Properties Of Gases

As we add heat to a gas, the temperature increases, therefore increasing kinetic energy. As kinetic energy increases, this means the particles of the gases move faster, hitting the container wall more often (creating more pressure) and in turn expanding/increasing the volume.

When the pressure on a gas doubles, according to Boyle's Law, the volume of the gas will decrease by half. This is because as the pressure increases, the gas molecules are compressed closer together, resulting in a decrease in volume.

When the temperature of a gas is doubled, according to Charles's Law, the volume of the gas will also double. This is because as the gas molecules gain more energy from the increase in temperature, they move faster and collide with the container walls more frequently, causing the volume to increase. Therefore, the correct answer is that the volume of the gas will increase by a factor of 2.

Pressure is defined as the force per unit area. It is a measure of the amount of force applied to a given area. When a force is applied to a surface, the pressure is the force distributed over that surface. It is calculated by dividing the force applied by the area over which it is applied. Therefore, pressure is the correct answer to the given question.

When the pressure on a gas increases, the gas molecules are forced closer together. This reduces the space between the molecules, resulting in a decrease in volume. Therefore, as the pressure increases, the volume of the gas decreases.

Absolute zero, or 0 K, means there is no kinetic energy, or movement of molecules.

STP is a standardized set of conditions for measuring and comparing the properties of gases. The temperature at STP is defined as 0 degrees Celsius (273.15 Kelvin), and the pressure is set at 1 atmosphere (101.325 kPa). These conditions allow for consistent data comparison and reproducibility in scientific experiments.

According to the kinetic molecular theory:

All molecules of a substance stay in constant motion: This theory posits that gas molecules are always moving.

All atoms or molecules of a gas have no intermolecular attractions: Gas particles are assumed to move independently without attractive forces between them.

Collisions between molecules are completely elastic (no energy is lost): When gas molecules collide, they do so without losing energy, meaning the total kinetic energy remains constant.

Gases have no set volume: Gases expand to fill the volume of their container, meaning they do not have a fixed volume.

At Standard Temperature and Pressure (STP), the temperature is defined as 0 degrees Celsius (273.15 Kelvin) and the pressure is 1 atmosphere (101.325 kPa). STP is a reference point used in various scientific contexts, particularly in chemistry and physics, to allow for consistent conditions when comparing different sets of data or conducting experiments.