Question

For a gaseous phase reaction 2A + B + 2AB, the
following rate data was obtained at 300 K.
The rate constant for the reaction is
(1) 0.5 mol-1 min-1 litre.
(2) 0.8 mol-1 min-1 litre

(3) 1.5 mole-1 min-1 litre

(4) 2 mol-1 min-1 litre​

Answer 1

Rate constant for the reaction is 0.8 litre mol-1 time-1

Explanation:

Rate of reaction "R" = K [A]^m [B]^n

where m and n are order of the reaction.

Rate of disappearance of B2 = k[A]^m[B]^n

r1 =1.8 x 10-3 = k[0.015]m[0.15]n

r2=1.08  x 10-2 =k[0.09]m[0.15]n

r3=5.4  x 10-3 =k[0.15]m[0.45]n

Now dividing r1/r2  

(1.8 x  10-3/1.08 x 10-2)  =  k[0.015/0.09]m

Thus we get m=1

Similarly dividing r1/r3 we get n=1

Rate of disappearance of B2 =k[0.015]^1[0.15]^1

1.8 x 10-3=k[0.015]^1[0.15]^1  

Rate constant (k) = 0.8 litre mol-1 time-1

Thus rate constant for the reaction is 0.8 litre mol-1 time-1

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