The temp will increase.
A decrease in temperature or a decrease in the number of gas particles in the container will cause a decrease in gas pressure. Additionally, if some of the gas particles escape from the container, it will also lead to a decrease in pressure.
A decrease in temperature will cause a decrease in gas pressure in a closed container as the gas molecules will have less kinetic energy, resulting in less frequent collisions with the container walls. Alternatively, removing some of the gas from the container will also lower the gas pressure as there are fewer gas molecules present to exert pressure on the walls.
Pressure affects the behavior of gases in a closed container by influencing their volume, temperature, and density. As pressure increases, the gas molecules are forced closer together, leading to a decrease in volume. This can also cause an increase in temperature due to the molecules colliding more frequently. Additionally, higher pressure can result in an increase in gas density within the container.
False. As heat is applied to a closed container containing a gas, the temperature will increase, causing the gas molecules to move faster and collide more frequently with the container walls, resulting in an increase in pressure, not a decrease.
A decrease in temperature or a decrease in the number of gas molecules in the container will cause a decrease in gas pressure. Alternatively, if some of the gas molecules escape from the container, the pressure will also decrease.
When a gas is compressed in a closed container, the pressure of the gas increases because the volume it occupies decreases. This increase in pressure can lead to the gas molecules being closer together, resulting in an increase in temperature.
Lowering the temperature will cause a decrease in gas pressure in a closed container.
A decrease in gas pressure in a closed container could be caused by a decrease in temperature, which reduces the average kinetic energy of the gas molecules, leading to fewer collisions with the container walls. It could also be caused by a leak in the container allowing gas to escape, or by a chemical reaction that consumes gas molecules.
In a closed system the pressure is directly proportional to the temperature (Gay-Lussac law).At higher temperature the volume tend to increase but in a container the volume is limited.
yes because it directly proportional with it
No, in a closed container, increasing the temperature of a gas will actually increase the force with which particles hit the walls of the container. This is because higher temperature leads to higher kinetic energy of the gas particles, causing them to move faster and collide with the walls with greater force.
it decreases.
Since you have specified a closed container, the amount of gas doesn't change, and the volume that it occupies doesn't change. The only thing that is likely to change is the temperature, and changes in temperature will cause corresponding changes in pressure. And if the pressure gets too high, your closed container is going to explode. So avoid overheating.
If you increase the temperature of a gas, its particles (atoms or molecules) will speed up. If it is in a closed container, the pressure will also increase.
A. temperature B. volume C. number of particles D. size of particles
it lowers the boiling pt temperature
A decrease in temperature or a decrease in the number of gas particles in the container will cause a decrease in gas pressure. Additionally, if some of the gas particles escape from the container, it will also lead to a decrease in pressure.