7. Equilibrium Flashcards

1
Q

What are the features of dynamic equilibrium?

A
  • Requires a closed system
  • Forward and reverse reactions are at the same rate
  • Forward and reverse reactions concentrations remain constant.
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2
Q

Define ‘yield’.

A

The amount of product in the equilibrium mixture, usually expressed as a percentage.

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3
Q

Define a ‘homogeneous system’.

A

All reactants, products and catalysts are in the same phase.

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4
Q

Define a ‘heterogeneous system’.

A

One of the chemicals is in a different state.

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5
Q

State Le Chatelier’s principle.

A
  • High pressure favours the side with the fewest moles of gas.
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6
Q

How do catalysts affect equilibrium?

A

They don’t because they increase the rate of both reactions equally.

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7
Q

What happens if you remove a substance from the equilibrium mixture?

A

The position of equilibrium will shift to replace the substance.

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8
Q

What does Kc refer to?

A

The concentration of reactants.

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9
Q

What does a large Kc mean?

A

Lots of products are formed.

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10
Q

What is Kc affected by?

A

Only temperature and stochiometric coefficients.

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11
Q

Kc= ?

A

[products]/ [reactants]

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12
Q

What does it mean if Kc>1?

A

The products are favoured over reactants.

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13
Q

What does it mean if Kc<1?

A

The reactants are favoured over the products.

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14
Q

What does it mean if Kc=1?

A

The mixture contains appreciable amounts of both products and reactants.

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15
Q

What is the effect on Kc if the coefficient is halved?

A

√Kc

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16
Q

What is the effect on Kc if the coefficient is doubled?

A

Kc²

17
Q

What is the effect on Kc if the equation is reversed?

A

1/Kc

18
Q

What is the effect on Kc if the equations are added together?

A

The Kc values are added together.

19
Q

How does an increase in temperature affect an exothermic forward reaction?

A
  • The equilibrium will shift in the endothermic direction (to the left)
  • Yield of products decreases
20
Q

How does an increase in temperature affect an endothermic forward reaction?

A
  • The equilibrium will shift in the endothermic direction (to the right)
  • Yield of products increases
21
Q

What is the reaction quotient?

A

When a system is not at equilibrium, the ratio of concentrations of products and reactants differs from the Kc value.

22
Q

What does it mean if Q>K?

A

There are less reactants and more products than needed for equilibrium, so the reverse reaction will be favoured.

23
Q

What does it mean if Q<K?

A

The mixture contains more reactants and less products than needed for equilibrium, so the forward reaction is favoured.

24
Q

What does it mean if Q=K?

A

Equilibrium has been achieved so the rate of forward and backward reaction will be the same.

25
Q

What is the equation that links K and Gibbs Energy?

A

∆G= -RT lnK

26
Q

What does a negative ∆G value for a reaction indicate?

A
  • The reaction is feasible/ spontaneous
  • The equilibrium concentration of the products is greater than the equilibrium concentration of the reactants.
  • The value of the equilibrium constant will be greater than 1.
27
Q
A