wiz-icon
MyQuestionIcon
MyQuestionIcon
1
You visited us 1 times! Enjoying our articles? Unlock Full Access!
Question

Consider activation energy of two reaction is differ by 50kJ/mol but they have equal expotential factor and same order of reaction. Then, calculate the log ratio of the rate constants of this reaction at 30C.
(R=8.314J K1mol1)

A
8.61
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
B
4×105
No worries! We‘ve got your back. Try BYJU‘S free classes today!
C
14.3
No worries! We‘ve got your back. Try BYJU‘S free classes today!
D
11.6
No worries! We‘ve got your back. Try BYJU‘S free classes today!
Open in App
Solution

The correct option is A 8.61
We know that,
log10k=log10AE2.303RT

So, log10k2=log10AE22.303RT....eqn(1)

and log10k1=log10AE12.303RT.....eqn(2)

Substracting equation (2) from (1), we get,

log10(k2k1)=(E1E2)2.303RT

log10(k2k1)=50×10002.303×8.314×303

log10 k2k1=8.61
Hence, (a) is correct.

flag
Suggest Corrections
thumbs-up
0
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Order and Molecularity of Reaction
CHEMISTRY
Watch in App
Join BYJU'S Learning Program
CrossIcon