Question

What mass of carbon dioxide is produced from the complete combustion of 2.40×10−3 g of methane?

Answer 1

Let us first write the combustion reaction for methane

CH₄ + 2O₂ ---> CO₂ + 2H₂O

Data given: Weight of Methane = 2.40 *10^-3 grams

As per the question complete combustion takes place, hence methane will completely react to form carbon dioxide and water

Molar mass of Methane = 16 grams/mole

Moles of methane = weight of methane/molar mass of methane = 2.40 *10^-3/ 16   = 1.5*10^-4 moles

As per the reaction stoichometry

1 mole of CH₄ = 1 mole of CO₂

Hence moles of CO₂ produced will be same as mole of methane reacted, that is , 1.5*10^-4 moles

Moles of CO₂ produced =1.5*10^-4 moles

Molar mass of CO₂ = 12+32 = 44 grams/mole

weight of CO₂ = Moles of CO₂ *Molar mass of CO₂ = 1.5*10^-4 * 44 =6.6*10^-3 grams

Hence, Mass of carbon dioxide produced for complete combustion of 2.4*10^-3 grams of methane is 6.6*10^-3 grams