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Chemistry > Chemical Equilibrium [Unit 3] > Flashcards

Chemical Equilibrium [Unit 3] Flashcards

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1
Q

Reversible Reaction

A

A reaction which proceeds in both the forward and reverse direction

  • Indicated by ⇌
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2
Q

Forward Reaction

A

→ Forming products

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3
Q

Reverse Reaction

A

← Forming reactants

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4
Q

Equilibrium

A

The point in a reversible reaction where there is no change in the concentration of products and reactants

  • Where the rate of the forward and reverse reactions are equal
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5
Q

Dynamic Equilibrium

A

Both the forward and reverse reactions are occurring

  • No change overall
  • Steady-state (Properties are constant)
  • Only occurs in a closed system
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6
Q

Static Equilibrium

A

The forward and reverse reactions do not occur

  • No change at all
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7
Q

Rate of Reaction

A

How fast a reaction takes place

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8
Q

Extent of a Reaction

A

How many of the reactants are turned into products in the time taken to reach equilibrium

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9
Q

Closed System

A

Does not allow matter to be transferred with the surroundings

  • Energy can be transferred to and from the surroundings
  • Has a lid
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10
Q

Open System

A

Matter and energy can be transferred to and from the surroundings

  • Reactants or products may be lost to the environment
  • Prevents equilibrium from being reached
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11
Q

Parts of a Chemical System

A
  • Boundary - Barrier between chemical and surroundings (E.g. The glassware/beaker)
  • System - Chemicals involved in the reaction
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12
Q

Links between Collision Theory and Equilibrium

A
  • As reactants are used up, the forward reaction slows down
  • As more product is formed, the reverse reaction speeds up

Eventually a point is reached where the rates are equal and equilibrium is reached

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13
Q

In Collision Theory Particles Must:

A
  • Collide with at least a minimum amount of kinetic energy
  • Collide with the correct orientation
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14
Q

Application of Collision Theory

A
  1. What happens to the reactants and products over time?
  2. How does that affect the number of collisions between reactants and products?
  3. Do more reactant or product particles now satisfy the conditions of collision theory?
  4. What happens to the rate of the forward and reverse reaction?
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15
Q

Application of Collision Theory in a Forward Reaction

A
  1. Reactants decrease over time - Less particles
  2. Fewer particles = Less collisions
  3. Less reactant particles meet the conditions of collision theory - Lower concentration = Less collisions
  4. Fewer successful collisions → Decrease in the rate of the forward reaction
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16
Q

Application of Collision Theory in a Reverse Reaction

A

Chemistry (13 decks)

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