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Balancing Chemical Equations
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Balancing Chemical Equations
⚖️ Part 1: Understanding Conservation of Mass
1. What does the Law of Conservation of Mass state about chemical reactions?
Atoms can be created during reactions
Matter is neither created nor destroyed in reactions
Mass always increases in reactions
Only energy is conserved in reactions
2. When balancing chemical equations, which part can you change?
The subscripts in chemical formulas
The coefficients in front of formulas
The chemical symbols of elements
The arrow direction
3. In the equation H₂ + O₂ → H₂O, how many hydrogen atoms are on the reactant side?
1
2
3
4
🧮 Part 2: Balancing Practice
4. Balance the following synthesis reaction by writing the correct coefficients:
____ H₂ + ____ O₂ → ____ H₂O
5. Balance this decomposition reaction:
____ H₂O₂ → ____ H₂O + ____ O₂
6. Balance this single-replacement reaction:
____ Zn + ____ HCl → ____ ZnCl₂ + ____ H₂
7. Balance this double-replacement reaction:
____ AgNO₃ + ____ NaCl → ____ AgCl + ____ NaNO₃
8. For the balanced equation 2H₂ + O₂ → 2H₂O, count the atoms on each side:
Reactants: H atoms = _____, O atoms = _____
Products: H atoms = _____, O atoms = _____
✍️ Part 3: Explaining Your Reasoning
9. Choose one equation from Part 2 and explain in 2-3 sentences how you ensured atoms were conserved when balancing it.
10. Why is it important that chemical equations are balanced? Connect your answer to the Law of Conservation of Mass.
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