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(a)
Interpretation: The effect of increasing pressure by injecting oxygen (reactant) on the equilibrium needs to be explained.
Concept introduction: According to Le Chatelier's principle if any stress is given to the equilibrium, it will shift in a direction to reduce the given stress. If change in concentration, pressure or temperature takes place at equilibrium, it will shift in the direction to undo the change or its effect.
(a)
Answer to Problem 33A
The reaction will move in the backward direction.
Explanation of Solution
According to Le Chatelier’s principle, if the pressure is increased, the direction of equilibrium will shift so as to reduce the pressure. Pressure is created when gas molecules collides with the sides of their container. The more the number of molecules in the container, the more will be the pressure. The system can decrease the pressure by reacting in such a way as to generate fewer molecules.
The concerned reaction: 4NH3(g)+5O2(g)⇌4NO(g)+6H2O(g)
In this reaction change in the number of moles Δn=(4+6)−(4+5)=+1
So, here in the backward reaction moles of gas decreases. If pressure is increased reaction shifts in backward direction.
(b)
Interpretation: The effect of addition of desiccant in the system needs to be explained.
Concept introduction: According to Le Chatelier's principle if any stress is given to the equilibrium, it will shift in a direction to reduce the given stress. If change in concentration, pressure or temperature takes place at equilibrium, it will shift in the direction to undo the change or its effect.
(b)
Answer to Problem 33A
The reaction equilibrium will shift towards right.
Explanation of Solution
The concerned reaction: 4NH3(g)+5O2(g)⇌4NO(g)+6H2O(g)
Equilibrium constant for the reaction is given by the equation, K=[NO]4[H2O]6[NH3]4[O2]5
When H2O (product) is absorbed then the value of K will decrease as the concentration of H2O is in nominator. To maintain the value of K concentration of the products ( NH3 and O2 ) will decrease. Hence, the reaction will shift towards right.
(c)
Interpretation: The effect on equilibrium when the system is compressed and ammonia liquefies needs to be explained.
Concept introduction: According to Le Chatelier's principle if any stress is given to the equilibrium, it will shift in a direction to reduce the given stress. If change in concentration, pressure or temperature takes place at equilibrium, it will shift in the direction to undo the change or its effect.
(c)
Answer to Problem 33A
The reaction will move in the backward direction.
Explanation of Solution
The concerned reaction: 4NH3(g)+5O2(g)⇌4NO(g)+6H2O(g)
Equilibrium constant for the reaction is given by the equation, K=[NO]4[H2O]6[NH3]4[O2]5
When the system is compressed pressure increases. According to Le Chatelier’s principle, if the pressure is increased, the direction of equilibrium will shift so as to reduce the pressure. Pressure is created when gas molecules collides with the sides of their container. The more the number of molecules in the container, the more will be the pressure. The system can decrease the pressure by reacting in such a way as to generate fewer molecules.
And also when NH3 is started to get liquefy concentration of the gaseous NH3 decreases. To maintain the value of K reaction equilibrium shifts to backward direction to increase the amount of reactants.
Chapter 17 Solutions
World of Chemistry, 3rd edition
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