Ammonia gas is made by the reaction between nitrogen, N2\text{N}_2N2, and hydrogen, H2\text{H}_2H2.
The reaction reaches a dynamic equilibrium.
This is the equation for the reaction: N2(g)+3H2(g)⇌2NH3(g)\text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g)N2(g)+3H2(g)⇌2NH3(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.
The highest yield of ammonia is made using a very high pressure, such as 1000 atmospheres.
The reaction is actually carried out using a catalyst at a pressure of 200 atmospheres.
Suggest why a pressure of 200 atmospheres is used instead of 1000 atmospheres.
A factory uses 140 tonnes of nitrogen a day.
The factory produces 130 tonnes of ammonia per day as shown in the equation: N2(g)+3H2(g)⇌2NH3(g)\text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g)N2(g)+3H2(g)⇌2NH3(g)
Calculate the percentage yield of ammonia, NH3\text{NH}_3NH3.
Give your answer to 2 significant figures.
Relative atomic mass (ArA_rAr): H=1.0\text{H} = 1.0H=1.0 N=14.0\text{N} = 14.0N=14.0.