Effusion and Grahams Law, Daltons Law and non Ideal gases

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Effusion and Grahams Law, Daltons Law and non Ideal gases

Effusion The process by which particles of a gas escape their container through a very small hole. Graham’s law of effusion Rate of effusion of gas 1 Rate of effusion of gas 2 = Molar mass (gas 2) 𝑀𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠 (𝑔𝑎𝑠 1) Basically , the smaller the molar mass of a gas, the faster it will effuse

Daltons law of partial pressure The air you breathe is a mixture of nitrogen, oxygen, argon, carbon dioxide, water vapor, and small amounts of other gases (Table 10.1). Each of these gases exerts its own pressure, and atmospheric pressure is the sum of the pressures exerted by each gas. The pressure of each gas in the mixture is called its partial pressure.

P1 + P 2 ….=Ptotal

Non Ideal gases The ideal gas law works very well for gases at “regular” pressures and temperatures. However it does not work for gases at Extremely high pressures Extremely low temperatures Thinking about the kinetic theory of gases, why would this be? Because of intermolecular forces! Closer (more pressure) or slower = more intermolecular interaction.