Oxygen is the limiting reagent, phosphorus is in excess, and the theoretical yield is determined by the complete reaction of 5 moles of oxygen with 3 moles of phosphorus to produce P4O10.
To determine the limiting reagent, excess reagent, and theoretical yield, we need to compare the stoichiometric coefficients of the balanced chemical equation for the reaction between oxygen gas (O2) and solid phosphorus (P4). Assuming the balanced equation is P4(s) + 5O2(g) → P4O10(s), we can analyze the given moles of reactants.
Given:
Moles of oxygen gas (O2) = 5 moles
Moles of solid phosphorus (P4) = 3 moles
According to the balanced equation, one mole of solid phosphorus reacts with five moles of oxygen gas. Therefore, the molar ratio is 1:5.
Limiting Reagent:
Calculate the moles of oxygen needed for complete reaction with 3 moles of solid phosphorus using the molar ratio:
3 moles × (5/1) = 15 moles
Since only 5 moles of oxygen are available, oxygen is the limiting reagent.
Excess Reagent:
Phosphorus is the excess reagent because not all of it will react due to the limited availability of oxygen.
Theoretical Yield:
The theoretical yield is the amount of product formed when the limiting reagent is completely consumed. In this case, the theoretical yield of P4O10 is determined by the moles of limiting reagent (oxygen).