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Equilibrium and Acid Reactions - Coggle Diagram
Equilibrium and Acid Reactions
Static and Dynamic Equilibrium
Reversibility of chemical reactions
Cobalt(II) chloride hydrated and dehydrated
Iron(III) nitrate and potassium thiocyanate
Burning magnesium
Burning steel wool
Models of static and dynamic equilibrium and differences between open and closed systems
Examples of non-equilibrium systems in terms of the effect of entropy and enthalpy
Combustion reactions
Photosynthesis
Relationship between collision theory and reaction rate
Factors that affect equilibrium
Le Chatelier's Principle; effects of temperature, concentration, volume and/or pressure on a system at equilibrium
Heating cobalt(II) chloride hydrate
Interaction between nitrogen dioxide and dinitrogen tetroxide
Iron(III) thiocyanate and varying concentration of ions
Overall observations about equilibrium in terms of the collision theory
How activation energy and heat of reaction affect the position of equilibrium
Calculating the equilibrium constant (Keq)
Equilibrium expression (in terms of Keq) for homogeneous reactions occurring in solution
Finding the value of Keq and concentrations of substances within an equilibrium system, and using these values to make predictions on the direction in which a reaction may proceed
Qualitative effect of temperature on the value of Keq
Investigation to determine Keq of a chemical equilibrium system
Keq of the iron(III) thiocyanate equilibrium
Use of Keq for different types of chemical reactions
Dissociation of ionic solutions
Dissociation of acids and bases
Solution equilibria
Processes involved in the dissolution of ionic compounds in water
Use of solubility equilibria by Aboriginal and Torres Strait Islander Peoples when removing toxicity from foods
Toxins in cycad fruit
Solubility rules and prediction of the composition of substances when two ionic solutions are mixed
Potassium chloride and silver nitrate
Potassium iodide and lead nitrate
Sodium sulfate and barium nitrate
Equilibrium expressions for saturated solutions in terms of Ksp and the solubility of an ionic substance from its Ksp value
Prediction of a formation of a precipitate given the standard reference values for Ksp