Calculate the heat of reaction for the reduction of 1 mol of benzene with hydrogen at 179.0 °C to produce propane also at 179.0 °C. $\Delta H = $ __ kJ
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Use the given equations to determine the enthalpy of reaction when propyne, C3H4 (g), reacts with hydrogen gas, H2 (g), to form propane, C3H8 (g). C3H4 (g) + 2H2 (g) → C3H8 (g) (1) H2O (l) → H2 (g) + ½ O2 (g) ΔH° = +285.8 kJ (2) C3H4 (g) + 4O2 (g) → 3CO2 (g) + 2H2O (l) ΔH° = -1936.8 kJ (3) C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (l) ΔH° = -2219.2 kJ
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Propane is often used as a home fuel in areas where natural gas is not available. When $3.00$ grams of propane, $\mathrm{C}_{3} \mathrm{H}_{8}(g)$, are burned in excess oxygen in a bomb calorimeter that has a total heat capacity of $32.7 \mathrm{~kJ} \cdot \mathrm{K}^{-1}$, the temperature of the calorimeter increases by $4.25 \mathrm{~K} .$ Calculate the standard enthalpy of combustion in kilojoules per gram and kilojoules per mole of propane. Assume that $\Delta H_{\mathrm{rxn}} \approx \Delta U_{\mathrm{rxn}}$
Calculate the enthalpy of combustion of propane, $\mathrm{C}_{3} \mathrm{H}_{8}(g),$ for theformation of $\mathrm{H}_{2} \mathrm{O}(g)$ and $\mathrm{CO}_{2}(g) .$ The enthalpy of formation of propane is $-104 \mathrm{kJ} / \mathrm{mol}$ .
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