Write A Balanced Equation For The Combustion Of C9H20(l) (nonane ...

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Step 1: Write the balanced chemical equation for the combustion of C9H20(l): C9H20(l) + 14O2(g) -> 9CO2(g) + 10H2O(l) Show more…

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Enthalpy of Combustion - Alkanes Write a balanced equation for the combustion of C9H20(l) (nonane) - i.e. its reaction with O2(g) forming the products CO2(g) and H2O(l). Given the following standard heats of formation: ΔHf° of CO2(g) is -393.5 kJ/mol ΔHf° of H2O(l) is -286 kJ/mol ΔHf° of C9H20(l) is -229.0 kJ/mol What is the standard heat of reaction (ΔH°) for the combustion reaction of C9H20(l)? 1 pt Calculate the difference, ΔH - ΔE = Δ(PV) for the combustion reaction of 1 mole of nonane. (Assume standard state conditions and 298 K for all reactants and products.)

Adi S.

For the unbalanced combustion reaction shown, $1 \mathrm{~mol}$ of ethanol, $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH},$ releases $1370 \mathrm{~kJ}:$ $$ \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}+\mathrm{O}_{2} \longrightarrow \mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O} $$ (a) Write a balanced equation for the combustion reaction. (b) What is the sign of $\Delta H$ for this reaction? (c) How much heat (in kilocalories) is released from the combustion of $5.00 \mathrm{~g}$ of ethanol? (d) How many grams of $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$ must be burned to raise the temperature of $500.0 \mathrm{~mL}$ of water from $20.0^{\circ} \mathrm{C}$ to $100.0^{\circ} \mathrm{C} ?$ (The specific heat of water is $4.184 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C}$ See Section 1.11.) (e) If the density of ethanol is $0.789 \mathrm{~g} / \mathrm{mL},$ calculate the combustion energy of ethanol in kilojoules/milliliter.

The equation for the combustion of $\mathrm{CH}_{4}$ (the main component of natural gas) is shown below. How much heat is produced by the complete combustion of $237 \mathrm{g}$ of $\mathrm{CH}_{4} ?$ $$\begin{array}{r}\mathrm{CH}_{4}(g)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g) \\&\Delta H_{\mathrm{rxn}}=-802.3 \mathrm{kJ} \end{array}$$

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