refers to the relative concentrations of reactants and products in a reversible reaction at equilibrium.

occurs in a closed system when the forward and reverse reactions of a reversible chemical reaction are occurring at the same rate; and the concentrations of reactants and products remain constant.

is the speed with which a chemical reaction takes place, measured by the amount of a reactant used or amount of product formed in a given time.

an industrial method for producing ammonia.

an industrial method for producing sulfuric acid.

Equilibrium: balance between rate, safety, environment and economics

Chemistry

In the Rates and energy changes unit, pupils learned about how energy changes are always involved in reaction, along with a range of methods for measuring and comparing rates of reaction using properties of reactants and/or products.

Industrial chemistry

At equilibrium, the relative concentrations of reactants and products.

Forward and reverse reactions occur at the same rate.

Speed at which a chemical reaction takes place.

Industrial method for producing sulfuric acid.

Match the following terms with the correct definitions.

Which of the following factors does **not** affect the position of equilibrium?

What impact would increasing the pressure have on this reversible reaction?
3H₂ (g) + N₂ (g) ⇌ 2NH₃ (g)

A high temperature would increase the rate of the reaction.

A high temperature would increase the yield.

A high temperature would decrease the yield.

A high temperature would decrease the rate of reaction.

A reversible reaction is exothermic in the forward reaction. Which of the following statements about the reaction are correct?

It decreases the concentration of the desired product (in the reaction mixture).

It shifts the equilibrium position towards the desired product.

It decreases the yield of the desired product.

During a reversible reaction the desired product is removed, the pressure and temperature are kept constant. What impact does this have on the reaction?

Increasing the pressure would decrease the rate of reaction.

Increasing the pressure would increase the cost.

Increasing the pressure would increase the equipment failure risk.

Increasing the pressure would decrease the yield.

Why is ammonia manufactured at 200 atmospheres rather than the higher 400 atmospheres?
3H₂ (g) + N₂ (g) ⇌ 2NH₃ (g)

The industrial method for producing ammonia from hydrogen and nitrogen is called the {{}}.

What name is given to a substance that increases the rate of a reaction, by providing an alternative reaction pathway?

Which of the following chemical reactions are exothermic?

In an equation for a chemical reaction, what is the meaning of this symbol ⇌?

Which of the following factors does **not** increase the rate of this chemical reaction?
NaOH (aq) + HCl (aq) → H₂O (l) + NaCl (aq)

What is normally used as a catalyst in the Haber process?

This lesson will soon be taken down.

Equilibrium: balance between rate, safety, environment and economics

Lesson outcome