🤓 Based on our data, we think this question is relevant for Professor Bedlek-Anslow's class at SEMINOLESTATE.

Calculate ΔHrxn for the following reaction:

CH_{4}(g) + 4Cl_{2}(g) → CCl_{4}(g) + 4HCl(g)

Use the following reactions and given ΔH′s.

C(s) + 2H_{2}(g) → CH_{4}(g) ΔH = −74.6kJ

C(s) + 2Cl_{2}(g) → CCl_{4}(g) ΔH = −95.7kJ

H_{2}(g) + Cl_{2}(g) → 2HCl(g) ΔH = −184.6kJ

For Hess's Law, we need to get the corresponding equation below using the sequence of reactions given

By manipulating the reaction, either reversing them or multiplying/dividing them to a certain factor, we can get to the target equation as well as the total enthalpy

CH_{4}(g) + 4Cl_{2}(g) → CCl_{4}(g) + 4HCl(g)

C(s) + 2H_{2}(g) → CH_{4}(g) ΔH = −74.6kJ (needs to reverse)

C(s) + 2Cl_{2}(g) → CCl_{4}(g) ΔH = −95.7kJ (retain)

H_{2}(g) + Cl_{2}(g) → 2HCl(g) ΔH = −184.6kJ (multiply by 2 to get 4Cl_{2} and cancel out 4 HCl and 4 H_{2})