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E2C.7(b) Calculate A,H and AU at 298 K and AH at 427 K for the (g), Hus hydrogenation of ethyne (acetylene) to ethene (ethylene) from the enthalpy of combustion and heat capacity data in Tables 2C.3 and 2C.4 of the Resource section. Assume the heat capacities to be constant over the temperature: e range involved. 16911 91 art of anibro

E2C.7(b) Calculate A,H and AU at 298 K and AH at 427 K for the (g), Hus hydrogenation of ethyne (acetylene) to ethene (ethylene) from the enthalpy of combustion and heat capacity data in Tables 2C.3 and 2C.4 of the Resource section. Assume the heat capacities to be constant over the temperature: e range involved. 16911 91 art of anibro

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Chapter1: Chemical Foundations
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Only calculate at 298K ignore heat capacity statements
**Exercise E2C.7(b): Calculation of Thermodynamic Properties** Calculate the standard enthalpy change (\(\Delta H^\circ\)) and the standard internal energy change (\(\Delta U^\circ\)) at 298 K, and \(\Delta H^\circ\) at 427 K for the hydrogenation of ethyne (acetylene) to ethene (ethylene). Use the enthalpy of combustion and heat capacity data provided in Tables 2C.3 and 2C.4 of the Resource section. Assume the heat capacities remain constant across the temperature range considered.
Transcribed Image Text:**Exercise E2C.7(b): Calculation of Thermodynamic Properties** Calculate the standard enthalpy change (\(\Delta H^\circ\)) and the standard internal energy change (\(\Delta U^\circ\)) at 298 K, and \(\Delta H^\circ\) at 427 K for the hydrogenation of ethyne (acetylene) to ethene (ethylene). Use the enthalpy of combustion and heat capacity data provided in Tables 2C.3 and 2C.4 of the Resource section. Assume the heat capacities remain constant across the temperature range considered.
**Table 2C.3: Standard Enthalpies of Formation and Combustion of Organic Compounds at 298 K** | Compound | ΔH⁰ₑ (kJ mol⁻¹) | ΔH⁰ₐ (kJ mol⁻¹) | |--------------------|----------------|-----------------| | Benzene, C₆H₆(l) | +49.0 | -3268 | | Ethane, C₂H₆(g) | -84.7 | -1560 | | Glucose, C₆H₁₂O₆(s)| -1274 | -2808 | | Methane, CH₄(g) | -74.8 | -890 | | Methanol, CH₃OH(l) | -238.7 | -721 | *More values are given in the Resource section.* **Explanation:** This table shows two important thermodynamic values for different organic compounds: - **ΔH⁰ₑ (Standard Enthalpy of Formation):** It indicates the energy change when one mole of a compound is formed from its elements in their standard states. - **ΔH⁰ₐ (Standard Enthalpy of Combustion):** It represents the energy change when one mole of a substance is burned in excess oxygen under standard conditions. Each compound is listed with its corresponding values for both enthalpy changes. Negative values indicate exothermic reactions, releasing energy to the surroundings.
Transcribed Image Text:**Table 2C.3: Standard Enthalpies of Formation and Combustion of Organic Compounds at 298 K** | Compound | ΔH⁰ₑ (kJ mol⁻¹) | ΔH⁰ₐ (kJ mol⁻¹) | |--------------------|----------------|-----------------| | Benzene, C₆H₆(l) | +49.0 | -3268 | | Ethane, C₂H₆(g) | -84.7 | -1560 | | Glucose, C₆H₁₂O₆(s)| -1274 | -2808 | | Methane, CH₄(g) | -74.8 | -890 | | Methanol, CH₃OH(l) | -238.7 | -721 | *More values are given in the Resource section.* **Explanation:** This table shows two important thermodynamic values for different organic compounds: - **ΔH⁰ₑ (Standard Enthalpy of Formation):** It indicates the energy change when one mole of a compound is formed from its elements in their standard states. - **ΔH⁰ₐ (Standard Enthalpy of Combustion):** It represents the energy change when one mole of a substance is burned in excess oxygen under standard conditions. Each compound is listed with its corresponding values for both enthalpy changes. Negative values indicate exothermic reactions, releasing energy to the surroundings.
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