Sulfur trioxide, SO3\text{SO}_3SO3, is manufactured by the reversible reaction between sulfur dioxide, SO2\text{SO}_2SO2, and oxygen, O2\text{O}_2O2.
The reaction reaches a dynamic equilibrium.
This is the equation for the reaction: 2SO2(g)+O2(g)⇌2SO3(g)2\text{SO}_2(g) + \text{O}_2(g) \rightleftharpoons 2\text{SO}_3(g)2SO2(g)+O2(g)⇌2SO3(g)
State what is meant by a dynamic equilibrium.
The position of equilibrium moves if the reaction conditions are changed.
The forward reaction is exothermic.
The temperature of the equilibrium mixture is increased.
State and explain what happens to the position of the equilibrium.
Although a higher yield of sulfur trioxide could be obtained at a higher pressure such as 50 atmospheres, the reaction is commercially carried out at a much lower pressure of about 2 atmospheres.
Suggest why a pressure of 2 atmospheres is used instead of 50 atmospheres.
A chemical plant uses 240 tonnes of sulfur dioxide per day.
The plant produces 250 tonnes of sulfur trioxide per day according to the equation: 2SO2(g)+O2(g)⇌2SO3(g)2\text{SO}_2(g) + \text{O}_2(g) \rightleftharpoons 2\text{SO}_3(g)2SO2(g)+O2(g)⇌2SO3(g)
Calculate the percentage yield of sulfur trioxide, SO3\text{SO}_3SO3.
Give your answer to 2 significant figures.
Relative atomic masses (ArA_rAr): O=16.0\text{O} = 16.0O=16.0, S=32.0\text{S} = 32.0S=32.0.