- #1
LogicX
- 181
- 1
For a process at constant pressure, ΔH=q.
My textbook clearly says that the only way that enthalpy can change is with a change in temperature. So ΔH=0. But q≠0 for an isothermal process.
I know that ΔU=0 for an isothermal process. So ΔH=0+Δ(PV)=Δ(nRT)=0
It really seems like ΔH should be zero for an isothermal process, but I can also make ΔH=q, which is not zero. What is the issue here?
My textbook clearly says that the only way that enthalpy can change is with a change in temperature. So ΔH=0. But q≠0 for an isothermal process.
I know that ΔU=0 for an isothermal process. So ΔH=0+Δ(PV)=Δ(nRT)=0
It really seems like ΔH should be zero for an isothermal process, but I can also make ΔH=q, which is not zero. What is the issue here?