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

The first order rate constant for a certain reaction increases from 1.667×106 s1 at 727oC to 1.667×104 s1 at 1571oC. The rate constant at 1150oC, assuming constancy of activation energy over the given temperature range is
[Given:log19.91.299]

A
3.911×105s1
No worries! We‘ve got your back. Try BYJU‘S free classes today!
B
1.139×105s1
No worries! We‘ve got your back. Try BYJU‘S free classes today!
C
3.318×105s1
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
D
1.193×105s1
No worries! We‘ve got your back. Try BYJU‘S free classes today!
Open in App
Solution

The correct option is B 3.318×105s1
According to Arrehnius equation,
logk2k1=Ea2.303R[T2T1T1T2]
2.303logk2k1=EaR[T2T1T1T2]
2.303log[1.667×1041.667×106]=EaR[1184411000]
2.303×2=EaR×8441844×1000.......(1)
EaR=4.606×1844×1000844
2.303log[k31.667×106]=EaR×142310001423×1000
=EaR×4231423×1000........(2)
Dividing equation (2) by equation (1)
log[k31.667×106]=4231423×1000×1844×100844
log[k31.667×106]=2×423×18441423×844=1.299
On taking Antilog, k3=19.9
k3=19.9×1.667×106=3.318×105s1

flag
Suggest Corrections
thumbs-up
0
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Collision Theory
CHEMISTRY
Watch in App
Join BYJU'S Learning Program
CrossIcon