🤓 Based on our data, we think this question is relevant for Professor Cheek's class at AUSTINCC.

Solution: Using Hess' Law, calculate the enthalpy of formation for C 3H8(g) using the following thermodynamic data.C(s) + O2(g) → CO2(g) ΔH = -393.5 kj/molH2(g) + 1/2O2(g) → H2O(I) ΔH = -285.8 kj/molC3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(I) ΔH = 2199.0 kJ/mol

Problem

Using Hess' Law, calculate the enthalpy of formation for C 3H8(g) using the following thermodynamic data.

C(s) + O2(g) → CO2(g) ΔH = -393.5 kj/mol

H2(g) + 1/2O2(g) → H2O(I) ΔH = -285.8 kj/mol

C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(I) ΔH = 2199.0 kJ/mol