Find $\Delta$H^$\circ$_rxn for the reaction CH₄(g) + 2O₂(g) $\rarr$CO₂(g) + 2H₂O(l).[$\Delta$H^$\circ$_f (CH₄(g)) = -74.8 kJ/mol; $\Delta$H^$\circ$_f (CO₂(g)) = -393.5 kJ/mol; $\Delta$H^$\circ$_f (H₂O(l)) = -285.5 kJ/mol] A) -879.7 kJ/mol B) -889.7 kJ/mol C) -899.7 kJ/mol D) -909.7 kJ/mol E) None of the above

Question

Quizplus · Accepted Answer

The standard enthalpy change for the reaction ($\Delta H_{rxn}^\circ$) can be calculated using the standard enthalpy of formation ($\Delta H_f^\circ$) values for the reactants and products. The formula is: $\Delta H_{rxn}^\circ = \sum (\Delta H_f^\circ \text{ of products}) - \sum (\Delta H_f^\circ \text{ of reactants})$.For the given reaction: $\Delta H_{rxn}^\circ = [(-393.5) + 2(-285.5)] - [(-74.8) + 2(0)] = -393.5 - 571 + 74.8 = -889.7 \, \text{kJ/mol}$. Note: The enthalpy of formation for $O_2(g)$ is zero because it is in its standard state.

Find Δ\DeltaΔ H ∘\circ∘ rxn for the Reaction CH4(g) + 2O2(g) →\rarr→ CO2(g) + 2H2O(l)

Find $\Delta$ H^$\circ$_rxn for the Reaction CH₄(g) + 2O₂(g) $\rarr$ CO₂(g) + 2H₂O(l)