The correct option is B $0.5 m o l^{- 1} l i t r e$
For $1^{s t}$ order, $(t_{1 / 2})_{1} = \frac{0.693}{K_{1}}$
For zero order, $(t_{1 / 2})_{0} = \frac{a}{2 K_{0}}$
$∴ \frac{K_{1}}{K_{0}} \times \frac{1.386}{2 \times 0.693} = \frac{(t_{1 / 2})_{0}}{(t_{1 / 2})_{1}}$
$\frac{K_{1}}{K_{0}} = \frac{20 \times 2 \times 0.693}{40 \times 1.386} = 0.5 m o l^{- 1} l i t r e$

Suggest Corrections

Similar questions

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, 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:

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

A reactant with initial concentration 1.386 mol litre−1 showing first order change takes 40 minutes to become half. If it shows zero-order change taking 20 minutes to becomes half under the similar conditions, the ratio, K1K0 for the first order and zero order kinetics will be:

The correct option is B 0.5mol−1litreFor 1st order, (t1/2)1=0.693K1For zero order, (t1/2)0=a2K0∴K1K0×1.3862×0.693=(t1/2)0(t1/2)1K1K0=20×2×0.69340×1.386=0.5mol−1litre