wiz-icon
MyQuestionIcon
MyQuestionIcon
7
You visited us 7 times! Enjoying our articles? Unlock Full Access!
Question

The heat of combustion of gaseous methane (CH4) at constant volume is measured in a bomb calorimeter at 298 K and is found to be 885.4kJmol1 . Find the value of enthalpy change.

Open in App
Solution

Combustion of CH4-
CH4(g)+2O2(g)CO2(g)+2H2O(l)
Δng=nPnR=1(2+1)=2
Given:- ΔU=885.4kJ/mol
T=298K
As we know that,
ΔH=ΔU+ΔngRT
ΔH=885.4+(2×8.314×103×298)
ΔH=885.44.95=890.05kJ/mol
Hence the value of enthalpy change is 890.05kJ/mol.

flag
Suggest Corrections
thumbs-up
0
similar_icon
Similar questions
View More
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Calorimetry
PHYSICS
Watch in App
Join BYJU'S Learning Program
CrossIcon