The exothermic formation of ClF3 is represented by the equation:
Cl2(g)+2F2(g)⇌2ClF3(g);ΔHr=−329kJ
Which of the following will increase the quantity of ClF3 in an equilibrium mixture of Cl2,F2 and ClF3?
The exothermic formation of ClF3 is represented by the equation:
The correct option is C Adding F2
For the given reaction Cl2(g)+2F2(g)⇌2ClF3(g), the enthalpy change of the
reaction is given as△Hr=−329kJ . We know that if the
enthalpy change is negative then the reaction is an exothermic reaction.
Therefore, according to Le Chatlier’s principle increasing the temperature will
shift the equilibrium towards the side of the reactants and hinder the
formation of the product.
Removing Cl2
will result in the decrease in the quantity of the product, since the equilibrium
of the reaction will move backward.
By increasing the volume of the container the value of Qc will become greater than the value
of Kc hence favoring the backward
reaction and resulting in the decrease of the quantity of the product.
So, for the given reaction if we want to increase the
quantity of the product ClF3 then
the correct option will be to add F2
so that the to decrease the concentration of F2
and to bring the system into equilibrium the reaction will move forward and
hence the quantity of the product ClF3
will increase.
Hence, the correct
option is C.) Adding F2
For the given reaction Cl2(g)+2F2(g)⇌2ClF3(g), the enthalpy change of the reaction is given as△Hr=−329kJ . We know that if the enthalpy change is negative then the reaction is an exothermic reaction. Therefore, according to Le Chatlier’s principle increasing the temperature will shift the equilibrium towards the side of the reactants and hinder the formation of the product.
Removing Cl2 will result in the decrease in the quantity of the product, since the equilibrium of the reaction will move backward.
By increasing the volume of the container the value of Qc will become greater than the value of Kc hence favoring the backward reaction and resulting in the decrease of the quantity of the product.
So, for the given reaction if we want to increase the quantity of the product ClF3 then the correct option will be to add F2 so that the to decrease the concentration of F2 and to bring the system into equilibrium the reaction will move forward and hence the quantity of the product ClF3 will increase.
Hence, the correct option is C.) Adding F2
