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

2C4H10C8H18+H2. Given that bond energy of CC,CH are 347.3 and 414.2
kJ mol1 and the heat of formation of hydrogen atom is 217.55 kJ mol1. Find ΔH for the above reaction in kJ mol1.
(If ΔH=x, input the answer to the nearest integer as x9).

Open in App
Solution

For 2C4H10C8H18+H2;ΔH=?
ΔH= bond energy data used for the formation of bond + bond energy data used for dissociation of bond

ΔH=[7×E(CC)+18×E(CH)+E(HH)]+2[3×E(CC)+10×E(CH)]
ΔH=e(CC)+2×e(CH)e(HH)

Given, 12H2H;ΔH=217.55 kJ

e(HH)=2×217.55=435.10 kJ

ΔH=347.3+2×(414.2)1×(435.1)

ΔH=46.0 kJ mol1

Now,
469=5.115 kJ mol1

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