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Combining the previous gas laws, the ideal gas law is obtained
Example
A gas occupies 250 mL, and its pressure is 550 mmHg at 25°C.
If the gas is expanded to 450 mL, what is the pressure of the gas now?
What temperature is needed to increase the pressure of the gas to exactly 1 atmosphere and 250 mL?
How many moles of gas are in this sample?
The sample is an element and has a mass of 0.525g. What is it?
Kinetic molecular theory describes gasses at the particle level.
Pressure is determined by the velocity of gas particles colliding with container walls. Changing temperature changes the force of collision in addition to the frequency.
If the volume of a container is decrease, the particles will collide with the wall more frequently, and pressure will increase
By increasing temperature, the average kinetic energy is increase so the particle velocity is increased, and the pressure will increase since the collisions are stronger
Graham’s law of effusion compares the rate of effusion of two gasses and says the rates are inversely related to the square root of the mass of the gas particles
Effusion through a pinhole in a vacuum requires a gas to hit the pinhole just right in order to escape. More collisions mean a higher rate of effusion, or a higher likelihood that it will escape.
Dalton’s law of partial pressures says that if two gasses are mixed together, they will act independently of each other.
Example
A mixture of gasses contain 2 mol of O2, 3 mol of N2, and 5 mol of He. Total pressure is 850 torr. What is the partial pressure of each gas?
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