The following reaction was studied: 2Fe(s) + 3Cl₂(g) → 2FeCl₃(s). A scientist mixed 100 g of Fe(s) with 200 g of Cl₂(g). What is the limiting reagent? What mass of FeCl₃(s) forms? Note the following molar masses:
Fe = 55.85 g/mol
Cl = 35.45 g/mol

Fe is limiting, and 290 g of FeCl₃ forms.
Cl₂ is limiting, and 305 g of FeCl₃ forms.
Fe is limiting, and 269 g of FeCl₃ forms.
Cl₂ is limiting, and 300 g of FeCl₃ forms.

CO(g) and O₂(g) are reacted via this equation: 2CO(g) + O₂(g) → 2CO₂(g).
5.0 mol of O₂(g) is reacted with excess CO(g), and 4.7 mol of CO₂(g) is produced. What is the percent yield? (Hint: a conversion will need to be performed to calculate the theoretical yield of CO₂(g), and then this is used in the % yield calculation; at no time is it necessary to convert moles to grams)

Options:
- 47%
- 94%
- 24%
- 12%