Industrial reaction conditions for the production of ammonia is as shown below in the graph: What temperature achieves the highest yield of ammonia?

The production of ammonia by Haber's process is an exothermic process, where energy is released as heat into the surroundings during the reaction. The reverse reaction, which produces hydrogen and nitrogen gas, is therefore endothermic, and takes in energy from the surroundings. Therefore, a temperature of 200 ° C , achieves the highest yield of ammonia according to the graph given.

Industrial reaction conditions for the production of ammonia is as shown below in the graph: Describe how the yield changes as the pressure is increased.

In the manufacture of ammonia by Haber's process, for all temperatures, as the pressure increases the yield of ammonia increases. This can be shown by the graph as given below:

Industrial reaction conditions for the production of ammonia is as shown below in the graph: A pressure of 200 atm is used during the process. Why does industry not use a much higher pressure to maximise yield?

A pressure of 200 atm is used is used during the process of manufacture of ammonia by Haber's process.The cost of building and maintaining equipment capable of withstanding high pressures during the manufacture of ammonia is expensive; improved safety practices must be employed when dealing with equipment at high pressure. Therefore, the industry does not use a much higher pressure to maximise the yield.

Industrial reaction conditions for the production of ammonia is as shown below in the graph: Explain with reference to the position of the equilibrium why increasing the pressure of this closed system favours the forward reaction.

In the manufacture of ammonia by Haber's process, the equilibrium reaction involves four moles of reactants and two moles of products; and an increase in pressure favours the side of the equilibrium with the smaller number of moles of gas in accordance with Le Chatelier's principle. Therefore, the forward reaction is favoured as the pressure is increased. N 2 g + 3 H 2 g ⇌ 2 NH 3 g

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MYP:4-5

IMPORTANT

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How does the total amount of energy contained in the reactants compare to the products in Haber's process for the manufacture of ammonia? Which substances will be more energetically stable, reactants or products?

Important Questions on Balance

EASY

MYP:4-5

IMPORTANT

MYP Chemistry A concept-based approach Years 4&5>Chapter 1 - Balance>Research>Q 1

What is the source of the reactants, nitrogen and hydrogen, used in the Haber's process?

EASY

MYP:4-5

IMPORTANT

MYP Chemistry A concept-based approach Years 4&5>Chapter 1 - Balance>Research>Q 2

Write a balanced chemical equation for the production of hydrogen gas.

MEDIUM

MYP:4-5

IMPORTANT

MYP Chemistry A concept-based approach Years 4&5>Chapter 1 - Balance>Uses of nitrogen-containing chemicals>Q 1

Gather information from a variety of sources about the main uses of the chemicals nitric acid,

{HNO}_{3}

, ammonium nitrate,

{NH}_{4} {NO}_{3}

, ammonium sulphate,

{({NH}_{4})}_{2} {SO}_{4}

and urea,

{NH}_{2} {CONH}_{2}

. Structure the information as a summary and present it. Based on your research, share ideas with your peers, while answering the following question: Why must the total amount of ammonia production keep increasing each year?

EASY

MYP:4-5

IMPORTANT

MYP Chemistry A concept-based approach Years 4&5>Chapter 1 - Balance>Data-based question: Industrial reaction conditions for the production of ammonia>Q 1

Industrial reaction conditions for the production of ammonia is as shown below in the graph:

Question Image

What temperature achieves the highest yield of ammonia?

EASY

MYP:4-5

IMPORTANT

MYP Chemistry A concept-based approach Years 4&5>Chapter 1 - Balance>Data-based question: Industrial reaction conditions for the production of ammonia>Q 2

Industrial reaction conditions for the production of ammonia is as shown below in the graph:

Question Image

Describe how the yield changes as the pressure is increased.

EASY

MYP:4-5

IMPORTANT

MYP Chemistry A concept-based approach Years 4&5>Chapter 1 - Balance>Data-based question: Industrial reaction conditions for the production of ammonia>Q 3

Industrial reaction conditions for the production of ammonia is as shown below in the graph:

Question Image

The ideal temperature used by Haber is approximately $450^{°} C$ . Outline the reasons why a higher temperature would be used to increase production of ammonia instead of a lower temperature.

EASY

MYP:4-5

IMPORTANT

MYP Chemistry A concept-based approach Years 4&5>Chapter 1 - Balance>Data-based question: Industrial reaction conditions for the production of ammonia>Q 4

Industrial reaction conditions for the production of ammonia is as shown below in the graph:

Question Image

A pressure of $200 atm$ is used during the process. Why does industry not use a much higher pressure to maximise yield?

EASY

MYP:4-5

IMPORTANT

MYP Chemistry A concept-based approach Years 4&5>Chapter 1 - Balance>Data-based question: Industrial reaction conditions for the production of ammonia>Q 5

Industrial reaction conditions for the production of ammonia is as shown below in the graph:

Question Image

Explain with reference to the position of the equilibrium why increasing the pressure of this closed system favours the forward reaction.

How does the total amount of energy contained in the reactants compare to the products in Haber's process for the manufacture of ammonia? Which substances will be more energetically stable, reactants or products?

Important Questions on Balance

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