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Question

Match the column I with column II and mark the appropriate choice.

Column IColumn II
(A) Zero order(i) logk2k1=Ea2.303R[T2T1T1T2]
(B) First order(ii) ΔH>0
(C) Endothermic reaction(iii) k=2.303tlog[A]0[A]
(D) Activation energy(iv) k=1t([A]0[A])

934490_c2c0a6152ec5404694498ba4718d0f2b.png

A
(A)(iv),(B)(iii),(C)(ii),(D)(i)
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B
(A)(i),(B)(ii),(C)(iii),(D)(iv)
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C
(A)(ii),(B)(iii),(C)(iv),(D)(i)
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D
(A)(iii),(B)(iv),(C)(i),(D)(ii)
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Solution

The correct option is D (A)(iv),(B)(iii),(C)(ii),(D)(i)
(A) For zero order reaction, the integrated rate law equation is K=1t([A]0[A])

(B) For first order reaction, the integrated rate law equation is
K=2.303t log ([Ao][A])

(C) ΔH>0

(D) Activation Energy (EA)

K=AeEa/RT

For two temperatures, it can be written as

log(k2k1)=Ea2.303R[T2T1T1T2]

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