Test
Stoichiometry practice
Students practise stoichiometry using mole ratios from balanced equations, mass-to-mass conversions, and step-by-step calculations. Guided through short question sets on limiting reagents and excess. Level: 11th grade.
By Edform · Chemistry · Grade 11 · Published Oct 28, 2026 · New
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Questions
- For the balanced equation 2H₂ + O₂ → 2H₂O, what is the mole ratio of H₂ to O₂?
- According to N₂ + 3H₂ → 2NH₃, how many moles of NH₃ can form from 6.0 mol H₂ when N₂ is in excess?
- For 2Mg + O₂ → 2MgO, approximately what mass of MgO forms from 12.0 g Mg when O₂ is in excess? Use molar masses Mg = 24.3 g/mol and MgO = 40.3 g/mol.
- For 2Al + 3Cl₂ → 2AlCl₃, 4.0 mol Al reacts with 3.0 mol Cl₂. How many moles of AlCl₃ can form?
- Put the steps of a mass-to-mass stoichiometry calculation in the correct order.
- Match each balanced equation to the mole ratio named in the right column.
- Complete the stoichiometric relationship using the balanced equation.
- Choose the amount that completes the calculation.
- For each statement about balanced equations and stoichiometry, mark whether it is true or false.
- For CaCO₃ → CaO + CO₂, calculate the mass of CO₂ produced from 25.0 g CaCO₃. Use molar masses CaCO₃ = 100.1 g/mol and CO₂ = 44.01 g/mol. Give your answer in grams.
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