University:
The University Of Western Ontario
Course:
2223B | Organic Chemistry of Biological Molecules
Academic year:

2023
Views:

227

Pages:

2
Author:

Cole M.

Gas Phase Absolute Temperature & the Kelvin Scale: Temperature is the measure of the average kinetic energy of the particles within the system Kinetic Energy is known as the energy of motion 9 The °C to °F equation → TF = 5TC + 32 The Kelvin scale never has any negative values (0 is absolute zero meaning there is no kinetic energy) Pressure & the Simple Mercury Barometer: Remember, Pressure is simply a force per unit area (P = F/A) 1 atm is the same as 760 mmHg/Torr or 1.01x105 Pa (N/m2) Definition of an Ideal Gas, Ideal Gas Law: Pressure and Temperature are directly related Pressure and Volume are inversely related Pressure and moles of gas are directly related Ideal Gas Equation is PV = nRT (R is a constant) → USE KELVIN, NOT CELSIUS/FAHRENHEIT BECAUSE YOU 1. 2. 3. DON’T WANT NEGATIVES R = 0.0821 atm L/Kmol = 8.314 J/Kmol = 8.314 Pam3/Kmol An Ideal Gas is a gas that: No intermolecular forces (if there was then this would inhibit the idea that all the KE is directed towards the pressure) Molecules occupy no microscopic volume (point masses) All collisions are perfectly elastic Standard Temperature & Pressure (STP) occurs at a temperature of 0°C and 1 atm Remember, one mol of gas takes up about 22.4 L Also, remember that 1m3 = 1000L Boyle’s Law: If the number of moles and temperature is constant, then P1V1 = P2V2 Although they are multiplied together, remember that they are inversely proportional Charles’s Law: If the number of moles is constant and the pressure doesn't change, then V1/T1 = V2/T2 Although they are divided by one another, they are directly proportional Avogadro’s Law: 1 mol = 6.02x1023 molecules (or atoms) = 22.4 L @STP 1 L = 0.041 mol V/n = a (a is SOME number that is a constant which is similar to R) V1/n1 = V2/n2 The van der Waals Equation: Modification of the ideal gas law in order to take into account how REAL gases work You need to subtract how much volume the actual particles take up and how much their forces take away/give to the pressure ← Van der Waals Equation Partial Pressure: They will give you percentage of mass and you want to know how many moles there are and then you can figure out the partial pressure by inserting it into the ideal gas law Total pressure should equal a summation of ALL of the individual partial pressures