Given the equation 2CO + O₂ → 2CO₂, how many grams of CO₂ form if 34.0 grams of CO are combined with excess oxygen?

Question

Quizplus · Accepted Answer

The equation shows that 2 moles of CO react to form 2 moles of COS. The molar mass of CO is 28.01 g/mol, so 34.0 g of CO is 34.0 g / 28.01 g/mol = 1.214 moles of CO. Since the reaction produces COS in a 1:1 mole ratio with CO, 1.214 moles of COS are produced. The molar mass of COS is approximately 60.07 g/mol (12.01 for C, 16.00 for O, and 32.06 for S), so the mass of COS produced is 1.214 moles * 60.07 g/mol = 72.9 g. However, given the options and the apparent typo in the chemical formula (assuming COS is intended), none of the numerical values directly match this calculation. Given the choices, the closest or most reasonable extrapolation based on typical question formats and potential typographical errors in the question would be to assume a calculation mistake or misunderstanding in the chemical formula interpretation. Without clear chemical formulas or correct molar masses based on the provided formulas, the calculation aligns closest with the principle of stoichiometry but doesn't match any provided answer exactly. Therefore, the response is based on an attempt to correct for apparent errors in the question's presentation.

Given the Equation 2CO + O2 → 2CO2, How Many

Given the Equation 2CO + O₂ → 2CO₂, How Many