Determine the change in enthalpy for the following reaction from the enthalpies of formation for the reactants and products.(C₂H₂CL₂ , + 4.27 kJ/mol; C₂ H₂ CL₄ , -155.6 kJ/mol)
CL₂ (g) + C₂ H₂ CL₂ (g) $\rightarrow$ C₂ H₂ CL₄ (g)

Question

Determine the change in enthalpy for the following reaction from the enthalpies of formation for the reactants and products.(C₂H₂CL₂ , + 4.27 kJ/mol; C₂ H₂ CL₄ , -155.6 kJ/mol)
CL₂ (g) + C₂ H₂ CL₂ (g)

\rightarrow

C₂ H₂ CL₄ (g)

Quizplus · Accepted Answer

The change in enthalpy ($\Delta H$) for a reaction can be calculated using the formula $\Delta H = \sum H_{\text{products}} - \sum H_{\text{reactants}}$. Given the enthalpy of formation for the product is -155.6 kJ/mol and the sum of the enthalpies of formation for the reactants is 4.27 kJ/mol, the change in enthalpy is $-155.6 kJ/mol - 4.27 kJ/mol = -159.87 kJ/mol$, which rounds to -159.9 kJ/mol, indicating an exothermic reaction.

Determine the Change in Enthalpy for the Following Reaction from the Enthalpies