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.
An increase in temperature.
A rise in temperature.
altitude
The number and vibration of the molecules that make up the gas cause the pressure.
An increase in temperature of a contained liquid will cause its molecules to move faster and further apart, leading to an expansion in volume. This expansion can potentially increase pressure inside the container if it is sealed, and may also change the physical state of the liquid (e.g. from solid to liquid, or liquid to gas) depending on the specific substance.
The three factors that affect the pressure of a gas in a closed container are the temperature of the gas (higher temperature leads to higher pressure), the volume of the container (smaller volume leads to higher pressure), and the number of gas molecules present (more molecules lead to higher pressure).
A reduction in the temperature of the container.
A restriction will increase pressure and decrease volume
Increasing the number of moles of gas, decreasing the volume of the container, or iIncreasing the temperature could cause a rigid container of gas to explode.
Increase the pressure of the gas inside
The pressure inside a sealed container will not change in a pressurized airplane because the cabin is pressurized to a level that is comfortable for passengers. Therefore, the pressure inside the container will remain constant as long as it is not breached.
the container is made larger
The volume of the container is increased.
When the temperature increases gas and liquid are expending meaning that they are require more volume to occupy. Because containers are usually not expandable the increase of the temperate will cause some damage to the container eventually rising pressure due to the temperature increase will cause explosion which can be really dangerous for everything around.
Lowering the temperature will cause a decrease in gas pressure in a closed container.
Contact between the particles of a gas and walls of the container cause pressure in a closed container of gas.
Pressure based on kinetic theory of gases is given as P = 1/3 * rho * C2 Here rho is the density. Rho = M/V Hence P = 1/3 * M/V * C2 Hence for a given volume, ie V constant as we add more gas ie as M increases then Pressure has to increase. Hence the outcome
The gas molecules gain energy from the heat and so they speed up, causing the pressure to increase.
When a fire is lit in a sealed container it is very likely to cause an explosion because of the build up of internal pressure from smoke.
What causes the pressure exerted by gas molecules on their container? idk