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Question

The activation energy of the reaction:
A+B Products is 105.73 KJ/mol. At 40 C , the products are formed at the rate of 0.133 mol L1 min1 the rate of formation of products at 80 C will be


A
13.3 mol L1min1
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B
5.6 mol L1min1
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C
17.8 mol L1min1
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D
None of the above
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Solution

The correct option is A 13.3 mol L1min1
Let the rate law be defined as
At T1:r1=k1[A]x[B]y
At T2:r2=k2[A]x[B]y
r2=r1[k2k1]
Using Arrhenius equation, find k at 40 C
log k2k1=Ea2.303R(T2T1T1T2)
log k2k1=105.73×1032.303×8.31(40313×353)
logk2k1=2.0
k2k1=100
r2=0.133×100=13.3 mol L1 min1

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