17 Equilibrium (AHL)

1. 17 Equilibrium (AHL) DP Chemistry R. Slider

2. Liquid-Vapour Equilibrium

3. Liquid-Vapour Equilibrium Some molecules at the surface of a liquid gain enough kinetic energy to escape from the surface Vapour particles spread out in the container depending upon the temperature of the system. Some vapour particles now lose energy and move back to the liquid phase. With enough time, there are equal numbers of particles moving from liquid to vapour and back again. Source: http://dluetgens.com/vapor_pressure_equilibrium.html LV Equilibrium - when the rate of condensation and vapourisation is equal.

4. Measuring Vapour Pressure The diagram to the left shows a vessel that can be used to measure vapour pressure. The U-tube contains liquid mercury and clearly shows that a pressure is created by vapour particles filling the vessel. Note that vapour pressure is temperature dependent, but is not affected by volume or surface area Source: http://itl.chem.ufl.edu/2041_u99/lectures/lec_f.html

5. Vapour Pressure vs. Temperature Vapour pressure is temperature dependent Vapour pressure increases exponentially with increased temperature. The graph shows that those substances with a lower boiling point have a higher vapour pressure. WHY? This is due to differences in forces holding molecules together in the liquid phase. Water with H-bonding is held more strongly than ether which has only weak Dispersion forces.

6. Vapour Pressure vs. Temperature Vapour pressure is temperature dependent Kinetic energy increases with an increase in temperature. This shifts the Maxwell-Boltzmann distribution and leads to more particles having enough energy to move into the vapour phase. More vapour particles in the same volume leads to greater vapour pressure

7. Vapour Pressure vs. Temperature These graphs show phase diagrams for water and CO2. “Normal” b.p. values are measured at 1atm. Liquid water can exist up to 3740C with sufficient pressure. Above, it only exists as a gas. This is known as the critical temperature (D on the graph) CO2 can only exist as a liquid above 5.11 atm. This graph also shows why CO2 sublimes at atmospheric pressure (1atm)

8. Enthalpy of Vapourisation (ΔHvap) The amount of energy required to convert 1 mole of a substance to the gas phase is known as the enthalpy of vapourisation in kJ.mol-1. When a substance such as water boils, there is no change in temperature. This can be seen in the graph between D and E. The added energy goes into breaking the attractive forces between particles. • The stronger the attractive forces: • The higher the enthalpy of vapourisation • The lower the vapour pressure at a given temperature • The higher the boiling point

9. Boiling Point This is the temperature where the vapour pressure is equal to the atmospheric pressure. Normal boiling point: the boiling temperature at atmospheric pressure (1atm or 101.3kPa) Source: http://www.tiptoptens.com/2011/05/15/10-highest-mountains-in-the-world/ Source: http://www.sciencephoto.com/media/221314/enlarge At high elevations, water will boil at a lower temperature due to lower atmospheric pressure. A pressure cooker allows water to boil at a higher temperature. This means food cooks much faster.

10. Equilibrium Law Recall that for a system at equilibrium, we can calculate the equilibrium constant Kc For AHL, you will be expected to solve for K, but may also be expected to solve for an equilibrium or starting concentration based on given data. You must practise many different types of problems until you feel comfortable solving these types of questions.

11. Reaction quotient Q Q (the reaction quotient)is similar to K as it is calculated the same way except that the concentrations are taken before equilibrium has been reached. So, If Q < K, the reaction is proceeding forward If Q > K, the reaction is proceeding in reverse You will need to practise these types of problems as well. See your text and your teacher…