Assertion If the activation energy of a reaction is zero, temperature will have no effect on the rate constant. Reason Lower the activation energy, faster is the reaction.

Question

Assertion If the activation energy of a reaction is zero, temperature will have no effect on the rate constant. Reason Lower the activation energy, faster is the reaction. (A) If both Assertion and Reason are true and Reason is the correct explanation of Assertion (B) If both Assertion and Reason are true but Reason is not the correct explanation of Assertion (C) If Assertion is true but Reason is false (D) If both Assertion and Reason are false

Tardigrade Admin · Accepted Answer

According to Arrhenius equation, k=Ae-Ea/RT when, Ea=0,k=A From the Arrhenius equation, it is also clear that lower the value of textE texta text, higher is the value of k and thus, faster is the reaction.

Q. Assertion If the activation energy of a reaction is zero, temperature will have no effect on the rate constant. Reason Lower the activation energy, faster is the reaction.

If both Assertion and Reason are true and Reason is the correct explanation of Assertion

If both Assertion and Reason are true but Reason is not the correct explanation of Assertion

If Assertion is true but Reason is false

If both Assertion and Reason are false

According to Arrhenius equation, $k = A e^{- E_{a} / RT}$ when, $E_{a} = 0, k = A$ From the Arrhenius equation, it is also clear that lower the value of $E_{a},$ higher is the value of k and thus, faster is the reaction.

Q. Assertion If the activation energy of a reaction is zero, temperature will have no effect on the rate constant. Reason Lower the activation energy, faster is the reaction.

If both Assertion and Reason are true and Reason is the correct explanation of Assertion

If both Assertion and Reason are true but Reason is not the correct explanation of Assertion

If Assertion is true but Reason is false

If both Assertion and Reason are false

According to Arrhenius equation, k=Ae−Ea​/RT when, Ea​=0,k=A From the Arrhenius equation, it is also clear that lower the value of Ea​, higher is the value of k and thus, faster is the reaction.

According to Arrhenius equation, $k = A e^{- E_{a} / RT}$ when, $E_{a} = 0, k = A$ From the Arrhenius equation, it is also clear that lower the value of $E_{a},$ higher is the value of k and thus, faster is the reaction.