Asked by bennett
The chemical reaction representing production of water gas is as follows:
C(s)+H2O(l)=CO(g)+H2(g)
calculate the enthalpy change in the production of 200L(at 500mmHg and 65degree celcius) of hydrogen by this reaction.
C(s)+H2O(l)=CO(g)+H2(g)
calculate the enthalpy change in the production of 200L(at 500mmHg and 65degree celcius) of hydrogen by this reaction.
Answers
Answered by
bobpursley
I think temperature will be a factor. Ignoring that
figure the moles of H2, and the moles of CO2, and the moles of H2O(l).
ChangeEnthalpy=HformationCO*molesCO -HeatformationH2O*molesH20
Now the problem. Heat of Formation is given in tables at some standard temperature, usually 273K. I hate to tell you to ignore that, as it is significant.
figure the moles of H2, and the moles of CO2, and the moles of H2O(l).
ChangeEnthalpy=HformationCO*molesCO -HeatformationH2O*molesH20
Now the problem. Heat of Formation is given in tables at some standard temperature, usually 273K. I hate to tell you to ignore that, as it is significant.
Answered by
bennett
so would i find the moles using the ideal gas law? PV=nRT
i didn't understand the heat of formation? could you explain a little more? thanks
i didn't understand the heat of formation? could you explain a little more? thanks
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