Using the following equation for the combustion of octane, calculate the heat of reaction for 400.0 g of octane. The molar mass of octane is 114.33 g/mol. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O ΔH°rxn = -11018 kJ
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33 g/mol = 3.496 moles ≈ 3.5 moles Show more…
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Tianyu L.
Using the following equation for the combustion of octane, calculate the heat associated with the combustion of excess octane with 92 g of oxygen gas assuming complete combustion. The molar mass of octane is 114.33 g/mol. The molar mass of oxygen is 31.9988 g/mol. C8H18 + 25 O2 → 16 CO2 + 18 H2O ΔH°rxn = -11018 kJ
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The standard enthalpy of reaction for the combustion of octane is $\Delta_{\mathrm{r}} H^{\circ}=-5.48 \times 10^{3} \mathrm{kJ} / \mathrm{mol} \mathrm{C}_{8} \mathrm{H}_{18}(1)$ How much heat, in kilojoules, is liberated per gallon of octane burned? (Density of octane $=0.703 \mathrm{g} / \mathrm{mL}$ 1 gal = 3.785 L.)
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