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Limiting reactant and percent yield

This educational material helps 12th-grade students practice identifying limiting and excess reactants, calculating theoretical and percent yields through varied question types, and understanding key concepts in reaction stoichiometry and yield calculations. The lessons include problem-solving exercises, multiple-choice questions, and step-arrangement tasks.

By Edform · Chemistry · Grade 12 · Published Oct 15, 2026 · New

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Questions

  1. In a reaction where 4.0 g of hydrogen reacts with 32.0 g of oxygen to form water, which is the limiting reactant?
  2. Which of the following statements about limiting reactants and excess reactants are correct?
  3. If 5.0 g of Na reacts with 10.0 g of Cl₂ to produce NaCl, what is the theoretical yield of NaCl in grams? (Na: 23 g/mol, Cl₂: 71 g/mol, NaCl: 58.5 g/mol)
  4. Arrange the steps for calculating percent yield in the correct order.
  5. Fill in the blanks: In a chemical reaction, the _ reactant is the one that is completely _ up, while the ___ reactant is left over.
  6. Choose the correct word for each blank: The _ yield is the amount of product predicted by stoichiometry, while the _ yield is the amount actually obtained in the lab.
  7. Match each term to its correct definition.
  8. Sort the following items into 'Limiting Reactant' or 'Excess Reactant' based on the scenario: 10 g H₂ and 80 g O₂ react to form water. (Molar masses: H₂ = 2 g/mol, O₂ = 32 g/mol)
  9. Indicate whether each statement about percent yield is true or false.
  10. What is the formula for calculating percent yield? (Give the formula in words or symbols.)

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