Mass Relationships in Chemical Reactions
A Grade 12 Chemistry worksheet exploring stoichiometry, limiting reactants, percent yield, and mass conservation in chemical reactions.
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Mass Relationships in Chemical Reactions
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Read each question carefully and provide your answers in the space provided. Show all your work for calculations.
1. Balance the following chemical equation and then answer the questions below: Fe(s) + O₂(g) → Fe₂O₃(s)
a) What type of reaction is this?
b) If 10.0 moles of Fe react completely, how many moles of Fe₂O₃ will be produced?
2. In a chemical reaction, the is the reactant that is completely consumed and limits the amount of product formed. The reactant that is left over is called the reactant.
3. Consider the reaction: 2Al(s) + 3Cl₂(g) → 2AlCl₃(s). If 50.0 g of Al reacts with excess Cl₂ to produce 150.0 g of AlCl₃, what is the percent yield of the reaction? (Molar mass of Al = 26.98 g/mol, AlCl₃ = 133.34 g/mol)
4. The law of conservation of mass states that matter cannot be created or destroyed in a chemical reaction.
True
False
Match each term on the left with its definition on the right.
a. Stoichiometry
i. The maximum amount of product that can be formed from given amounts of reactants.
b. Theoretical Yield
ii. The study of the quantitative relationships between reactants and products in chemical reactions.
c. Actual Yield
iii. The amount of product actually obtained from a chemical reaction.
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