I. C(s) + O2(g) → CO2(g)

Question

ΔHf = −394 kJ

II. H2(g) + O2(g) → H2O(l)
ΔHf = −242 kJ

III. 2C(s) + 3H2(g) → C2H6(g)
ΔH =−84 kJ

The combustion of C2H6 is shown by the following equation:

C2H6(g) + O2(g) → 2CO2(g) + 3H2O(l)

Which option correctly gives the enthalpy of combustion of 0.2 moles of C2H6(g)?

I came up with -286 kJ, is this correct?

Answer 1

In the future please show how you cam up with this answer. Yes, -286 is correct but I spent considerable time putting all of this together to work the problem and to check your answer. I could hve checked your equatiions much faster and helped others.