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

Answer: 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.

Question 2: What are the scientific units used to measure pressure and volume of gases?

Answer: Pressure is measured in pascals (Pa), and volume is measured in liters (L) or cubic meters (m³).

Question 3: Explain why increasing the pressure on a gas in a sealed container decreases its volume, assuming temperature remains constant.

Answer: According to Boyle's Law, increasing pressure forces gas particles closer together, reducing the volume they occupy, provided temperature stays the same.

Question 1: A gas sample has a volume of 3.0 liters at a pressure of 100 kPa. What will be its volume when the pressure increases to 150 kPa, assuming temperature remains constant?

Answer: 2.0 liters

Question 2: A sealed container holds 5 liters of gas at a pressure of 80 kPa. If the volume is reduced to 2 liters, what is the new pressure of the gas?

Answer: 200 kPa

Question 1: Describe a simple experiment to demonstrate Boyle's Law using a syringe, a pressure sensor, and a sealed container. Include the variables you would change and measure.

Answer: A student can connect a syringe with a sealed, flexible container to a pressure sensor. By gradually pushing the syringe plunger to decrease the volume inside the container, the pressure reading increases. Variables include the volume of the gas (controlled by the syringe plunger) and the pressure measured by the sensor. The temperature should be kept constant, and safety precautions include ensuring the container is sealed properly to prevent gas leaks.

Question 2: Identify the key variables involved in an experiment testing Boyle's Law and explain their roles.

Answer: The key variables are pressure and volume. Volume is varied by changing the container size or syringe piston position, and pressure is measured to observe the inverse relationship. Temperature must be kept constant to ensure Boyle's Law applies accurately.

Question 1: A sealed container initially has a volume of 4 liters and a pressure of 120 kPa. When the volume is decreased to 2 liters, the pressure increases to 240 kPa. Explain how this data supports Boyle's Law.

Answer: The data shows that when the volume halves (from 4 L to 2 L), the pressure doubles (from 120 kPa to 240 kPa), demonstrating the inverse relationship predicted by Boyle's Law.

Question 1: A cylinder contains 2 liters of gas at a pressure of 100 kPa. If the gas is compressed to 1 liter at the same temperature, what is the new pressure? Show your calculations.

Answer: 200 kPa

Question 2: Discuss the importance of Boyle's Law in industries such as scuba diving or medical equipment. Include real-world applications and safety considerations.

Answer: Boyle's Law is crucial in industries like scuba diving, where divers use compressed air tanks; understanding pressure-volume relationships helps prevent accidents such as tank rupture or decompression sickness. In medical equipment like ventilators, Boyle's Law guides the regulation of air pressure and volume to ensure patient safety. Proper application of Boyle's Law ensures equipment functions efficiently, and safety precautions include regular equipment checks and adherence to safety standards.

Question 1: Explain how Boyle's Law is used in the operation of a syringe or a spray can.

Answer: In a syringe, pulling the plunger increases the volume, which decreases pressure, allowing liquid to be drawn in. When pushing the plunger, volume decreases, pressure increases, forcing the liquid out. Similarly, in spray cans, increasing pressure pushes the contents out as the volume decreases inside the can.

Question 2: Describe a scenario where Boyle's Law could be involved in a safety situation in a high-altitude environment.

Answer: At high altitude, external pressure decreases, causing gases inside sealed containers or lungs to expand. Without proper regulation, this expansion can cause containers to burst or lead to lung injury, highlighting the importance of understanding Boyle's Law for safety.