Nature of Chemical Reactions/Equilibrium Flashcards

1
Q

Open and closed systems

A

Open system
- can exchange matter and energy with the surroundings

Closed system
- can only exhange energy with their surroundings

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2
Q

Reversible and irreversible reactions

A

Reversible
- when products can be used to reform reactants
- reactions that can proceed in the forward and backwards direction
- can only occur in a closed system

Irreversible
- reactions that can only proceed in the forward direction

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3
Q

Equilibrium

A
  • when the rate of production of products is = to rate of reformation of reactants in a reversible reaction

dynamic equilibrium
- when the forward/backward reactions are still occuring

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4
Q

When is equilibirum determiend in a concentration/time graph

A
  • as the concentration of reactants decrease, concentration of products increase
  • over time, concentration of both level off and become constant –> equilibrium
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5
Q

Why does concentration never = zero

A
  • as more products produced, greater chance of reactants being re-formed
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6
Q

what can concentration/time graphs indicate

A

The rate of reaction
- the steeper the curve, the quicker the RoR / the more that is being made at the point in time

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7
Q

Position of equilibrium

A
  • compares the concentration of products/reactants at equilibrium
  • if PoE lies to the right –> the reaction favours the products
  • if PoE lies to the left –> reaction favours the production of reactants
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