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Reactions are often WHAT which means taht not only are the products WHAT but the reactants can be WHAT
Reactions are often REVERSIBLE which means taht not only are the products FORMED but the reactants can be REFORMED
We use WHAT to show this relationship
Double arrows
eg: A + B → ← C + D
The forward and reverse reactions will proceed at different WHAT… it depends on the WHAT of the reactants and products
The forward and reverse reactions will proceed at different RATES… it depends on the CONCENTRATION of the reactants and products
If we start with only the reactants A and B, the WHAT reaction will initially be the WHAT as it is the only WHAT possible
As the products C and D are formed, the WHAT reaction slows down and the WHAT reaction will speed up
At some point the rates of forward and reverse reactions become WHAT
If we start with only the reactants A and B, the FORWARD reaction will initially be the FASTEST as it is the only REACTION possible
As the products C and D are formed, the FORWARD reaction slows down and the REVERSE reaction will speed up
At some point the rates of forward and reverse reactions become EQUAL
A system is said to be un a state of WHAT equilibrium when:
The WHAT of the forward and reverse reactions are WHAT
The WHAT (macroscopic) properties of the system, such as temperature, pH, pressure, concentration are WHAT
The system is a WHAT system at CONSTANT WHAT
A system is said to be un a state of DYNAMIC equilibrium when:
The RATES of the forward and reverse reactions are EQUAL
The OBSERVABLE (macroscopic) properties of the system, such as temperature, pH, pressure, concentration are CONSTANT
The system is a CLOSED system at CONSTANT TEMPERATURE
Just because a reaction has reached equilibrium the WHAT of reactants and products are NOT WHAT
Just because a reaction has reached equilibrium the CONCENTRATION of reactants and products are NOT EQUAL