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)
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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
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