Calculate the standard enthalpy change of formation of butane, C4H10.
Use the data:
∆Hc (graphite, C) = -393 kJ/mol
∆Hc (hydrogen, H2) = -286 kJ/mol
∆Hc (butane, C4H10) = -2877 kJ/mol
My main problem is getting the balanced equation. If I have that for the formation of butane, I think I could do it from there.
Creating a energy cycle and Hess's cycle Watch
- Thread Starter
- 19-01-2015 22:48
- 19-01-2015 23:37
I think the equation you're looking for may be:
4C(g) + 5H2(g) --------------> C4H10