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Chemistry > Chapter 11 > Flashcards

Chapter 11 Flashcards

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1
Q

What is Kc?

A

Kc is the equilibrium constant

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2
Q

What is the equilibrium constant calculated from?

A

The ratio of the product concentration compared to the reactant concentration

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3
Q

For the reaction H2 + I2 –> 2HI, what is the equation for the equilibrium constant?

A

kc = (HI squared) / (H2 X I2)

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4
Q

What does the definition of Kc only apply to?

A

Homogenous equilibria

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5
Q

What is a homogenous equilibria?

A

An equilibria where all the products and reactants are in the same phase

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6
Q

In a heterogenous equilibria, is everything included in the expression for Kc?

A

Not nececarily

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7
Q

What don’t you include in the expression for Kc?

A

Solids or liquids

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8
Q

Why don’t you include solids or liquids in the expression for Kc?

A

Because their concentrations stay constant throughout the reaction

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9
Q

When calculating the value of Kc, what are the concentrations?

A

The concentration at equilibrium

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10
Q

What will Fe2+ and Ag+ form an equilibrium with?

A

Fe3+ and Ag

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11
Q

How can you work out the equilibrium constant of a reaction between Fe2+ and Ag+ ions?

A

Titrate them, to calculate the equilibrium concentration of Fe2+ ions. From this you can calculate the equilibrium concentrations of the other components, and Kc

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12
Q

What do the square brackets represent in a Kc expression?

A

The square brackets represent the equilibrium concentrations

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13
Q

What do the powers represent in a Kc expression?

A

The powers represent the number of moles of each substance

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14
Q

What is the total pressure equal to?

A

The sum of the partial pressures

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15
Q

What is a mole fraction?

A

The proportion of a gas mixture that is a particular gas

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16
Q

What does the mole fraction of a gas in a mixture equal?

A

Number of moles in gas / Total Number of moles of gas in mixture

17
Q

What does the partial pressure of a gas equal?

A

Mole fraction of gas X total pressure of mixture

18
Q

What is Kp?

A

An equilibrium constant you can calculate when dealing with equilibria involving gases

19
Q

What is the difference between Kp and Kc?

A

With Kp you deal with partial pressures

20
Q

What is the unit of a partial pressure?

A

Atmosphere

21
Q

When calculating Kp for heterogenous equilibria, what does the calulation only involve?

A

Gases

22
Q

For a reaction where a solid S decomposes to form gases P and Q, what is the expression for Kp?

A

P(P)p(Q)

23
Q

When a reversible reaction reaches a dynamic equilibrium, what happens?

A

The forward reaction happens at the same rate as the backward reaction

24
Q

If you change the concentration, pressure or temperature of a reversible reaction, what are you going to do?

A

You are going to alter the position of the equilibrium

25
Q

What is Le Chatelier’s principle?

A

If there’s a change in concentration, pressure or temperature, the equilibrium will move to help counteract the change

26
Q

What does the greater the value of Kp or Kc mean?

A

The greater the value the further to the right the equilibrium lies

27
Q

What does the smaller the value of Kp or Kc mean?

A

The smaller the value the further to the left the equilibrium lies

28
Q

If the forward reaction is exothermic, and the temperature of the reaction is increased, what happens to the value of Kp?

A

The value of Kp decreases as there is less product

29
Q

If the backward reaction is endothermic, why does the position of the equilibrium shift to the left when the temperature is raised?

A

The equilibrium shifts to the left to absorb the extra heat

30
Q

As the value of the equilibrium constant is fixed at a given temperature, what happens if the concentration of one thing in the mixture changes?

A

The concentrations of the others must change to keep the value of Kc the same

31
Q

What does increasing the total pressure do?

A

It increases the partial pressures of each of the products and reactants

32
Q

Do catalysts effect the position of the equilibrium?

A

No, but they do mean an equilibrium can be reached faster

Chemistry (25 decks)

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