Final answer:
The mass of carbon dioxide produced from the complete combustion of 8.40×10⁻³ g of methane is approximately 2.30×10⁻³ g, based on the stoichiometry of the balanced chemical equation and molar masses involved.
Step-by-step explanation:
The question pertains to the mass of carbon dioxide produced from the complete combustion of methane (CH₄). To determine the mass of CO₂ produced, we need to use stoichiometry based on the balanced chemical equation for the combustion of methane:
CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(l)
From the equation, we can see that one mole of methane produces one mole of carbon dioxide. Knowing the molar mass of methane (16.04 g/mol) and carbon dioxide (44.01 g/mol), we can calculate the mass of CO₂ produced from 8.40×10⁻³ g of methane:
The number of moles of methane combusted is 8.40×10⁻³ g divided by 16.04 g/mol, which equals approximately 5.24×10⁻⁴ moles. Since the mole ratio of CH₄ to CO₂ is 1:1, the same number of moles of CO₂ will be produced. Hence, the mass of CO₂ produced is 5.24×10⁻⁴ moles multiplied by 44.01 g/mol, giving approximately 2.30×10⁻³ g of CO₂.