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Hydrogenation of double and triple bonds is an important industrial process. Calculate (in kJ) the standard enthalpy change ΔH° for the hydrogenation of ethyne (acetylene) to ethane using average bond enthalpies (use exam data sheet values).   H–C≡C–H(g) + 2H2(g) → H3C–CH3(g)

Hydrogenation of double and triple bonds is an important industrial process. Calculate (in kJ) the standard enthalpy change ΔH° for the hydrogenation of ethyne (acetylene) to ethane using average bond enthalpies (use exam data sheet values).   H–C≡C–H(g) + 2H2(g) → H3C–CH3(g)

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Hydrogenation of double and triple bonds is an important industrial process. Calculate (in kJ) the standard enthalpy change ΔH° for the hydrogenation of ethyne (acetylene) to ethane using average bond enthalpies (use exam data sheet values).

 

H–C≡C–H(g) + 2H2(g) → H3C–CH3(g)

 

### Key Constants and Enthalpy Changes #### Fundamental Constants: 1. **Atomic Mass Unit (AMU):** - \(1.66053873 \times 10^{-27} \, \text{kg}\) 2. **Rydberg Constant:** - \(1.097 \times 10^{7} \, \text{m}^{-1}\) 3. **Faraday's Constant:** - \(9.64853383 \times 10^{4} \, \text{C/mol}\) 4. **Ideal Gas Constant:** - \(0.0821 \, \text{L} \cdot \text{atm/(mol} \cdot \text{K)}\) - \(8.314 \, \text{kg} \cdot \text{m}^2/\text{sec}^2 \cdot \text{mol} \cdot \text{K}\) - \(8.314 \times 10^4 \, \text{g} \cdot \text{cm}^2/\text{sec}^2 \cdot \text{mol} \cdot \text{K}\) - \(6.24 \times 10^4 \, \text{cm}^3 \cdot \text{torr/(mol} \cdot \text{K)}\) - \(8.314 \, \text{J/(mol} \cdot \text{K)} \, = \, 8.314 \, \text{J/(mol} \cdot \text{K)}\) #### Enthalpy Changes Involving Water: **Per Mole:** - **Heat Capacity (g):** \(33.1 \, \text{J/mol} \cdot \text{K}\) - **Heat Capacity (l):** \(75.35 \, \text{J/mol} \cdot \text{K}\) - **Heat Capacity (s):** \(36.9 \, \text{J/mol} \cdot \text{K}\) - **Heat of Fusion (0°C):** \(5.99 \, \text{kJ/mol}\) - **Heat of Vaporization (100°C):** \(40.63 \, \text{kJ/mol}\) **Per Gram:
Transcribed Image Text:### Key Constants and Enthalpy Changes #### Fundamental Constants: 1. **Atomic Mass Unit (AMU):** - \(1.66053873 \times 10^{-27} \, \text{kg}\) 2. **Rydberg Constant:** - \(1.097 \times 10^{7} \, \text{m}^{-1}\) 3. **Faraday's Constant:** - \(9.64853383 \times 10^{4} \, \text{C/mol}\) 4. **Ideal Gas Constant:** - \(0.0821 \, \text{L} \cdot \text{atm/(mol} \cdot \text{K)}\) - \(8.314 \, \text{kg} \cdot \text{m}^2/\text{sec}^2 \cdot \text{mol} \cdot \text{K}\) - \(8.314 \times 10^4 \, \text{g} \cdot \text{cm}^2/\text{sec}^2 \cdot \text{mol} \cdot \text{K}\) - \(6.24 \times 10^4 \, \text{cm}^3 \cdot \text{torr/(mol} \cdot \text{K)}\) - \(8.314 \, \text{J/(mol} \cdot \text{K)} \, = \, 8.314 \, \text{J/(mol} \cdot \text{K)}\) #### Enthalpy Changes Involving Water: **Per Mole:** - **Heat Capacity (g):** \(33.1 \, \text{J/mol} \cdot \text{K}\) - **Heat Capacity (l):** \(75.35 \, \text{J/mol} \cdot \text{K}\) - **Heat Capacity (s):** \(36.9 \, \text{J/mol} \cdot \text{K}\) - **Heat of Fusion (0°C):** \(5.99 \, \text{kJ/mol}\) - **Heat of Vaporization (100°C):** \(40.63 \, \text{kJ/mol}\) **Per Gram:
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