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.
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Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.27QP: Hypothetical elements A2 and B2 react according to the following equation, forming the compound AB....
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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
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
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Transcribed Image Text: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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