# Equilibrium
# Roadmap
# What is Equilibrium?
# Equilibrium constant
Equilibrium expression
Calc Kc from [eqm]
Manipulating Kc
# Q
prediction perturb
# La Chatelier
# Eqm calculations
7.1.NoS1
Obtaining evidence for scientific theoriesâisotopic labelling and its use in defining equilibrium. (1.8)
7.1.NoS2
Common language across different disciplinesâthe term dynamic equilibrium is used in other contexts, but not necessarily with the chemistry definition in mind. (5.5)
7.1.U1
A state of equilibrium is reached in a closed system when the rates of the forward and reverse reactions are equal.
7.1.U2
The equilibrium law describes how the equilibrium constant (Kc) can be determined for a particular chemical reaction.
7.1.U3
The magnitude of the equilibrium constant indicates the extent of a reaction at equilibrium and is temperature dependent.
7.1.U4
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.
7.1.U5
A catalyst has no effect on the position of equilibrium or the equilibrium constant.
7.1.AS1
The characteristics of chemical and physical systems in a state of equilibrium.
7.1.AS2
Deduction of the equilibrium constant expression (K_{c}) from an equation for a homogeneous reaction.
7.1.AS3
Determination of the relationship between different equilibrium constants (Kc) for the same reaction at the same temperature.
7.1.AS4
Application of Le Châtelierâs 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.
7.1.G1
Physical and chemical systems should be covered.
7.1.G2
Relationship between Kc values for reactions that are multiples or inverses of one another should be covered.
7.1.G3
Specific details of any industrial process are not required.
7.1.IM1
The Haber process has been described as the most important chemical reaction on Earth as it has revolutionized global food production. However, it also had a large impact on weaponry in both world wars.
7.1.ToK1
Scientists investigate the world at different scales; the macroscopic and microscopic. Which ways of knowing allow us to move from the macroscopic to the microscopic?
7.1.ToK2
Chemistry uses a specialized vocabulary: a closed system is one in which no matter is exchanged with the surroundings. Does our vocabulary simply communicate our knowledge; or does it shape what we can know?
7.1.ToK3
The career of Fritz Haber coincided with the political upheavals of two world wars. He supervised the release of chlorine on the battlefield in World War I and worked on the production of explosives. How does the social context of scientific work affect the methods and findings of science? Should scientists be held morally responsible for the applications of their discoveries?
7.1.Uz1
Square brackets are used in chemistry in a range of contexts: eg concentrations (topic 1.3), Lewis (electron dot) structures (topic 4.3) and complexes (topic 14.1).
7.1.Aims1
Aim 6: Le Châtelierâs principle can be investigated qualitatively by looking at pressure, concentration and temperature changes on different equilibrium systems.
7.1.Aims2
Aim 7: Animations and simulations can be used to illustrate the concept of dynamic equilibrium.
7.1.Aims3
Aim 8: Raise awareness of the moral, ethical, and economic implications of using science and technology. A case study of Fritz Haber can be used to debate the role of scientists in society.
17.1.NoS
Employing quantitative reasoningâexperimentally determined rate expressions for forward and backward reactions can be deduced directly from the stoichiometric equations and allow Le Châtelierâs principle to be applied. (1.8, 1.9)
17.1.U1
Le Châtelierâs principle for changes in concentration can be explained by the equilibrium law
17.1.U2
The position of equilibrium corresponds to a maximum value of entropy and a minimum in the value of the Gibbs free energy
17.1.U3
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, âG = âRT lnK .
17.1.AS1
Solution of homogeneous equilibrium problems using the expression for Kc.
17.1.AS2
Relationship between âG and the equilibrium constant.
17.1.AS3
Calculations using the equation âG = âRT lnK.
17.1.G1
The expression âG = âRT lnK is given in the data booklet in section 1.
17.1.G2
Students will not be expected to derive the expression âG = âRT lnK.
17.1.G3
The use of quadratic equations will not be assessed
17.1.ToK1
The equilibrium law can be deduced by assuming that the order of the forward and backward reaction matches the coefficients in the chemical equation. What is the role of deductive reasoning in science?
17.1.ToK2
We can use mathematics successfully to model equilibrium systems. Is this because we create mathematics to mirror reality or because the reality is intrinsically mathematical?
17.1.ToK3
Many problems in science can only be solved when assumptions are made which simplify the mathematics. What is the role of intuition in problem solving?
17.1.Uz1
The concept of a closed system in dynamic equilibrium can be applied to a range of systems in the biological, environmental and human sciences.
17.1.Aims1
Aim 6: The equilibrium constant for an esterification reaction and other reactions could be experimentally investigated.
17.1.Aims2
Aim 7: The concept of a dynamic equilibrium can be illustrated with computer animations.
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