What will happen to the pressure when the volume is doubled?

If volume increases, then pressure decreases and vice versa, when the temperature is held constant. Therefore, when the volume is halved, the pressure is doubled; and if the volume is doubled, the pressure is halved.

What would happen to the volume if the temperature doubled?

The volume of a sample of gas is dependent upon the Kelvin temperature of the gas. Increasing the Kelvin temperature increases the volume. The two quantities are directly proportional to one another. A doubling of the Kelvin temperature will double the volume of the gas.

What happened to pressure if the volume is reduced to half and the temperature is doubled?

The law itself can be stated as follows: for a fixed amount of an ideal gas kept at a fixed temperature, P (pressure) and V (volume) are inversely proportional—that is, when one doubles, the other is reduced by half. The moving wall converts the effect of molecular collisions into pressure and acts as a pressure gauge.

What happens to pressure when volume and temperature decrease?

The combined gas law states that the pressure of a gas is inversely related to the volume and directly related to the temperature. If temperature is held constant, the equation is reduced to Boyle’s law. Therefore, if you decrease the pressure of a fixed amount of gas, its volume will increase.

What happens to the pressure if the gas temperature is increased while N and V are held constant?

As the temperature increases, the average kinetic energy increases as does the velocity of the gas particles hitting the walls of the container. The force exerted by the particles per unit of area on the container is the pressure, so as the temperature increases the pressure must also increase.

When volume of a system is increased two times and temperature is decreased half of its initial temperature then pressure becomes?

So ans is it becomes 1/4 times.

When temperature increases what happens to pressure?

The temperature of the gas is proportional to the average kinetic energy of the gas molecules. The particles moving faster collide with the container walls frequently with greater force. This causes the force on the walls of the container to increase and so the pressure increases.