Dynamic Equilibrium

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6 Terms

1
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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

2
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We use WHAT to show this relationship

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eg: A + B → ← C + D

3
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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

4
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  1. 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

  2. As the products C and D are formed, the WHAT reaction slows down and the WHAT reaction will speed up

  3. At some point the rates of forward and reverse reactions become WHAT

  1. 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

  2. As the products C and D are formed, the FORWARD reaction slows down and the REVERSE reaction will speed up

  3. At some point the rates of forward and reverse reactions become EQUAL

5
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A system is said to be un a state of WHAT equilibrium when:

  1. The WHAT of the forward and reverse reactions are WHAT

  2. The WHAT (macroscopic) properties of the system, such as temperature, pH, pressure, concentration are WHAT

  3. The system is a WHAT system at CONSTANT WHAT

A system is said to be un a state of DYNAMIC equilibrium when:

  1. The RATES of the forward and reverse reactions are EQUAL

  2. The OBSERVABLE (macroscopic) properties of the system, such as temperature, pH, pressure, concentration are CONSTANT

  3. The system is a CLOSED system at CONSTANT TEMPERATURE

6
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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