Question 1: Boyle's Law states that for a fixed amount of gas at constant temperature, the pressure of the gas is inversely proportional to its volume. Write a brief explanation of why this relationship exists based on the particle model.

Answer: In the particle model, reducing the volume increases the frequency of particle collisions with the container walls, which increases pressure. Conversely, increasing volume decreases collision frequency, lowering pressure, assuming temperature and amount of gas remain constant.

Question 1: Define Boyle's Law in your own words.

Answer: Boyle's Law states that at constant temperature, the pressure of a gas is inversely proportional to its volume.

Question 2: What assumptions are made about gases when applying Boyle's Law?

Answer: The gas is assumed to be ideal, with constant temperature, fixed amount of gas, and no change in the gas's composition.

Question 1: A gas occupies 3.0 liters at a pressure of 1.0 atm. If the pressure is increased to 2.0 atm at constant temperature, what will be the new volume of the gas? (Use Boyle's Law: P₁V₁ = P₂V₂)

Answer: 1.5 liters

Question 2: A sealed container has a volume of 10 liters and a pressure of 0.8 atm. If the volume is reduced to 5 liters at constant temperature, what is the pressure inside the container?

Answer: 1.6 atm

Question 1: Describe a simple experiment to demonstrate Boyle's Law using a syringe and a pressure sensor. What variables would you control, and what safety precautions should be taken?

Answer: Fill a syringe with air and connect it to a pressure sensor. Vary the volume by pushing or pulling the syringe plunger while keeping the temperature constant. Record the pressure readings at different volumes. Control variables include temperature and amount of gas. Safety precautions include ensuring no sharp objects are present and handling the syringe carefully to avoid injury.

Question 1: A scuba diver compresses a gas-filled container at depth, increasing pressure from 1 atm to 4 atm, while the temperature remains constant. The initial volume of the gas was 5 liters. What is the new volume of the gas after compression?

Answer: 1.25 liters

Question 1: Explain how Boyle's Law is used in the operation of a syringe or in a car's internal combustion engine.

Answer: In a syringe, pulling the plunger increases volume and decreases pressure, drawing in air or fluid. Pushing the plunger decreases volume and increases pressure, forcing out the contents. In a car engine, compression of gases in the cylinder follows Boyle's Law, increasing pressure and temperature to facilitate combustion.

Question 1: A sealed container initially has a volume of 8 liters and a pressure of 1 atm at room temperature. The container is compressed to half its original volume. Calculate the new pressure inside the container. Explain the steps in your calculation and the scientific principle involved.

Answer: Using Boyle's Law: P1V1 = P2V2. Initial pressure P1 = 1 atm, initial volume V1 = 8 L, final volume V2 = 4 L. Therefore, P2 = (P1 * V1) / V2 = (1 atm * 8 L) / 4 L = 2 atm. This demonstrates that decreasing volume increases pressure proportionally, assuming constant temperature and amount of gas.