Formulas and examples for gas law applications in reaction stoichiometry.

📚 Quick Study Guide

🔍 Ideal Gas Law: $PV = nRT$, where P = pressure, V = volume, n = moles, R = ideal gas constant, T = temperature. 🌡️ Standard Temperature and Pressure (STP): 0°C (273.15 K) and 1 atm. 📐 Molar Volume at STP: 22.4 L/mol for an ideal gas. ⚖️ Stoichiometric Coefficients: Ratios from balanced chemical equations used to determine mole relationships. 💡 Combining Gas Laws with Stoichiometry: Use the ideal gas law to find moles (n) and then apply stoichiometric ratios to relate reactants and products.

🧪 Practice Quiz

1. What volume will 2 moles of $H_2$ gas occupy at STP?
   1. 11.2 L
   2. 22.4 L
   3. 33.6 L
   4. 44.8 L
2. In the reaction $N_2(g) + 3H_2(g) \rightarrow 2NH_3(g)$, if you start with 5 L of $N_2$ and excess $H_2$, what volume of $NH_3$ is produced, assuming constant temperature and pressure?
   1. 2.5 L
   2. 5 L
   3. 10 L
   4. 15 L
3. If 4.0 grams of $H_2$ react completely with $O_2$ to form water, how many grams of water ($H_2O$) are produced?
   1. 9.0 g
   2. 18.0 g
   3. 36.0 g
   4. 72.0 g
4. What is the density of $O_2$ gas at STP?
   1. 0.714 g/L
   2. 1.429 g/L
   3. 2.857 g/L
   4. 3.500 g/L
5. In the reaction $2CO(g) + O_2(g) \rightarrow 2CO_2(g)$, if you have 10 L of CO and 8 L of $O_2$ at the same temperature and pressure, what volume of $CO_2$ can be produced?
   1. 8 L
   2. 10 L
   3. 16 L
   4. 20 L
6. How many moles of gas are present in a 10 L container at 27°C and 2 atm pressure? (R = 0.0821 L atm / (mol K))
   1. 0.81 moles
   2. 1.63 moles
   3. 2.45 moles
   4. 3.26 moles
7. What mass of $CO_2$ is produced when 10 liters of $CH_4$ undergo complete combustion at STP according to the equation $CH_4 + 2O_2 \rightarrow CO_2 + 2H_2O$?
   1. 19.6 g
   2. 28.3 g
   3. 11.6 g
   4. 1.96 g