The answer to this question lies in the ideal gas law: PV=nrT
in which:
P = presssure
V = Volume
n = number of moles
r = ideal gas constant
T = temperature
because we want P to increase, we can achieve that in a couple of ways:
1. decrease the volume
2. increase the number of moles
3. increase the temperature.
Value of r cannot change; it is a constant.
Both compressing and heating a gas will increase its pressure.
Increase the pressure of the gas inside
The volume decrease only when the external pressure increase.
If the pressure of the gas increase, the solubility in a liquid increase.
The pressure increase.
An increase in temperature or a decrease in volume would call the pressure to increase. Apex- increasing the number of gas particles
The volume of the container is increased.
temperature increase The pressure of a contained sample of gas can be increased by increasing its temperature, or by decreasing its volume, or by injecting additional mass into it.
It would increase.
it would change the pressure exerted by the gas in the container.
Increase the pressure of the gas inside
The temperature
The pressure would increase.
Both compressing and heating a gas will increase its pressure.
If you increase the volume of the container, and not the gas itself, then the pressure decreases. If you increase the volume of the gas, and not the container, then the pressure increases.
According to the combined gas law, volume and pressure are indirectly related. Therefore, if the pressure of a gas increases, the volume will decrease.
As indicated by the Ideal Gas Laws, increasing temperature will tend to increase both volume and pressure. Of course, volume can't always increase, that depends upon the flexibility or inflexibility of the container that the gas is in, and if the volume does increase that will counteract the increase in pressure that would otherwise have happened. Temperature, pressure, and volume are all interconnected in a gas.