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Avogadro's Law Calculations
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Avogadro's Law Calculations
📚 Part 1: Understanding Avogadro's Law
1. State Avogadro's Law in your own words:
2. What conditions must remain constant for Avogadro's Law to apply? (Check all that apply)
Temperature
Pressure
Volume
Number of moles
3. At STP (Standard Temperature and Pressure), what volume does 1 mole of any gas occupy?
11.2 dm³
22.4 dm³
44.8 dm³
67.2 dm³
🧮 Part 2: Basic Calculations
4. Calculate the volume of 3.5 moles of hydrogen gas at STP.
5. How many moles of oxygen gas are present in 89.6 dm³ at STP?
6. If 2.8 dm³ of nitrogen gas contains 0.125 moles at STP, what volume would 0.5 moles occupy under the same conditions?
⚗️ Part 3: Chemical Reaction Applications
7. In the reaction: 2H₂ + O₂ → 2H₂O, if 44.8 dm³ of hydrogen gas reacts at STP, what volume of oxygen gas is required?
8. For the decomposition reaction: 2KClO₃ → 2KCl + 3O₂, calculate the volume of oxygen gas produced when 1.5 moles of KClO₃ decompose at STP.
9. Complete the following statement about Avogadro's Law:
If the temperature and pressure remain __________, then the volume of a gas is __________ proportional to the number of __________ present. This relationship can be expressed mathematically as V₁/n₁ = __________.
🎨 Part 4: Visual Understanding
10. Draw two gas containers showing Avogadro's Law. Label one container with 1 mole of gas and 22.4 dm³, and the other with 2 moles of gas and the corresponding volume at STP.
11. Match the gas quantities with their corresponding volumes at STP:
1. 0.5 moles
2. 2.0 moles
3. 4.5 moles
4. 0.25 moles
A. 100.8 dm³
B. 44.8 dm³
C. 11.2 dm³
D. 5.6 dm³
🔬 Part 5: Problem Solving Challenge
12. A student collects hydrogen gas by the displacement of water. If 3.36 dm³ of hydrogen gas is collected at STP, how many moles of hydrogen were produced?
13. Explain why Avogadro's Law is important in stoichiometric calculations involving gases:
14. True or False: According to Avogadro's Law, different gases at the same temperature and pressure will have the same density.
True
False
Explain your answer:
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