3.5 Chemical Equilibrium Flashcards

1
Q

What is a reversible reaction?

A

The products can react together to make the reactants again

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2
Q

What is a closed system of a reaction?

A

No products or reactants can escape

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3
Q

What is equilibrium?

A

The balance point where both reactions happen at the same time

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4
Q

When is equilibrium reached in a closed system?

A

When the rate of the forwards reaction is equal to the rate of the reverse reaction

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5
Q

What can change depending on the reaction conditions?

A

The amount of product or reactants made

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6
Q

Why is it important to control reactions?

A

To make more of the product the you want

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7
Q

In equilibrium:

Whatever condition you apply…

A

The reaction does the opposite

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8
Q

In equilibrium:

If you increase temperature on the outside…

A

It will try to cool it on the inside
Therefore
The endothermic reaction takes place (takes heat in, cooling the surroundings)

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9
Q

In equilibrium:

If you decrease the temperature on the outside…

A

It will try to beat it on the inside
Therefore
The exothermic reaction will take place (gives heat out, heating the surroundings)

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10
Q

In equilibrium:

If you increase pressure on the outside…

A

It will move to the side with the least number of particles (big number)

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11
Q

In equilibrium:

If you decrease pressure on the outside…

A

It will move to the side with the most number of particles (big number)

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12
Q

What is the Haber process?

A

Used to make ammonia

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13
Q

What is ammonia used for?

A

Fertilisers

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14
Q

What is the equation for ammonia

A

N2 + 3H2 ⇌ 2NH3

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16
Q

What is used to make ammonia and how are they acquired?

A

Nitrogen and hydrogen

Nitrogen: from the air
Hydrogen: from fossil fuels

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17
Q

What conditions are used to make ammonia?

A

Iron catalyst
450 degrees
200 atmospheres

18
Q

What are the ideal conditions for maximum ammonia production?

A

Cold temperature

High pressure

19
Q

Why do they use not the ideal conditions to make ammonia?

A

A cold temperature affects rate of reaction making production slower

High pressure is expensive to generate and very dangerous

20
Q

What are the conditions called that they use to make ammonia? Why?

A

Compromise conditions

For a fast rate of reaction and a reasonable ammonia yield = 15%