Use Boyle's Law, applicable for ideal gases at constant temperature, to solve this problem: P1*V1 = P2*V2
If the volume of a container of air is reduced by one half the partial pressure of the oxygen with in the container will be doubled. If the volume of a container of gas is reduced, the pressure inside the container will increase.
Increasing the temperature of a gas will increase it's pressure ONLY if the volume is held constant.
At isobaric (pressure) expansion (volume increase) the temperature will increase because V is proportional to T for the same amount of gas (closed container) at constant pressure.
The pressure increases. Hopefully, the container is strong enough to withstand the increased pressure. If there is a weakness in the container, gas will escape as a leak.
Because the pressure increases The real answer is: Charles's Law. He found that if you increase the temperature of a constant pressure the volume increases also.
The pressure will increase. The reason is that the more air particles relative the volume the more of a pressure you are going to have, the same thing is true of temperature changes.
Assuming the volume is kept constant, the pressure will also decrease in this case.
In a container the volume remain constant but the pressure increase.
Assuming the temperature stays constant and there is no leakage of gas, then if the container decreases in size then the pressure will increase.
it decreases.
A loss of gas, or a decrease in temperature.
The constant collision of gas molecules against the inside walls of a container produces pressure which is directly proportional to the number of collisions.