Ammonia is formed in the Haber process according to the following balanced equation - Leaving Cert Chemistry - Question 11(a) - 2009
Question 11(a)
Ammonia is formed in the Haber process according to the following balanced equation.
$$3H_2(g) + N_2(g) \rightleftharpoons 2NH_3(g)$$
The table shows the percentag... show full transcript
Worked Solution & Example Answer:Ammonia is formed in the Haber process according to the following balanced equation - Leaving Cert Chemistry - Question 11(a) - 2009
Step 1
Find from the table the conditions of temperature and pressure at which the highest yield of ammonia is obtained.
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Answer
From the table, the highest percentage of ammonia is found at a temperature of 573 K and a pressure of 1000 atm, yielding 92% ammonia.
Step 2
Deduce from the data whether this reaction is exothermic or endothermic. Explain your reasoning.
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Answer
The forward reaction is determined to be exothermic. This can be inferred from the data, as lower temperatures yield higher amounts of NH₃, indicating that a decrease in temperature shifts the equilibrium to favor the production of ammonia, consistent with Le Chatelier's principle.
Step 3
Identify one industrial problem associated with the use of high pressures.
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High pressures in industrial settings can lead to significant costs in building maintenance and safety measures, as well as risks of leaks or explosions.
Step 4
Write an equilibrium constant (K_c) expression for this reaction.
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Answer
The equilibrium constant expression for the reaction is given by:
Kc=[H2]3[N2][NH3]2
where the concentration of species is expressed in moles per liter and square brackets indicate concentration.
Step 5
State the effect on the value of K_c of using a catalyst. Justify your answer.
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Answer
The use of a catalyst has no effect on the value of K_c. While a catalyst increases the rate at which equilibrium is reached, it does not change the position of the equilibrium or the ratio of products to reactants at equilibrium.
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