# What volume of carbon dioxide, at 1 atm pressure and 112°C, will be produced when 80.0 grams of methane is burned? Methane burns in air to produce carbon dioxide and water: CH4(g) + 2 O2(g) --> CO2(g) + H2O(l)

80 g of methane burns to produce carbon dioxide and water.

CH4 + 2 O2 --> CO2 + H2O

The molar mass of methane is 16 /mol. 80 g of methane is 5 moles. According to the chemical equation given, the combustion of methane leads to the formation of 5...

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80 g of methane burns to produce carbon dioxide and water.

CH4 + 2 O2 --> CO2 + H2O

The molar mass of methane is 16 /mol. 80 g of methane is 5 moles. According to the chemical equation given, the combustion of methane leads to the formation of 5 moles of CO2.

Assuming the pressure of 1 atm. and the temperature of 112 degree C are the conditions after combustion, we can calculate the volume using the ideal gas law.

P*V = n*R*T

V = n*R*T/P

here, the pressure P = 1 atm., the temperature T = 385 K, the amount of substance n = 5 mole and R = 0.08205746 L*atm/K*mol.

Substituting the values,

V = 5*0.08205746*385/1 = 157.85 L

The volume of carbon dioxide produced is 157.85 L

Approved by eNotes Editorial Team