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Question
For the reaction 2A(g)+B(g)⇌C(g), △H=+x kJ, Which of the following favour the formation of reactants?
For the reaction 2A(g)+B(g)⇌C(g), △H=+x kJ, Which of the following favour the formation of reactants?
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Solution
The correct option is A Low pressure
As per Le chatelier principle,
Backward reaction is exothermic as
C(g)⇌2A(g)+B(g) ΔH = - x kJ
So, As the temperature increases the reaction will favour the formation of products
Also the reaction is accompanied by increase in number of moles of gaseous species in backward reaction.
So, as the reaction pressure will increase the reaction will tend toward the direction where number of moles is less. Hence it is favoured by low pressure.
As per Le chatelier principle,
Backward reaction is exothermic as
C(g)⇌2A(g)+B(g) ΔH = - x kJ
So, As the temperature increases the reaction will favour the formation of products
Also the reaction is accompanied by increase in number of moles of gaseous species in backward reaction.
So, as the reaction pressure will increase the reaction will tend toward the direction where number of moles is less. Hence it is favoured by low pressure.
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