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When the volume and number of particles of a gas are constant is also constant?
The temperature and pressure.
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.
Does Charles law the temperature and number of moles stay constant?
Charles' Law: V1/T1 = V2/T2 The number of moles and the pressure are constant.
What happens to pressure on the molecule level when the number of moles of gas is increased at constant volumeWhat happens to the number of collisions with the side of the container?
Pressure in a constant volume (container) is directly proportinal to the number of moles and to the absolute temperature (in K)p :=: n * T with ':=:' meaning 'proportianal to' (not: equal to!)The number of collision is related to and determined by the pressure-value only! (pressure is the result ofcollisions only)
How does the kinetic theory explain the fact that the pressure of a gas in a sealed container remains constant indefinitely provided the volume and temperature are kept constant?
because according to kinetic theory number of collisions exert force per unit area(pressure) so when the temperature is constant along with volume then the same number of collisions are taking place per unit time thats why pressure remains constant....
When the volume and number of particles of a gas are constant is also constant?
The temperature and pressure.
What When the volume and number of particles of a gas are constant is also constant?
The temperature and pressure.
When temperature and number of particles of a gas are constant what is also constant?
The product of pressure and volume. Does PV = nRT look familiar? (:
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.
Volume of a gas increases with increasing temperatures if the pressure is constant?
Pressure*Volume=Number of atoms*gas constant*temperature PV=nRT
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.
How does reducing the volume of a gas affect its pressure if the temperature of a gas and the number of particles are constant?
At a constant temperature, the volume and the pressure are inversely proportional, that it, the greater the volume, the lesser the pressure on the gas, and viceversa.
Does Charles law the temperature and number of moles stay constant?
Charles' Law: V1/T1 = V2/T2 The number of moles and the pressure are constant.
How does reducing the volume of a gas affect it's pressure if the temperature of the gas and the number of particles are constant?
At a constant temperature, the volume and the pressure are inversely proportional, that it, the greater the volume, the lesser the pressure on the gas, and viceversa.
If the pressure and number of particles are constant?
Then the specific volume varies directly with temperature.
The volume of a given mass of an ideal gas at constant pressure is?
directly proportional to the Kelvin temperature
What happens to pressure on the molecule level when the number of moles of gas is increased at constant volumeWhat happens to the number of collisions with the side of the container?
Pressure in a constant volume (container) is directly proportinal to the number of moles and to the absolute temperature (in K)p :=: n * T with ':=:' meaning 'proportianal to' (not: equal to!)The number of collision is related to and determined by the pressure-value only! (pressure is the result ofcollisions only)
