Determine $\Delta$H for the following reaction:C₂H₂₍_g) + 2 H_2(g) $\rarr$ C₂H_6(g);$\Delta$H =? given the following heats of combustion: C₂H₂ + 5/2 O₂ $\rarr$ 2 CO₂ + H₂O $\quad $$\Delta$H = -1300 kJ H₂ + 1/2 O₂ $\rarr$ H₂O $\quad $$\quad $$\quad $$\quad $$\quad $$\Delta$H = -286 kJ C₂H₆ + 7/2 O₂ $\rarr$ 2 CO₂ + 3 H₂O $\quad $$\Delta$H = -1560 kJ ($\Delta$H_rxn = $\Delta$H_products- $\Delta$H_reactants; $\Delta$H_rxn = Bond broken - Bonds made)

Question

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The correct $\Delta H$ for the reaction can be calculated using Hess's Law, which involves manipulating and combining the given heats of combustion to match the target reaction. The given heats of combustion are for the combustion of $C_2H_2$, $H_2$, and $C_2H_6$. By reversing and adjusting the coefficients of these reactions, we can find the heat of the target reaction. The calculation involves using the given $\Delta H$ values for the combustion reactions, adjusting for the stoichiometry of the target reaction, and ensuring the correct sign (positive or negative) based on the direction of the reaction.

Determine Δ\DeltaΔ H for the Following Reaction:C2H2(g) + 2 H2(g) →\rarr→ C2H6(g); Δ\DeltaΔ

Determine $\Delta$ H for the Following Reaction:C₂H₂₍_g) + 2 H_2(g) $\rarr$ C₂H_6(g); $\Delta$