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Q.

Two reactions  R1  and  R2  have identical pre-exponential factors. Activation energy of  R1 exceeds that of  R2 by 10 kJ mol-1. If  K1  and  K2  are rate constants for reactions R₁ and R₂ respectively at 300 K, then  ln ( K2/K1 ) is equal to (R = 8.314 J mol1 K-1)

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a

8

b

12

c

6

d

4

answer is B.

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Detailed Solution

According to the arrhenius equation,
 k=AeEa/RT
For reaction  R1;k1=AeEa1/RT
In k1  = In  AEa1RT
For reaction  R2;k2=AeEa2/RT
In  k2  = In  AEa1RT
Now , in  (k2k1)=Ea1RTEa2RT=Ea1Ea2=RTΔEaRT=10×1038.314×300=4

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