Final answer:
The mass of carbon dioxide produced when 10.1 g of methane reacts with 38.0 g of oxygen is 27.77 g.
Step-by-step explanation:
To determine the mass of carbon dioxide produced when methane reacts with oxygen, we need to balance the chemical equation and calculate the molar masses. The balanced equation for the reaction is:
CH4 + 2O2 → CO2 + 2H2O
1 mole of methane reacts with 2 moles of oxygen to produce 1 mole of carbon dioxide. The molar mass of CH4 is 16.04 g/mol, and the molar mass of CO2 is 44.01 g/mol.
Using the given masses of methane and oxygen, we can calculate the moles of each substance:
Moles of CH4: 10.1 g / 16.04 g/mol = 0.6308 mol
Moles of O2: 38.0 g / 32.00 g/mol = 1.1875 mol
Since the stoichiometry of the reaction is 1:1 for CH4 and CO2, the number of moles of CO2 produced is also 0.6308 mol.
To calculate the mass of CO2 produced, we can use the molar mass:
Mass of CO2 = Moles of CO2 × Molar mass of CO2
Mass of CO2 = 0.6308 mol × 44.01 g/mol = 27.77 g