Physics Check By Mr. Garry

The value -273 degrees Celsius is also known as absolute zero. Absolute zero is the lowest possible temperature, where all molecular motion ceases. It is the point at which all substances have their minimum possible energy.

The Kelvin scale starts at absolute zero, which is -273.15 degrees Celsius. To convert Celsius to Kelvin, you simply add 273. Therefore, 25 degrees Celsius is closest to 298 Kelvin.

Boyle's Law describes the relationship between the pressure and volume of a gas at a constant temperature. According to the law, as the volume of a gas decreases, the pressure increases, and vice versa. This means that the pressure and volume are inversely proportional to each other. Therefore, the correct answer is true.

The correct answer is option 4. This graph shows an inverse relationship between volume and pressure of gas at constant temperature. As the volume decreases, the pressure increases and vice versa. This is known as Boyle's Law, which states that the pressure of a gas is inversely proportional to its volume when the temperature is held constant.

The ideal gas law relates the pressure (P), volume (V), number of moles (N), and temperature (T) of a gas. The equation PV = NRT is derived from the ideal gas law, where P represents pressure, V represents volume, N represents the number of moles, R represents the gas constant, and T represents temperature. This equation states that the product of the pressure and volume of a gas is directly proportional to the number of moles, the gas constant, and the temperature.

When the temperature of an ideal gas is increased at constant pressure, the volume of the gas also increases. This relationship is described by Charles's Law, which states that the volume of an ideal gas is directly proportional to its temperature, assuming constant pressure. Therefore, if the initial volume of the gas is 30 Liters at 500 Kelvin, and the temperature is raised to 1500 Kelvin, the new volume of the gas would be 90 Liters.

The pressure of a gas is related to the collision of molecules with the container. When gas molecules collide with the walls of the container, they exert a force which creates pressure. The more frequent and intense the collisions, the higher the pressure. Therefore, the collision of molecules with the container is directly related to the pressure of the gas.

When the pressure of a gas decreases, its volume increases, according to Boyle's Law. Boyle's Law states that at constant temperature, the pressure and volume of a gas are inversely proportional. In this case, the pressure decreases by half from 200,000 Pa to 100,000 Pa. Therefore, the volume of the gas will double from 1 Liter to 2 Liters.

The correct answer is "Volume is directly proportional to Temperature." According to Charles's Law, the volume of a gas is directly proportional to its temperature, assuming constant pressure. This means that as the temperature increases, the volume of the gas expands, and as the temperature decreases, the volume of the gas shrinks. This is consistent with the behavior of the balloon in the diagram, as it expands when heated and shrinks when cooled.

This experiment tells us that when the volume is kept constant, the pressure of a gas increases as the temperature increases. This is because as the temperature rises, the gas molecules gain more kinetic energy and move faster, colliding with the walls of the container more frequently and with greater force. This increase in collisions leads to an increase in pressure.

An ideal gas is characterized by its molecules being spherical and very small, which means they occupy negligible space compared to the volume of the gas. Additionally, the molecules of an ideal gas are in rapid random motion, meaning they move in all directions with high speed and collide with each other and the walls of the container. These two descriptions are consistent with the behavior of an ideal gas and distinguish it from other types of gases. The other descriptions, such as molecules having attractive forces or sticking together when they collide, are not applicable to an ideal gas.