IB Chemistry HL Topic 7 Equilibrium FULL PPT

IB Chemistry HL Topic 7 Equilibrium FULL PPT
How equilibrium is affected by pressure, temperature, removal of products or reactants, catalysts. How to solve calculations involving the equilibrium constant Keq, the reaction quotient Q, the solubility constant Ksp and Gibbs free energy G.

This is an earlier PPT video so the sound is a little off. Sorry!

0:0 Introduction
0:19 What is equilibrium?
0:59 The equilibrium constant Keq
1:58 Le Chatelier’s principle
4:01 The Haber process
5:31 Combining Keq
5:40 Reaction Quotient Q
6:15 Solving Q problems (HL)
6:35 Solubility product constant Ksp (HL)
7:11 Solving K problems with RICE diagrams (HL)
8:07 Gibbs and K (HL)

​7.1 Equilibrium
• A state of equilibrium is reached in a closed system when the rates of the forward and reverse reactions are equal.
• The equilibrium law describes how the equilibrium constant (Kc) can be determined for a particular chemical reaction.
• The magnitude of the equilibrium constant indicates the extent of a reaction at equilibrium and is temperature dependent.
• The reaction quotient (Q) measures the relative amount of products and reactants present during a reaction at a particular point in time. Q is the equilibrium expression with non-equilibrium concentrations. The position of the equilibrium changes with changes in concentration, pressure, and temperature.
• A catalyst has no effect on the position of equilibrium or the equilibrium constant.
• The characteristics of chemical and physical systems in a state of equilibrium.
• Deduction of the equilibrium constant expression (Kc) from an equation for a homogeneous reaction.
• Determination of the relationship between different equilibrium constants (Kc) for the same reaction at the same temperature.
• Application of Le Châtelier’s principle to predict the qualitative effects of changes of temperature, pressure and concentration on the position of equilibrium and on the value of the equilibrium constant.

17.1 The equilibrium law
• Le Châtelier’s principle for changes in concentration can be explained by the equilibrium law.
• The position of equilibrium corresponds to a maximum value of entropy and a minimum in the value of the Gibbs free energy.
• The Gibbs free energy change of a reaction and the equilibrium constant can both be used to measure the position of an equilibrium reaction and are related by the equation, ∆G = -RT lnK.
• Solution of homogeneous equilibrium problems using the expression for Kc.
• Relationship between ∆G and the equilibrium constant.
• Calculations using the equation ∆G = -RT lnK

Connect with me:

[soumyasharma]

Mr.Weng. When the forward reaction is favored isn't the concentration of products greater????

[thealterlion]

Hi Mr Weng. My teacher said that the Haber Process is no longer present as questions in the SL syllabus. Is this correct or is my teacher wrong?

[webbiestemu]

This dude goes fast, but still nice vid