Assertion :The reciprocal of time in which $63$ % of the reactant is converted to the product is equal to the rate constant of first-order reaction. Reason: The rate constant for first order reaction depends on initial concentration of reactants.

Both Assertion and Reason are correct and Reason is the correct explanation for Assertion

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

Both Assertion and Reason are correct, but Reason is not the correct explanation for Assertion

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

Assertion is correct, but Reason is incorrect

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

Assertion is incorrect, but Reason is correct

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

Open in App

Solution

The correct option is C Assertion is correct, but Reason is incorrect
For 1st order reaction,
$a_{t} = a_{0} e^{- k t}$
given that $a_{t} = (1 - 0.63) a_{0} = 0.37 a_{0}$
$0.37 = e^{- k t}$
kt=1 or $k = \frac{1}{t}$
Also, $k = A e^{- \frac{E a}{R T}}$
rate constant does not depend on initial concentration of reactants.

Suggest Corrections

Similar questions

Assertion (A) The enthalpy of reaction remains constant in the presence of a catalyst.

Reason (R) A catalyst participating in the reaction forms different activated complex and lowers down the activation energy but the difference in enrgy of reactant and product remains the same.

(a) Both assertion and reason are correct and the reason is correct explanation of assertion
(b) Both assertion and reason are correct, but reason does not explain assertion.
(c) Assertion is correct, but reason is incorrect
(d) Both assertion and reason are incorrect
(e) Assertion is incorrect but reason is correct.

Assertion (A) Order and molecularity are same.

Reason (R) Order is determined experimentally and molecularity is the sum of the stoichimetric coeffcient of rate determining elementary step.

Assertion (A) Order of the reaction can be zero or fractional.

Reason (R) We cannot determine order from balanced chemical equation.

Assertion (A) Rate constant determined from Arrhenius equation are fairly accurate for simple as well as complex molecules.

Reason (R) Reactant molecules undergo chemical change irrespective of their orientation during collision.

Q. Assertion: The compressibility factor for

H_{2}

and

H e

(1 + \frac{P b}{R T})

Reason: The compressibility factor for

H_{2}

and

H e

can be derived from Van der Waal's equation.

Join BYJU'S Learning Program

Assertion :The reciprocal of time in which 63% of the reactant is converted to the product is equal to the rate constant of first-order reaction. Reason: The rate constant for first order reaction depends on initial concentration of reactants.

The correct option is C Assertion is correct, but Reason is incorrectFor 1st order reaction,at=a0e−ktgiven that at=(1−0.63)a0=0.37a00.37=e−ktkt=1 or k=1tAlso, k=Ae−EaRTrate constant does not depend on initial concentration of reactants.

Assertion :The reciprocal of time in which $63$ % of the reactant is converted to the product is equal to the rate constant of first-order reaction. Reason: The rate constant for first order reaction depends on initial concentration of reactants.