Using the following equation for the combustion of octane,calculate the heat associated with the formation of 100.0 g of carbon dioxide.The molar mass of octane is 114.33 g/mole.The molar mass of carbon dioxide is 44.0095 g/mole. 2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O ΔH°_rxn= -11018 kJ A) 12520 kJ B) 1564 kJ C) 1001 kJ D) 1391 kJ E) 11018 kJ

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Quizplus · Accepted Answer

First, we need to understand the given chemical equation, which represents the combustion of octane (C8H18) to produce carbon dioxide (CO2) and water (H2O), releasing energy (ΔH°rxn = -11018 kJ). The question asks for the heat associated with the formation of 100.0 g of CO2.From the balanced equation, 16 moles of CO2 are produced from the combustion of 2 moles of octane. The molar mass of CO2 is given as 44.0095 g/mole, so 100.0 g of CO2 is equivalent to $100.0 \, \text{g} \div 44.0095 \, \text{g/mole} = 2.272 \, \text{moles of CO2}$.Since 16 moles of CO2 are produced from the complete combustion of 2 moles of octane, which releases -11018 kJ, we can set up a proportion to find the heat associated with the formation of 2.272 moles of CO2:$\frac{-11018 \, \text{kJ}}{16 \, \text{moles of CO2}} = \frac{x \, \text{kJ}}{2.272 \, \text{moles of CO2}}$Solving for $x$, we find:$x = \frac{-11018 \, \text{kJ} \times 2.272 \, \text{moles of CO2}}{16 \, \text{moles of CO2}} = -1564 \, \text{kJ}$Therefore, the heat associated with the formation of 100.0 g of CO2 is -1564 kJ, indicating that this amount of energy is released.

Using the Following Equation for the Combustion of Octane,calculate the Heat