Given that Δ_fH°[CO(g)] = -110.5 kJ/mol and Δ_fH° [COCl₂(g)] = -219.1 kJ/mol,what is the enthalpy of reaction for the formation of phosgene,COCl₂ from carbon monoxide,CO,and chlorine gas,Cl₂(g)? A)+110.5 kJ /mol B)-110.5 kJ/mol C)+329.6 kJ /mol D)-108.6 kJ/mol E)-219.1 kJ/mol

Question

Quizplus · Accepted Answer

The enthalpy of reaction for the formation of phosgene (COCl2) from CO and Cl2 can be calculated using the given formation enthalpies. The reaction is CO(g) + Cl2(g) → COCl2(g). The enthalpy change for the reaction (ΔH°rxn) is the sum of the formation enthalpies of the products minus the sum of the formation enthalpies of the reactants. Given ΔHf°[COCl2(g)] = -219.1 kJ/mol and ΔHf°[CO(g)] = -110.5 kJ/mol, and knowing that the formation enthalpy of elemental Cl2(g) is 0 (since it's in its standard state), ΔH°rxn = ΔHf°[COCl2(g)] - (ΔHf°[CO(g)] + ΔHf°[Cl2(g)]). This simplifies to -219.1 kJ/mol - (-110.5 kJ/mol) = -108.6 kJ/mol.

Given That ΔfH°[CO(g)] = -110

Given That Δ_fH°[CO(g)] = -110