This lab worksheet guides students through observing chemical reactions and calculating mass to prove the Law of Conservation of Matter.

It looks like you've uploaded a worksheet titled "Law of Conservation of Matter Lab" that involves balancing chemical equations and applying the Law of Conservation of Mass, which states that matter cannot be created or destroyed in a chemical reaction. The goal is to balance chemical equations so that the number of atoms of each element is the same on both sides of the equation.

Since I can't view images directly, I'll help you solve this based on the text you provided. Let's go through each section step by step and fill in the blanks accordingly.

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🔬 Part 1: Type Description

This part asks you to identify the type of reaction (e.g., synthesis, decomposition, single replacement, etc.) for each chemical reaction. But since no specific reactions are listed here, we’ll skip ahead to the actual problems.

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🧪 Section #1: Sodium + Chlorine → Sodium Chloride

Unbalanced Equation:
Na + Cl₂ → NaCl

Step 1: Count atoms on each side
- Left: 1 Na, 2 Cl
- Right: 1 Na, 1 Cl

We need to balance chlorine. Since Cl₂ has two atoms, we need 2 NaCl on the right.

Balanced Equation:
2Na + Cl₂ → 2NaCl

✔ Now:
- Left: 2 Na, 2 Cl
- Right: 2 Na, 2 Cl

Answer Key:
- Actual reactants: 2Na + Cl₂ → 2NaCl
- Mass of 2 Na atoms: 2 × 23 = 46 g
- Mass of 1 Cl₂ molecule: 2 × 35.5 = 71 g
- Total mass of reactants: 46 + 71 = 117 g
- Mass of 2 NaCl molecules: 2 × (23 + 35.5) = 2 × 58.5 = 117 g
- Mass of products: 117 g

➡️ Conclusion: Mass is conserved. ✔

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🧪 Section #2: Hydrogen + Oxygen → Water

Unbalanced Equation:
H₂ + O₂ → H₂O

Step 1: Balance oxygen
- O₂ has 2 oxygen atoms; H₂O has 1 → need 2 H₂O
- So: H₂ + O₂ → 2H₂O
- Now hydrogen: 2 H on left, 4 H on right → need 2 H₂

Balanced Equation:
2H₂ + O₂ → 2H₂O

✔ Check:
- Left: 4 H, 2 O
- Right: 4 H, 2 O

Answer Key:
- Actual reactants: 2H₂ + O₂ → 2H₂O
- Mass of 2 H₂ molecules: 2 × (2 × 1) = 4 g
- Mass of 1 O₂ molecule: 2 × 16 = 32 g
- Total mass of reactants: 4 + 32 = 36 g
- Mass of 2 H₂O molecules: 2 × (2×1 + 16) = 2 × 18 = 36 g
- Mass of products: 36 g

➡️ Conclusion: Mass is conserved. ✔

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🧪 Section #3: Calcium + Oxygen → Calcium Oxide

Unbalanced Equation:
Ca + O₂ → CaO

Balance oxygen: O₂ has 2 O atoms; CaO has 1 → need 2 CaO
Then need 2 Ca on left

Balanced Equation:
2Ca + O₂ → 2CaO

✔ Check:
- Left: 2 Ca, 2 O
- Right: 2 Ca, 2 O

Answer Key:
- Actual reactants: 2Ca + O₂ → 2CaO
- Mass of 2 Ca atoms: 2 × 40 = 80 g
- Mass of 1 O₂ molecule: 2 × 16 = 32 g
- Total mass of reactants: 80 + 32 = 112 g
- Mass of 2 CaO molecules: 2 × (40 + 16) = 2 × 56 = 112 g
- Mass of products: 112 g

➡️ Conclusion: Mass is conserved. ✔

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🧪 Section #4: Magnesium + Oxygen → Magnesium Oxide

Unbalanced Equation:
Mg + O₂ → MgO

Balance: O₂ → need 2 MgO → need 2 Mg

Balanced Equation:
2Mg + O₂ → 2MgO

✔ Check:
- Left: 2 Mg, 2 O
- Right: 2 Mg, 2 O

Answer Key:
- Actual reactants: 2Mg + O₂ → 2MgO
- Mass of 2 Mg atoms: 2 × 24 = 48 g
- Mass of 1 O₂ molecule: 32 g
- Total mass of reactants: 48 + 32 = 80 g
- Mass of 2 MgO molecules: 2 × (24 + 16) = 2 × 40 = 80 g
- Mass of products: 80 g

➡️ Conclusion: Mass is conserved. ✔

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✔ Summary Table (Final Answers)

| Section | Balanced Equation | Mass Reactants | Mass Products |
|--------|---------------------------|----------------|---------------|
| #1 | 2Na + Cl₂ → 2NaCl | 117 g | 117 g |
| #2 | 2H₂ + O₂ → 2H₂O | 36 g | 36 g |
| #3 | 2Ca + O₂ → 2CaO | 112 g | 112 g |
| #4 | 2Mg + O₂ → 2MgO | 80 g | 80 g |

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📌 Conclusion:

In all cases, the total mass of reactants equals the total mass of products, demonstrating the Law of Conservation of Matter.

> 💡 Key Concept: Atoms are rearranged in chemical reactions, but not created or destroyed. Therefore, mass is conserved.

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If your worksheet includes any other sections (like decomposition or more complex reactions), feel free to describe them and I’ll help you balance those too!