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Ammonia is prepared industrially from hydrogen and nitrogen in the presence of a suitable catalyst according to the equation $$N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$$ The graph below shows the variation of the equilibrium yield of ammonia with pressure at different temperatures - VCE - SSCE Chemistry - Question 4 - 2002 - Paper 1
Question 4
Ammonia is prepared industrially from hydrogen and nitrogen in the presence of a suitable catalyst according to the equation $$N_2(g) + 3H_2(g) \rightleftharpoons 2... show full transcript
Worked Solution & Example Answer:Ammonia is prepared industrially from hydrogen and nitrogen in the presence of a suitable catalyst according to the equation $$N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$$ The graph below shows the variation of the equilibrium yield of ammonia with pressure at different temperatures - VCE - SSCE Chemistry - Question 4 - 2002 - Paper 1
Step 1
a. A particular industrial plant uses a pressure of 300 atm and a temperature of 500°C. From the graph, determine the percentage yield of ammonia under these conditions.
Answer
To determine the percentage yield of ammonia at a pressure of 300 atm and a temperature of 500°C, locate the point on the graph where the pressure is 300 atm. Then, trace upwards to find the corresponding curve for 500°C. The intersection point will indicate the percentage conversion to ammonia. Based on examination of the graph, the yield at these conditions is approximately 24%.
Step 2
b. State Le Chatelier's principle.
Answer
Le Chatelier's principle states that a system at equilibrium will shift so as to minimise the effects of any change in external conditions imposed on it. This means that if a change occurs (like changes in concentration, pressure, or temperature), the equilibrium will adjust to counteract that change and restore a new equilibrium.