From the following data for the reaction between A and B.
Calculate the following
(i) The order w.r.t. A and w.r.t. B
(ii) The rate constant at 300 K
(iii) The energy of activation
(iv) The pre-exponential factor
[e –22.18 = 2.3283 × 10 –10 , ln2 = 0.693]
Text Solution
Verified by ExpertsCHECK THE SOLUTION.
(i) 2, 1 (ii) 2.67 × 10 8 mol –2 litre 2 sec –1 (iii) 55.13 kJ mol –1 (iv) 1.147 × 10 18 mol –2 litre 2 sec –1
Sol. (i) r = K [A] x [B] Y
From (2 & 3) equation
= 
= 
= 
⇒ x = 2
From 1 & 2
= 
= 
= 
⇒ y = 1
(ii) Rate constant at 300 K
r = K [A] x [B] Y = 5 × 10 –4 ⇒ K 300 = 
K 300 = 
= 
⇒ K 300 = 2.67 × 10 8 Mole –2 Lit 2 sec –1
(iii) log 
= 
⇒ K 320 = 
= 
= 10.67 × 10 +8
log 
= 
× 
0.60 = 
(iv) K = A e – 
E a = 55.13 kJ/mole
2.67 × 10 8 = A e – 
= A e – 22.18
2.67 × 10 8 = A × 2.3283 × 10 –10 ,
A = 
= 1.147 × 10 18
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