Use the kinetic molecular theory of gases to explain each of the following:
a. a container of nonstick cooking spray explodes when thrown into a fire.
b. the air in a hot-air balloon is heated to make the balloon rise.
I will be happy to critique your thinking. Post it.
a. The container of nonstick cooking spray explodes when thrown into a fire due to the kinetic molecular theory of gases. According to this theory, gases consist of particles, such as molecules or atoms, that are in constant motion and possess kinetic energy. When the cooking spray can is thrown into the fire, the heat from the fire causes the molecules in the can to gain thermal energy.
As the thermal energy increases, the molecules start to move faster and collide with each other more frequently. Additionally, the increased temperature causes the pressure inside the can to rise rapidly. This pressure buildup is a result of the increased speed and frequency of molecular collisions inside the container.
When the pressure inside the can exceeds the strength of the container, it can no longer contain the increased gas pressure. As a result, the container of nonstick cooking spray explodes, releasing the high-pressure gas and causing the loud noise and sudden expansion of gases.
b. In a hot-air balloon, the air inside is heated to make the balloon rise in accordance with the kinetic molecular theory of gases. The theory states that when you increase the temperature of a gas, the average kinetic energy of its particles also increases.
In a hot-air balloon, a burner is used to heat the air inside the balloon. The heat energy from the burner is transferred to the air molecules inside the balloon, causing them to gain kinetic energy and move faster. The increase in kinetic energy leads to an increase in molecular collisions and the overall pressure inside the balloon.
Since the balloon is sealed, the increased pressure causes the balloon to expand and become less dense compared to the surrounding air. As a result, the buoyant force acting on the balloon becomes greater than the downward force of gravity, enabling the balloon to rise upwards.
By continuously heating the air inside the balloon, the hot air remains less dense than the colder air outside, allowing the balloon to continue rising and maintaining its altitude. The concept behind the hot-air balloon's movement is based on the kinetic molecular theory of gases, which explains how heating air increases its kinetic energy, resulting in the balloon's ascent.
a. According to the kinetic molecular theory of gases, gas particles are in constant random motion and have negligible volume compared to the container they occupy. They also exert pressure when they collide with the container walls.
In the case of a container of nonstick cooking spray exploding when thrown into a fire, it can be explained as follows: Nonstick cooking sprays typically contain ingredients such as vegetable oil, propellant gases (such as propane or butane), and a propellant agent like nitrous oxide. When the container is thrown into a fire, the heat from the fire causes the propellant gases to rapidly increase in temperature.
According to Charles's Law, as the temperature of a gas increases, its volume also increases, assuming the pressure remains constant. In this case, the increase in temperature leads to a substantial increase in the volume of the propellant gases inside the container.
However, the container is not designed to withstand high internal pressures, and the sudden increase in volume creates a significant increase in pressure. This increased pressure exceeds the container's ability to contain it, thus resulting in an explosion.
b. The air in a hot-air balloon is heated to make the balloon rise. According to the kinetic molecular theory of gases, heating a gas increases the average kinetic energy of its particles. This increase in kinetic energy causes the gas particles to move faster and collide more frequently with each other and the walls of the container.
In the case of a hot-air balloon, a burner is used to heat the air inside the balloon envelope. As the air inside the balloon is heated, the gas particles gain kinetic energy and their average speed increases. These fast-moving air particles collide with the surrounding particles, including the heavier cool air outside the envelope.
The collision between the hot air inside the balloon and the colder air outside leads to an increase in the pressure inside the balloon. Boyle's Law states that, at constant temperature, the pressure of a gas is inversely proportional to its volume. Hence, as the pressure increases, the volume of the hot air inside the balloon also expands.
Since the hot air is now less dense than the cooler air outside, it creates a buoyant force greater than the force of gravity, causing the balloon to rise. Heating the air inside the balloon creates the necessary temperature and pressure difference to generate the lift required for the balloon to ascend.