Assertion: For a reaction `A(g) rarr B(g)` `-r_(A) = 2.5 P_(A)` at `400 K` `r_(A) = 2.5 P_(A)` at `600 K` activation energy is `4135 J//"mol"`. Reason: Since for any reaction, values of rate constant at two different temp is same therefore activation energy of the reaction is zero.A. If both assertion and reason are true and the reason is the correct explanation of the assertion.B. If both assertion and reason are true but the reason is not the correct explanation of the assertion.C. If assertion is true but reason is false.D. If assertion is false but reason is true.

Assertion: For a reaction `A(g) rarr B(g)` `-r_(A) = 2.5 P_(A)` at `40

1.	Assertion: For a reaction `A(g) rarr B(g)` `-r_(A) = 2.5 P_(A)` at `400 K` `r_(A) = 2.5 P_(A)` at `600 K` activation energy is `4135 J//"mol"`. Reason: Since for any reaction, values of rate constant at two different temp is same therefore activation energy of the reaction is zero.A. If both assertion and reason are true and the reason is the correct explanation of the assertion.B. If both assertion and reason are true but the reason is not the correct explanation of the assertion.C. If assertion is true but reason is false.D. If assertion is false but reason is true.
Answer» Correct Answer - B `-r_(A) = [2.5 R(400)]C_(A)` (at `400 K`) `-r_(A) = [2.5 R(600)]C_(A)` (at `600 K`) `log((6)/(4)) = (E_(a))/(2.303 R) [(1)/(400) - (1)/(600)]` `E_(a) = 4135` So Assertion and Reason both are correct and reason is not the correct explanation.

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