Final answer:
To determine the limiting reactant, calculate the number of moles of each reactant and compare the ratios of the coefficients in the balanced equation. In this case, CS₂ is the limiting reactant and O₂ is in excess.
Step-by-step explanation:
To determine which reactant is limiting, we need to calculate the number of moles of each reactant using their molar masses, then compare the ratios of the coefficients in the balanced equation.
Given:
- Mass of CS₂ = 45.5 g
- Mass of O₂ = 30.3 g
- Molar mass of CS₂ = 76.14 g/mol
- Molar mass of O₂ = 32.00 g/mol
First, calculate the number of moles of each reactant:
- Moles of CS₂ = Mass of CS₂ / Molar mass of CS₂ = 45.5 g / 76.14 g/mol = 0.596 mol
- Moles of O₂ = Mass of O₂ / Molar mass of O₂ = 30.3 g / 32.00 g/mol = 0.946 mol
Next, compare the ratios of the coefficients in the balanced equation:
- Ratio CS₂: O₂ = 1:3
- Ratio O₂: CS₂ = 3:1
We can see that the ratio of moles of O₂ to CS₂ is 1.59, which is greater than the stoichiometric ratio of 3:1. Therefore, O₂ is in excess and CS₂ is the limiting reactant in this reaction.