Predict the shift in equilibrium position that will occur for each of the following reactions when the volume of the reaction container is increased.
a) 2cof2(g)⇌co2(g)+cf4(g).
i) to the left.
ii) to the right.
iii) does not shift.
b) 2no(g)+o2(g)⇌2no2(g).
i) to the left.
ii) to the right.
iii) does not shift.
c) 2n2o5(s)⇌4no2(g)+o2(g).
i) to the left.
ii) to the right.
iii) does not shift.
d) 2so2(g)+o2(g)⇌2so3(g).
i) to the left.
ii) to the right.
iii) does not shift.
e) pcl5(g)⇌pcl3(g)+cl2(g).
i) to the left.
ii) to the right.
iii) does not shift.

Explanation:

Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.

This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

Increase the volume:

If the volume of the container is increased, the pressure will decrease according to Boyle's Law. Now, according to the Le-Chatlier's principle, the equilibrium will shift in the direction where increase in pressure is taking place. So, the equilibrium will shift in a direction where more number gaseous moles are present.

A)

Number of gaseous moles on reactant side = 2

Number of gaseous moles on product side = 2

Equilibrium will not shift any direction as on both sides number of gaseous moles are same.

B)

Number of gaseous moles on reactant side = 3

Number of gaseous moles on product side = 2

Equilibrium will shift any left direction.

C)

Number of gaseous moles on reactant side = 2

Number of gaseous moles on product side = 5

Equilibrium will shift any right direction.

D)

Number of gaseous moles on reactant side = 3

Number of gaseous moles on product side = 2

Equilibrium will shift any left direction.

E)

Number of gaseous moles on reactant side = 1

Number of gaseous moles on product side = 2

Equilibrium will shift any right direction.

idk

explanation: