CameraIcon
CameraIcon
SearchIcon
MyQuestionIcon
MyQuestionIcon
1
You visited us 1 times! Enjoying our articles? Unlock Full Access!
Question

The following results have been obtained during the kinetic studies of the reaction, 2A+BC+D
Experiment[A] mol L1[B] mol L1Initial rate of formation ofD/mol L1 minI0.10.16.0×103II0.30.27.2×102III0.30.42.88×101IV0.40.12.40×102
Determine the rate law and the rate constant for the reaction.

Open in App
Solution

Rate law may be expressed as
Rate =k[A]x[B]y
(Rate)1=6.0×103=k(0.1)x(0.1)y(i)(Rate)2=7.2×102=k(0.3)x(0.2)y(ii)(Rate)3=2.88×101=k(0.3)x(0.4)y(iii)(Rate)4=2.40×102=k(0.4)x(0.1)y(iv)(Rate)1(Rate)4=6.0×1032.40×102=k(0.1)x(0.1)yk(0.4)x(0.1)y
or 14=(0.1)x(0.4)x=(14)x
x=1(Rate)2(Rate)3=7.2×1022.88×101=k(0.3)x(0.2)yk(0.3)x(0.4)y
or 14=(0.2)y(0.4)y=(12)y
y=2
Rate law expression is given by
Rate =k[A][B]2
Rate constant k can be determined by placing the values of A, B and rate of formation of D. By taking the values from experiment II.
Rate =k[A][B]2k=Rate[A][B]2=7.2×102 mol L1 min1(0.3 mol L1)(0.2 mol L1)2=6.0 mol2 L2 min1k=6.0 mol2 L2 min1


flag
Suggest Corrections
thumbs-up
32
Join BYJU'S Learning Program
Join BYJU'S Learning Program
CrossIcon