Although it isn't always accurate - especially at high pressures - the ideal gas law is a good, simple way of looking at the general relationship between pressure, volume, temperature and total number of particles in a gas.
According to the Ideal Gas Law:
PV = nRT
where
P is pressure, V is volume, n is the number of particles, R is the ideal gas constant , and T is absolute temperature.
If the system is closed, then by definition the number of particles remains the same even if volume changes. If the system is NOT closed, then the question is not sufficiently constrained to predict what will happen to the number of particles.
Assuming a closed system, if the volume increases then either the pressure must decrease or the temperature increase (or both).
If pressure is held constant, the temperature must increase to keep the pressure stable.
If the pressure is allowed to fall, the temperature may actually remain the same.
If the process is adiabatic, both the pressure and the temperature will decrease (for most gases - hydrogen and helium have a range where they actually heat up as they expand)
Assuming the pressure remains constant, the temperature will increase as the volume increases, and the number of particles will remain the same unless you add or remove some gas.
Increasing the temperature the number of particles remain constant and the pressure increase.
They move faster, number of collision increases,also the temperature increases.
The likelihood that two particles will collide in a given time increases. The number of particles per volume increases.
As the number of gaseous particles increase, the rate of condensation increases because more and more gaseous particles are coming into contact with the liquid surface.
Increase. As the temperature increases, the particles hit the walls of the container more often and with more force. This causes the pressure to increase, since the definition of pressure is the number and force of collisions the particles have with the walls of its container.
Increasing the temperature the number of particles remain constant and the pressure increase.
They move faster, number of collision increases,also the temperature increases.
increases
As per Charles' law pressure increases as temperature increases provided volume is kept constant
The likelihood that two particles will collide in a given time increases. The number of particles per volume increases.
It increases the collisions that have enough energy to react (apex)
As the number of gaseous particles increase, the rate of condensation increases because more and more gaseous particles are coming into contact with the liquid surface.
An objects temperature and the number of particles
Increase. As the temperature increases, the particles hit the walls of the container more often and with more force. This causes the pressure to increase, since the definition of pressure is the number and force of collisions the particles have with the walls of its container.
If temperature increases, then pressure increases. Temperature measures the average speed of particles, so if the temperature is high, then the particles are moving quickly and are colliding with other particles more forcefully. Pressure is defined as the force and number of collisions the particles have with the wall of its container. So if the high temperature causes the particles to move quickly, they are going to collide more often with the container, increasing the pressure. This remains true as long as the number of moles (n) remains constant.
It increases It increases
supply increases