Reversible Reactions and the Haber Process Flashcards Preview

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Flashcards in Reversible Reactions and the Haber Process Deck (20)
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1
Q

What is a reversible reaction?

A

One where the products of the reaction can themselves react to produce the original reactants.

2
Q

What kind of system is needed to reach equilibrium?

A

Closed system.

3
Q

What is the equilibrium position?

A

The amounts of reactants and products reach a balance and stay there.

4
Q

What is happening at the equilibrium position?

A

Reactions are taking place at exactly the same rate in both directions.

5
Q

What does the equilibrium position depend on?

A
  1. Temperature

2. Pressure

6
Q

Which direction does increasing the temperature move the equilibrium in?

A

The endothermic direction.

7
Q

Which direction does decreasing the temperature move the equilibrium in?

A

The exothermic direction.

8
Q

Which direction does raising the pressure move the equilibrium position in?

A

The reaction which produces less volume.

9
Q

Which direction does reducing the pressure move the equilibrium position in?

A

The reaction which produces more volume.

10
Q

How does adding a catalyst affect the equilibrium position?

A

It doesn’t, but it reaches equilibrium quicker.

11
Q

What is ammonia made of?

A

Nitrogen and hydrogen.

12
Q

Where does the nitrogen come from?

A

The air.

13
Q

Where does the hydrogen come from?

A

Natural gas or other sources.

14
Q

What are the industrial conditions for ammonia production?

A
  1. 200 atmospheres of pressure
  2. 450C
  3. Iron catalyst
15
Q

Why is the pressure for ammonia production high?

A

To increase the forward reaction - maximum yield.

16
Q

Why is the pressure for ammonia not 1000 atmospheres?

A

It would be too expensive to build such a plant.

17
Q

Why is the temperature for ammonia production high?

A

To increase the rate of reaction.

18
Q

What is the temperature a compromise between?

A
  1. Maximum yield

2. Speed of reaction

19
Q

What happens to the ammonia when it is formed?

A

It is formed as a gas, so it’s condensed.

20
Q

Why is the catalyst important in the Haber process?

A

Without it, a higher temperature would have to be used, reducing the yield further.