Mass Relationships in Chemical Reactions
A Grade 10 science worksheet focusing on stoichiometry, limiting reactants, and percentage yield 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. What does stoichiometry primarily deal with in chemical reactions?
The speed of the reaction
The energy changes during a reaction
The quantitative relationships between reactants and products
The types of bonds formed in a reaction
2. In the balanced chemical equation 2H₂ + O₂ → 2H₂O, what is the mole ratio of hydrogen to water?
1:1
2:1
1:2
2:2
3. The reactant that is completely consumed in a chemical reaction and limits the amount of product formed is called the reactant.
4. The actual yield of a product is usually than the theoretical yield due to various factors like incomplete reactions or loss during purification.
5. Calculate the molar mass of Calcium Carbonate (CaCO₃). (Atomic masses: Ca = 40.08 g/mol, C = 12.01 g/mol, O = 16.00 g/mol)
6. If 10.0 grams of hydrogen (H₂) reacts with excess oxygen (O₂) to produce water (H₂O), how many grams of water will be formed? (Balanced equation: 2H₂ + O₂ → 2H₂O)
7. The law of conservation of mass states that mass cannot be created or destroyed in a chemical reaction.
True
False
8. A percentage yield of 100% is commonly achieved in most laboratory chemical reactions.
True
False
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