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1) Particles do not take up space.
2) Particles bounce off of each other without losing energy.
3) Particles are not attracted to one another. (no intermolecular forces)
3 Rules for ideal gases (vs real gases)
1) Particles are small and inert.
2) Temperature is high.
3) Pressure is low.
3 Conditions when real gases act almost exactly like ideal gases.
1) Temperature must be in kelvins
2) Units for P1 must match P2 (and units for V1 must match V2)
2 Rules for units on the combined gas law (P₁V₁ / T₁ = P₂V₂ / T₂)
1) The right side of the equation flips so that 2 is over 1.
2) Rate = amount/time
2 Rules for on Graham's Law
Rate₁/Rate₂ = sq rt(M₂)/sq rt (M₁)
(all units must match the gas constant R)
1) Temperature must be in kelvins.
2) Pressure must be in atm.
3) Volume must be in L.
3 Rules for units on Ideal gas law
(PV = nRT)
Mass can be used to find n (or conversely, n can be used to find mass) by converting between moles and grams.
Mass in the ideal gas law
(PV = nRT)
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