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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)
What else can I help you with?
What happens to the temperature increase the number of particles what happens to the pressure?
Increasing the temperature the number of particles remain constant and the pressure increase.
What happens to molecules as their kinetic energy increases?
They move faster, number of collision increases,also the temperature increases.
Is the number of dissolved particles related to the temperature change?
Yes, the number of dissolved particles in a solution typically increases with temperature. As the temperature rises, particles gain more energy and move faster, which can disrupt the forces holding them in the solid phase, leading to more particles dissolving in the solution.
According to kinetic and collision theory why does increasing the temperature of the reaction increase the rate of reaction?
Increasing the temperature of a reaction increases the average kinetic energy of the molecules involved. This results in more frequent and energetic collisions between the molecules, leading to a higher probability of successful collisions that result in a reaction. In essence, increasing the temperature increases both the number of collisions and the proportion of collisions that have enough energy to overcome the activation energy barrier.
When the temperature of a gas gets higher what does its pressure do?
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.
What happens to the temperature increase the number of particles what happens to the pressure?
Increasing the temperature the number of particles remain constant and the pressure increase.
What happens to molecules as their kinetic energy increases?
They move faster, number of collision increases,also the temperature increases.
Is the number of dissolved particles related to the temperature change?
Yes, the number of dissolved particles in a solution typically increases with temperature. As the temperature rises, particles gain more energy and move faster, which can disrupt the forces holding them in the solid phase, leading to more particles dissolving in the solution.
What happens to the number of free electrons and holes in an intrinsic semiconductor when the temperature decreases?
increases
What happens to the average kinetic energy of the particles the pressure and number of collisions when the temperature is decreased?
When the temperature is decreased, the average kinetic energy of particles decreases since temperature is directly related to the average kinetic energy of particles. As a result, the pressure and number of collisions between particles will also decrease because particles will have less energy to move and collide with each other.
How does increasing the temperature affect collisions?
It increases the number of high-energy collisions
What effect does raising the temperature of a gas have on its pressure if the volume of the gas and the number of particles are kept constant?
Raising the temperature of a gas will increase its pressure, following the ideal gas law (PV = nRT). As temperature increases, the average kinetic energy of the gas particles also increases, leading to more frequent and forceful collisions with the walls of the container, resulting in higher pressure.
What is the temperature of a gas proportional to?
General Gas Law: p.V = n.R.T , soT = p.V/nR , hence Temperature is direct proportional to pressure and Volume.T = temperature, p = pressure, V = volume, n = number of moles,and R = gas constant
According to kinetic and collision theory why does increasing the temperature of the reaction increase the rate of reaction?
Increasing the temperature of a reaction increases the average kinetic energy of the molecules involved. This results in more frequent and energetic collisions between the molecules, leading to a higher probability of successful collisions that result in a reaction. In essence, increasing the temperature increases both the number of collisions and the proportion of collisions that have enough energy to overcome the activation energy barrier.
Do the number of particles in an object affect its thermal energy but not its temperature?
Yes, the number of particles in an object does affect its thermal energy, as thermal energy is directly proportional to the number of particles. However, the number of particles does not affect its temperature, as temperature is a measure of the average kinetic energy of the particles.
How are pressure and the number of the particle related?
PV = NkT P: pressure V: volume N: number of particles in gas k: Boltzmann's constant T: absolute temperature More particles in a constant volume, constant temperature space means more pressure.
If the pressure and number of particles are constant?
If the pressure and number of particles are constant, then according to Boyle's Law, the volume of the gas is inversely proportional to its pressure. This means that as the pressure increases, the volume decreases and vice versa, as long as the number of particles remains the same.
