Use standard enthalpies of formation to calculate ΔH°_rxn for each reaction. a. C₂H₄(g) + H₂(g) → C₂H₆(g)

Verified step by step guidance

1. Identify the standard enthalpy of formation (ΔH_f°) for each compound involved in the reaction. These values are typically found in tables in chemistry textbooks or reliable online resources.
2. Write the balanced chemical equation for the reaction: \[ \text{C}_2\text{H}_4(g) + \text{H}_2(g) \rightarrow \text{C}_2\text{H}_6(g) \]
3. Apply Hess's Law, which states that the change in enthalpy for a reaction is the sum of the enthalpy changes for each step of the reaction. Use the formula: \[ \Delta H_{\text{rxn}}^\circ = \sum \Delta H_f^\circ(\text{products}) - \sum \Delta H_f^\circ(\text{reactants}) \]
4. Substitute the standard enthalpies of formation into the formula: \[ \Delta H_{\text{rxn}}^\circ = [\Delta H_f^\circ(\text{C}_2\text{H}_6(g))] - [\Delta H_f^\circ(\text{C}_2\text{H}_4(g)) + \Delta H_f^\circ(\text{H}_2(g))] \]
5. Calculate the value of \( \Delta H_{\text{rxn}}^\circ \) using the substituted values to find the enthalpy change for the reaction.

Key Concepts

Enthalpy of Formation

The standard enthalpy of formation (ΔH°f) is the change in enthalpy when one mole of a compound is formed from its elements in their standard states. It is a crucial value used in thermodynamics to calculate the heat changes in chemical reactions. Each substance has a specific ΔH°f, which can be found in tables, and is typically expressed in kilojoules per mole (kJ/mol).

Hess's Law

Hess's Law states that the total enthalpy change for a reaction is the same, regardless of the number of steps taken to achieve the reaction. This principle allows for the calculation of the enthalpy change of a reaction by summing the enthalpy changes of individual steps, making it possible to use standard enthalpies of formation to find ΔH°rxn for complex reactions.

Reaction Enthalpy (ΔH°rxn)

The reaction enthalpy (ΔH°rxn) is the overall change in enthalpy when reactants are converted to products at standard conditions. It can be calculated using the formula ΔH°rxn = ΣΔH°f(products) - ΣΔH°f(reactants). This value indicates whether a reaction is exothermic (releases heat, ΔH°rxn < 0) or endothermic (absorbs heat, ΔH°rxn > 0), which is essential for understanding the energy dynamics of chemical processes.