Part 2 The Haber process produces ammonia (NH3) for the chemical industry from nitrogen (N₂) and hydrogen (H₂) as shown in the chemical equation below. This is a reversible reaction. N2 (8) + 3H2 (8) 2NH3 (8) AH = -92 kJ mol-¹ (exothermic) The following questions relate to the effect of changing factors that influence the direction of the above reaction, according to Le Chatelier's principle. For each change in factor (i - iv) listed in the Table, you need to: state the direction of equilibrium, give a reason for your choice, identify if the amount of ammonia produced will increase or decrease. Factor i) ii) Increase in pressure iii) Increase in Decrease in concentration of N₂ temperature iv) A catalyst is added Direction (shift) of equilibrium Scientific explanation for stated direction of equilibrium. Amount of NH3 Increases / decreases Part 3 During this reaction, compromises are made to speed up and maximise the production of ammonia. i) ii) Suggest why a moderate amount of pressure of around 200 atmospheres is used. Suggest why a moderate temperature of around 400°C is used.

Part 2 The Haber process produces ammonia (NH3) for the chemical industry from nitrogen (N₂) and hydrogen (H₂) as shown in the chemical equation below. This is a reversible reaction. N2 (8) + 3H2 (8) 2NH3 (8) AH = -92 kJ mol-¹ (exothermic) The following questions relate to the effect of changing factors that influence the direction of the above reaction, according to Le Chatelier's principle. For each change in factor (i - iv) listed in the Table, you need to: state the direction of equilibrium, give a reason for your choice, identify if the amount of ammonia produced will increase or decrease. Factor i) ii) Increase in pressure iii) Increase in Decrease in concentration of N₂ temperature iv) A catalyst is added Direction (shift) of equilibrium Scientific explanation for stated direction of equilibrium. Amount of NH3 Increases / decreases Part 3 During this reaction, compromises are made to speed up and maximise the production of ammonia. i) ii) Suggest why a moderate amount of pressure of around 200 atmospheres is used. Suggest why a moderate temperature of around 400°C is used.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.

Exergonic Reaction

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Question

Part 2 The Haber process produces ammonia (NH3) for the chemical
industry from nitrogen (N₂) and hydrogen (H₂) as shown in the chemical
equation below. This is a reversible reaction.
N2 (8) + 3H2(g) → 2NH3 (8) AH = -92 kJ mol-¹ (exothermic)
The following questions relate to the effect of changing factors that
influence the direction of the above reaction, according to Le Chatelier's
principle.
For each change in factor (i - iv) listed in the Table, you need to:
state the direction of equilibrium,
give a reason for your choice,
identify if the amount of ammonia produced will increase or
decrease.
Factor
Decrease in
concentration of N₂
i)
ii)
Increase in
pressure
iii) Increase in
temperature
iv) A catalyst is added
Direction
(shift) of
equilibrium
Scientific
explanation for
stated direction of
equilibrium.
Amount of
NH3
Increases /
decreases
Part 3 During this reaction, compromises are made to speed up and
maximise the production of ammonia.
i)
ii)
Suggest why a moderate amount of pressure of around 200
atmospheres is used.
Suggest why a moderate temperature of around 400°C is
used.

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