Use the following data to calculate the standard enthalpy of formation of pentane, C5H12(l)?
C5H12(l) + 8 O2 (g) -> 5 CO2 (g) + 6 H2O (l) delta H=-3535.9 kJ/mol

delta Hf of CO2 (g) = -393.5 kJ/mol

delta Hf of H2O (l) = -285.8 kJ/mol

please show all work

Explanation:

C₅H₁₂(l) + 8O₂(g) ⟶ 5CO₂(g) + 6H₂O(l); ΔᵣH = -3535.9 kJ·mol⁻¹

The formula for calculating the enthalpy change of a reaction by using the enthalpies of formation of reactants and products is

Let x = the heat of formation of pentane

                            C₅H₁₂(l) + 8O₂(g) ⟶ 5CO₂(g) + 6H₂O(l)

ΔH°f/kJ·mol⁻¹:            x                          -393.5      -285.8

-57.12

Explanation:

i used a calculator :)