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Chemistry > Chapter 10 > Flashcards

Chapter 10 Flashcards

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1
Q

What is a reversible reaction?

A

A reaction that goes both ways

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2
Q

As the reactants get used up, what happens to the forward reaction?

A

It slows down

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3
Q

As more of the product is formed, what happens to the reverse reaction?

A

It speeds up`

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4
Q

What is a dynamic equilibrium?

A

When the forward reaction will be going at the same rate as the backward reaction, so the amounts of reactants and products will not be changing

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5
Q

At an equilibrium, what happens to the concentration of the reactants and products?

A

The concentrations stay constant

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6
Q

What is a closed system?

A

When nothing can get in or out

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7
Q

What is the only system that a dynamic equilibrium can be achieved in?

A

A closed system

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8
Q

What is the symbol of the equilibrium constant?

A

Kc

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9
Q

What does the equilibrium constant give you an idea of?

A

How far left or right the equilibrium is.

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10
Q

What is a homogeneous system?

A

A system in which everything is in the same state

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11
Q

For a general reaction, aA +bB —> dD + eE, what is the equilibrium constant?

A

K=(D)^d x (E)^e / (A)^a x (B)^b

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12
Q

In the formula of the equilibrium constant, what do the lower case letters represent?

A

The number of moles in each substance

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13
Q

In the formula of the equilibrium constant, what do the upper case letters represent?

A

The concentration in moldm^-3

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14
Q

What is a heterogeneous system?

A

A system where not everything’s in the same state

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15
Q

When calculating the equilibrium constant of a heterogeneous system, what don’t you include in the calculation?

A

Solids or pure liquids, as their concentration stay constant throughout the reaction

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16
Q

Why don’t you include catalysts in expressions for the equilibrium constant?

A

Because catalysts don’t affect the equilibrium concentrations of the products or reactants

17
Q

What can you use to achieve a dynamic equilibrium quicker?

A

A catalyst

18
Q

What does le chatelier’s principle predict?

A

What will happen if conditions are changed

19
Q

If you move the position of the equilibrium to the left, what will you get more of?

A

The reactants

20
Q

If the position of the equilibrium moves to the right, what will you get more of?

A

The products

21
Q

If there’s a change in the concentration, pressure or temperature, what will happen to the position of the equilibrium?

A

It will change

22
Q

If you increase the concentration of the reactant, what does the equilibrium do?

A

It tries to get rid of the extra reactant, so it makes more product, so the equilibrium is shifted to the right

23
Q

What state does increasing the state only affect?

A

Gases

24
Q

What does increasing the pressure do to the position of the equilibrium?

A

It shifts the equilibrium to the side with fewer gas molecules, in order to reduce the pressure

25
Q

What does increasing the temperature of a reaction do to the position of the equilibrium?

A

It shifts it in the endothermic reaction

26
Q

What does decreasing the temperature of a reaction do to the position of the equilibrium?

A

It shifts it in the endothermic direction

27
Q

In an industrial process, what balance has to be achiveved?

A

A balance between high rate and high yield

28
Q

What can ethanol be formed from?

A

Ethene and steam

29
Q

Is the forward reaction of the production of ethanol a endothermic or exothermic reaction?

A

It is an exothermic reaction

30
Q

What pressure and temperature is ethanol formed at?

A

60-70 atmospheres and 300C

31
Q

Despite the forward reaction of ethanol being exothermic, what is the negative consequence of low temperatures?

A

A slower rate of reaction

32
Q

Why do you use a fairly high pressure in the production of ethanol?

A

Because it favours the forward reaction

Chemistry (25 decks)

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