🧪
Equilibrium, acids and redox
reactions
Class Chemistry
Created Sep 21, 2020 101 PM
Property ©Isha Shin 2020
Reviewed
Unit Unit 3
Chemical Equilibrium Systems 1
Chemical Equilibrium 1.1
How does a chemical reaction occur?
Activation energy is required to initiate the reaction. The smaller the Ea,
the more readily the reaction forms products. Overtime, concentration of
reactants decrease, and products increase (forward reaction)
Compare open and closed chemical systems
Explain concept of Dynamic Equilibrium
Physical reactions and some chemical reactions (reversible), reach a state
of equilibrium when the rate of forward and reverse reaction are equal.
The reaction is incomplete, bonds are being broken and re-formed
simulteneously
What observable changes in chemical reactions and physical changes can be
described and explained at atomic and molecular level?
Equilibrium, acids and redox reactions 1
, Colour change
Formation of precipitate/gas bubbles
Temperature change
Collisions - Kinetic energy
Changes in concentration measured by pH and observations.
How does reversibility take place?
Some reactants do not lose products, and can be contained within a
reaction vessel, so can proceed both forwards and backwards. Energy
profile is reversed, activation energy and enthalpy change.
Factors that affect equilibrium 1.2
State Le Châtelier's principle
If an equilibrium system is subjected to a change, the system will adjust
itself to partially oppose the effect of the change.
Stress changes
What is the effect of temperature change on systems at equilibrium
(considering enthalpy change)?
Exothermic reactions: products have more energy that reactants, so an
increase in temperature favours the reactants (less energy side)
Endothermic reactions: reactants have more energy than products, so
increase in temperature favours the products.
Energy profile diagrams
What is the effect on concentration and/or pressure change of systems at
equilibrium (considering collision theory)?
Adding or removing reactants/products: when reactant concentration
increased, system moves to product side (forward reaction). This is
Equilibrium, acids and redox reactions 2
Equilibrium, acids and redox
reactions
Class Chemistry
Created Sep 21, 2020 101 PM
Property ©Isha Shin 2020
Reviewed
Unit Unit 3
Chemical Equilibrium Systems 1
Chemical Equilibrium 1.1
How does a chemical reaction occur?
Activation energy is required to initiate the reaction. The smaller the Ea,
the more readily the reaction forms products. Overtime, concentration of
reactants decrease, and products increase (forward reaction)
Compare open and closed chemical systems
Explain concept of Dynamic Equilibrium
Physical reactions and some chemical reactions (reversible), reach a state
of equilibrium when the rate of forward and reverse reaction are equal.
The reaction is incomplete, bonds are being broken and re-formed
simulteneously
What observable changes in chemical reactions and physical changes can be
described and explained at atomic and molecular level?
Equilibrium, acids and redox reactions 1
, Colour change
Formation of precipitate/gas bubbles
Temperature change
Collisions - Kinetic energy
Changes in concentration measured by pH and observations.
How does reversibility take place?
Some reactants do not lose products, and can be contained within a
reaction vessel, so can proceed both forwards and backwards. Energy
profile is reversed, activation energy and enthalpy change.
Factors that affect equilibrium 1.2
State Le Châtelier's principle
If an equilibrium system is subjected to a change, the system will adjust
itself to partially oppose the effect of the change.
Stress changes
What is the effect of temperature change on systems at equilibrium
(considering enthalpy change)?
Exothermic reactions: products have more energy that reactants, so an
increase in temperature favours the reactants (less energy side)
Endothermic reactions: reactants have more energy than products, so
increase in temperature favours the products.
Energy profile diagrams
What is the effect on concentration and/or pressure change of systems at
equilibrium (considering collision theory)?
Adding or removing reactants/products: when reactant concentration
increased, system moves to product side (forward reaction). This is
Equilibrium, acids and redox reactions 2
