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

The heat liberated on complete combustion of 7.8g benzene is 327 KJ. This heat has been measured at constant volume and at 270 C. What is the heat of combustion of benzene at constant pressure at 270 C (R = 8.3 J mol1 K1)


A

-3273.735 KJ

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
B

-3274.735 KJ

No worries! We‘ve got your back. Try BYJU‘S free classes today!
C

-3275.735 KJ

No worries! We‘ve got your back. Try BYJU‘S free classes today!
D

-3270.735 KJ

No worries! We‘ve got your back. Try BYJU‘S free classes today!
Open in App
Solution

The correct option is A

-3273.735 KJ


Let us first write the chemical reaction which is

C6H6(l)+152O2(g)6CO2(g)+3H2O(l)

Δng = number of moles of gaseous products - number of moles of gaseous reactants

Δng = 6152 = 32

Now ΔU per mole = 327×787.8=3270KJ

ΔH=ΔU+ΔnRT=3270+(32)(8.3)(300)103

= 3270+(32)(8.3)(300)103

ΔH=3273.735KJ


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