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Which is the limiting reactant when 5.00 g of H_{2} and 10.0 g of O_{2} react and form water?
Accepted Answer
To determine the limiting reactant, we need to convert the masses of H₂ and O₂ to moles and compare their mole ratios to the balanced chemical equation for the reaction:
2H₂ + O₂ → 2H₂O
Moles of H₂: (5.00 g H₂) / (2.016 g/mol H₂) = 2.48 mol H₂
Moles of O₂: (10.0 g O₂) / (32.00 g/mol O₂) = 0.313 mol O₂
According to the balanced equation, 2 moles of H₂ react with 1 mole of O₂. To completely react with the 0.313 mol O₂, we would need 0.626 mol H₂. Since we have more H₂ (2.48 mol) than needed, O₂ is the limiting reactant.
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