Final answer:
To calculate the mass of carbon dioxide needed when using 6.0 × 104 g of methanol, we need to use the stoichiometry of the balanced chemical equation. The mass of carbon dioxide is 8.24 × 104 g.
Step-by-step explanation:
To calculate the mass of carbon dioxide needed, we need to use the stoichiometry of the balanced chemical equation. The balanced equation is:
CH3OH + CO -> CH3COOH
The molar mass of CH3OH is 32.04 g/mol, and the molar mass of CH3COOH is 60.05 g/mol. First, we need to convert the mass of methanol (6.0 × 104 g) to moles:
moles of CH3OH = mass of CH3OH / molar mass of CH3OH
= 6.0 × 104 g / 32.04 g/mol
= 1873.8 mol
According to the balanced equation, the mole ratio between CH3COOH and CO is 1:1. Therefore, the number of moles of CO needed is also 1873.8 mol. Finally, we can calculate the mass of carbon dioxide:
mass of CO2 = moles of CO2 x molar mass of CO2
= 1873.8 mol x 44.01 g/mol
= 8.24 × 104 g