Answer:
[tex]4.974\times 10^{3} kJ[/tex] of energy is produced by combustion of 1.5 L of gasoline.
Explanation:
The average heat of combustion of liquid octane = [tex]\Delta H_{comb}=5400 kJ/mol[/tex]
Density of gasoline = 0.70 g/mL
Mass of gasoline with volume 1.5 L be m
V = Volume = 1.5 L = 1500 mL
[tex]Density=\frac{Mass}{Volume}[/tex]
[tex]0.70 g/ml=\frac{m}{1500 mL}[/tex]
[tex]m=0.70 g/mL\times 1500 mL=1050 g[/tex]
Since gasoline consists of a mixture of octanes. We can treat gasoline as a compound as octane.
Moles of octane = [tex]\frac{1050 g}{114 g/mol}=9.2105 mol[/tex]
Energy produced by combustion of 9.2105 mol of gasoline:
[tex]\Delta H_{comb}\times 9.2105 mol[/tex]
[tex]=5400 kJ/mol\times 9.2105 mol=49,736.84 kJ\approx 4.974\times 10^{3} kJ[/tex]
