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Semester 2 Chemistry Revisions > Lecture 5 > Flashcards

Lecture 5 Flashcards

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1
Q

What is equilibrium?

A

A state in which there are NO observable CHANGES over time.

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2
Q

What are the requirements for equilibrium?

A

CLOSED SYSTEM
CONSTANT TEMPERATURE and PRESSURE.
REVERSIBLE process/ reaction.
Rates of opposing changes are EQUAL.

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3
Q

What are the properties of equilibrium systems?

A

DYNAMIC, in constant motion.
REVERSIBLE
Approach from either DIRECTION.
Both REACTANTS and PRODUCTS present at ALL times.

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4
Q

When will a reaction reach dynamic equilibrium?

A

When the rate of the forwards reaction is equal to the rate of the backwards reaction.

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5
Q

What is the Reaction Quotient?

A

CONCENTRATION of products and reactants to each other at ANY POINT in a reaction.

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6
Q

Reaction Quotient equation:

A

Q= [C]c[D]d/ [A]a[B]b

[Products]/ [Reactants]

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7
Q

What is the equilibrium constant?

A

The value of the reaction quotient at EQUILIBRIUM.

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8
Q

What is Kc?

A

Concentration Equilibrium Constant.

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9
Q

What do you not include in Kc or Kp equations?

A

SOLVENTS or SOLIDS

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10
Q

What is a homogenous equilibria?

A

Reactants and products are in the SAME physical STATES.

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11
Q

What is a heterogeneous equilibria?

A

Reactants and products are in DIFFERENT physical STATES.

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12
Q

What does K allow us to do?

A

PREDICT how a reaction will PROGRESS to achieve equilibrium.
CALCULATE the CONCENTRATION of reactants and products at equilibrium.

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13
Q

If there is a small Kc (less than one) what does this tell us about the reaction?

A

Favours reactants.
Equilibrium lies to LHS.
Little reaction occurs.

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14
Q

If there is a large Kc, what does this tell us about the reaction?

A

Favours products.
Equilibrium lies to RHS.
Reaction nearly complete.

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15
Q

If Kc is less that one what does this tell an individual about ΔG? Why?

A

The reaction is not spontaneous.

The log of a number smaller than one will be a MINUS and a MINUS + MINUS is POSITIVE so ΔG is NOT SPONTANEOUS.

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16
Q

What is Le Chatelier’s principal?

A

“When a change is applied to a system in dynamic equilibrium, the system reacts to oppose the effect.”

17
Q

What does Le chatelier’s principal mean?

A
  • A system at equilibrium under STRESS will SHIFT to RELIEVE the stress.
  • There will be a CHANGE in the rate of the forwards or reverse reaction to RETURN the system to equilibrium.
18
Q

What is the only thing that can change the value of the equilibrium constant?

A

Temperature.

19
Q

Why does temperature alter the equilibrium constant?

A

Altering the temperature affects both the forwards and backwards reaction but alters the two rates to DIFFERENT extents. Therefore the equilibrium moves producing a new equilibrium constant.

20
Q 
CONCENTRATION: What will happen to the reaction if you:
Add reactant
Remove reactant
Add product
Remove product
A

Forward
Back
Back
Forward

21
Q

PRESSURE: What will happen to the reaction if you:
Increase
Decrease

A

Towards fewer moles of gas.

Towards more moles of gas.

22
Q

For an endothermic reaction what happens when you:
Increase the temperature
Decrease the temperature

A

Forward K changes

Reverse K changes

23
Q

For an exothermic reaction what happens when you:
Increase the temperature
Decrease the temperature

A

Reverse K changes

Forward K changes

24
Q

What happens when you add a catalyst to an equilibrium reaction? Why?

A

Increases rate equally, but does not affect the position of equilibrium because the rate of both reactions is affected equally.

25
Q

Name an example of when changing concentration of an equilibrium is evident in the Human body.

A

Osmosis

26
Q

Name an example of when changing pressure of an equilibrium is evident in the Human body.

A

HAEMBOGLOBIN BINDING and RELEASING O2.

Semester 2 Chemistry Revisions (12 decks)

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