Mass Relationships in Chemical Reactions
Explore 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 answer to the best of your ability. Show all work for calculations.
1. Which law states that matter cannot be created or destroyed in a chemical reaction?
Law of Definite Proportions
Law of Conservation of Mass
Law of Multiple Proportions
Avogadro's Law
2. What is the molar mass of H₂O? (Atomic masses: H=1.01 g/mol, O=16.00 g/mol)
17.01 g/mol
18.02 g/mol
19.01 g/mol
34.02 g/mol
1. The coefficients in a balanced chemical equation represent the ratio of reactants and products.
2. A reactant is completely consumed in a chemical reaction and limits the amount of product formed.
3. The theoretical yield is the maximum amount of product that can be formed from a given amount of .
1. Balance the following chemical equation: N₂ + H₂ → NH₃
2. Explain the difference between actual yield and theoretical yield.
1. In a chemical reaction, the total mass of the reactants is always equal to the total mass of the products.
True
False
2. A percent yield greater than 100% is possible in a carefully conducted experiment.
True
False
Consider the reaction: 2Al(s) + 3Cl₂(g) → 2AlCl₃(s)
If 54.0 g of aluminum reacts with 71.0 g of chlorine gas, what is the limiting reactant?
What is the theoretical yield of aluminum chloride (AlCl₃) in grams?