2H2(g)+O2(g)=@H2O(l)

Calculate the volume of hydrogen gas at 25 celcius and 1.00atm required to produce an amount of energy equivalent to that produced by the combustion of a gallon of octane (C8H18). The density of octane is 2.66kg/gal, and its standard enthalpy of formation is -249.9kJ/mol.

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The complete combustion of octane, C8H18, a component of gasoline, proceeds as is shown below. 2 C8H18(l) + 25 O2(g) 16 CO2(g) + 18 H2O(l)

(a) How many moles of O2 are needed to burn 1.15 mol of C8H18?

(b) How many grams of O2 are needed to burn 1.40 g of C8H18?

(c) Octane has a density of 0.692 g/mL at 20Â°C. How many grams of O2 are required to burn 4.35 gal. of C8H18? 1 gal = 3.79 L.

The complete combustion of octane, C₈H₁₈, a component of gasoline, proceeds as follows:
2 C₈H₁₈(l) + 25 O₂(g) 16 CO₂(g) + 18 H₂O(g)

(a) How many moles of O₂ are needed to burn 1.50 mol of C₈H₁₈?
(b) How many grams of O₂ are needed to burn 10.0 g of C₈H₁₈?
(c) Octane has a density of 0.692 g/mL at 20 °C. How many grams of O₂ are required to burn 15.0 gal of C₈H₁₈ (the capacity of an average fuel tank)?
(d) How many grams of CO₂ are produced when 15.0 gal of C₈H₁₈ are combusted?