Question 1: Define Le Chatelier's Principle in your own words.

Answer: Le Chatelier's Principle states that if a system at equilibrium is subjected to a change in concentration, temperature, pressure, or volume, the system will adjust to partially counteract the effect of the change and restore a new equilibrium.

Question 2: Explain how increasing the temperature affects the position of equilibrium in an exothermic reaction.

Answer: Increasing temperature shifts the equilibrium position to favor the endothermic reaction, effectively counteracting the increase in heat.

Question 3: Which of the following changes will shift the equilibrium to the right in the reaction: N2 + 3H2 ⇌ 2NH3? (Select one) A) Increasing pressure B) Decreasing temperature C) Removing ammonia D) Adding inert gases

Answer: A) Increasing pressure

Question 4: Fill in the blank: When the concentration of reactants is increased in a system at equilibrium, the system will shift to produce more ________.

Answer: products

Question 5: Describe a practical scenario where Le Chatelier's Principle can be used to optimize a manufacturing process.

Answer: In the Haber process for ammonia production, increasing pressure and adjusting temperature are used to shift the equilibrium toward higher ammonia yield, optimizing production efficiency.

Question 6: In an experiment, adding more reactant to a system at equilibrium results in an increase in product formation. What does this tell you about the reaction's equilibrium state?

Answer: It indicates that the reaction shifts toward the products to re-establish equilibrium when more reactant is added.

Question 7: Calculate the change in pressure (in atm) if the volume of a gas sample at 25°C is decreased from 10 L to 5 L, assuming the amount of gas and temperature remain constant.

Answer: Using Boyle's Law: P1V1 = P2V2. Assuming initial pressure P1 = 1 atm, then P2 = (P1 * V1) / V2 = (1 atm * 10 L) / 5 L = 2 atm.

Question 8: Identify the variable that is changed in the following scenario: 'In a reaction at equilibrium, increasing the temperature.'

Answer: Temperature

Question 9: State one safety precaution to consider when conducting experiments involving gases at high pressure.

Answer: Use pressure-rated equipment and ensure proper safety gear to prevent accidents from gas leaks or explosions.