Mass Relationships in Chemical Reactions
Grade 9 Chemistry worksheet on understanding mass relationships, balancing equations, and the law of conservation of mass.
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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 your work for calculations.
1. Which law states that matter cannot be created or destroyed in a chemical reaction?
Law of Definite Proportions
Law of Multiple Proportions
Law of Conservation of Mass
Law of Conservation of Energy
2. In the reaction 2H₂ + O₂ → 2H₂O, if you start with 4 grams of hydrogen and 32 grams of oxygen, what is the mass of water produced?
18 g
36 g
20 g
40 g
3. The coefficients in a balanced chemical equation represent the ratios of reactants and products.
4. The sum of the atomic masses of all atoms in a molecule is called the mass.
5. Explain what a balanced chemical equation represents in terms of mass relationships.
6. The mass of reactants consumed in a chemical reaction is always less than the mass of products formed.
True
False
7. Consider the reaction: N₂ + 3H₂ → 2NH₃. If you have 28 grams of nitrogen (N₂) and 6 grams of hydrogen (H₂), calculate the theoretical yield of ammonia (NH₃). (Atomic masses: N=14, H=1).
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