When methane (CH4) burns, it reacts with oxygen gas to produce carbon dioxide and water. The unbalanced equation for this reaction is CH4(g) + O2(g) → CO2(g) + H2O(g). This type of reaction is referred to as a complete combustion reaction. What mass of carbon dioxide (CO2) is produced when 16 grams of methane is completely combusted?

• A. 88 grams
• B. 32 grams
• C. 22 grams
• D. 44 grams

Answer: (D)

Verified step by step guidance

1. Start by writing the balanced chemical equation for the complete combustion of methane: CH4(g) + 2O2(g) → CO2(g) + 2H2O(g).
2. Calculate the molar mass of methane (CH4). The atomic masses are approximately: C = 12.01 g/mol and H = 1.01 g/mol. Therefore, the molar mass of CH4 is 12.01 + (4 * 1.01) = 16.05 g/mol.
3. Determine the number of moles of methane in 16 grams by using the formula: moles = mass / molar mass. Substitute the known values: moles of CH4 = 16 g / 16.05 g/mol.
4. Use the stoichiometry of the balanced equation to find the moles of CO2 produced. According to the equation, 1 mole of CH4 produces 1 mole of CO2. Therefore, the moles of CO2 produced are equal to the moles of CH4 combusted.
5. Calculate the mass of CO2 produced using its molar mass. The molar mass of CO2 is approximately: C = 12.01 g/mol and O = 16.00 g/mol, so CO2 = 12.01 + (2 * 16.00) = 44.01 g/mol. Use the formula: mass = moles * molar mass to find the mass of CO2.