NCERT Class XII Chemistry
Chapter - Chemical Kinetics
Questions with Solutions

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Question : 11
Total: 39
The following results have been obtained during the kinetic studies of the reaction :
2A + B → C + D
 Experiment  [A]/ mol L1  [B]/ mol L1  Initial rate of formation ofD/ mol L1 min1
 I  0.1  0.1  6. 0 × 103
 II  0.3  0.2  7.2. × 102
 III  0.3  0.4  2.88 × 101
 IV  0.4  0.1  2.40 × 102
Determine the rate law and the rate constant for the reaction.
Solution:  
Suppose order with respect to A is m and with respect to B is n.Then the rate law will be
Rate =k[A]m[B]n
Substituting the value of experiments I to IV, we get
Expt. I: Rate =6.0×103=k(0.1)m(0.1)n...(i)
Expt. II: Rate =7.2×102=k(0.3)m(0.2)n...(ii)
Expt. III: Rate =2.88×101=k(0.3)m(0.4)n ...(iii)
Expt. IV: Rate =2.4×102=k(0.4)m(0.1)n ...(iv)
Comparing equation (i) and equation (iv)
( Rate)I
(Rate) IV
=
6.0×103
2.4×102
=
k(0.1)m(0.1)n
k(0.4)m(0.1)n

or,
1
4
=
(0.1)m
(0.4)m
=(
1
4
)
m
m=1

Comparing equation(ii) and equation (iii)
( Rate)II
(Rate)III
=
7.2×102
2.88×101
=
k(0.3)m(0.2)n
k(0.3)m(0.4)n

or, (
1
2
)
2
=
(0.2)n
(0.4)n
=(
1
2
)
n
n=2

Rate law expression is : Rate =k[A][B]2.
The rate constant can be calculated from the given data of any experimentusing expression:
k=
Rate
[A][B]2

From Expt. I, k=
6.0×103
0.1×(0.1)2
=6.0

Rate constant k=6.0 mol2 L2min1
Unit of k,k=
Rate
[A][B]2

=
mol L1min1
( mol L1 ) ( mol L1 )2

= mol2 L2min1
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