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Edexcel A Level Chemistry: 10: Equilibrium I

Chemistry34 CardsCreated about 2 months ago

These flashcards cover the concept of dynamic equilibrium in reversible reactions, explaining how and when it is achieved, and emphasizing the importance of a closed system for maintaining equilibrium.

What can reversible reactions reach?

Dynamic euqillibrium

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Key Terms

Term
Definition

What can reversible reactions reach?

Dynamic euqillibrium

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

It slows down

When is dynamic equilibrium achieved?

When the forwards reaction is going at exactly the same rate as the backwards reaction and the amounts of reactants and products aren’t changing

What does dynamic equilibrium happen in?

A closed system

What is Kc?

The equilibrium constant

What does Kc give you an idea of?

How far to the left or right the equilibrium is

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TermDefinition

What can reversible reactions reach?

Dynamic euqillibrium

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

It slows down

When is dynamic equilibrium achieved?

When the forwards reaction is going at exactly the same rate as the backwards reaction and the amounts of reactants and products aren’t changing

What does dynamic equilibrium happen in?

A closed system

What is Kc?

The equilibrium constant

What does Kc give you an idea of?

How far to the left or right the equilibrium is


What is a homogeneous system?

A system in which everything is in the same physical state

What can Kc be worked out using?

The concentrations of reactants and products at equilibrium

Which reactants and products are included in Kc for homogeneous equilibria?

All of them

What is the equation for Kc?

[products]/[reactants]

What is a heterogeneous equilibria?

One in which not everything is in the same physical state

What is not included in the Kc expression for heterogeneous equilibria?

Pure liquids or solids

Why are solids not included in the Kc expression?

Because their concentration is constant

Why are pure liquids not included in the Kc expression?

Because their concentration is constant

Why aren’t catalysts included in the Kc expressions?

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

How do catalysts affect equilibrium?

They increase the rate at which equilibrium is reached

What is Le Chatelier’s principle?

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


If the position of equilibrium is altered, what will happen?

The amounts of products and reactants at equlibrium change


What happens if the concentration of a reactant is increased?

The equilibrium shifts to the right to use up the extra reactants

What happens if the concentration of a product is increased?

Equilibrium shifts to the left to remove the extra product


What happens if the pressure is increased?

The equilibrium shifts to the side with fewer moles, reducing the pressure


What does pressure affect?

Gases

What happens if pressure is decreased?

Equilibrium shifts to the side with the most moles to raise the pressure


What happens if temprature is increased?

The equilibrium shifts to the endothermic side to absorb the heat


What happens if temperature is decreased?


The equilibrium shifts to the exothermic side to replace the heat


What happens if the forward reaction is endothermic?

The reverse reaction is exothermic

How are conditions chosen in industry?

As a compromise

What are conditions chosen to produce?

A high rate and high yield

How is ethanol made?

From ethene and steam

What is the equation for ethanol production?

C2H4 + H2O --> C2H5OH

What pressure is used for ethanol production?

60-70 atm

What temperature is used for ethanol production?

300 degrees

What catalyst is used for ethanol production?

Phosphoric acid

Why is the temperature for ethanol production relatively low?

Because the forward reaction is exothermic, so lower temperatures favour it