Answer:
a) Increase
b) the amount of SiCl₄ will decrease.
c) K will increases.
d) H₂O will increase.
e) SiCl₄ will decrease
f) HCl will decrease.
g) SiO₂ will decrease
Explanation:
The equilibrium changes are explained by Le-Chatelier's Principle.
If we apply a change to an equilibrium system then it shifts to the side where the effect of stress can be released.
a) Change : Increase in pressure
Quantity : amount of water
Change: We are increasing the pressure it will decrease the volume and hence will increase the moles per unit volume. so the system will move in the direction where the number of gaseous moles are less. It will move towards reactant side. thus the amount of water will increase.
b) Change : decrease in temperature
Quantity : amount of SiCl₄
As this is an exothermic reaction, the decrease in temperature will shift the reaction towards product side and hence the amount of SiCl₄ will decrease.
c)
Change : Increase in Temperature
Quantity: Kc
The equilibrium constant will increase as it increases with temperature.
d) Change : increase in temperature
Quantity : amount of H₂O
As this is an exothermic reaction, the increase in temperature will shift the reaction towards reactant side and hence the amount of H₂O will increase.
e) Change : Add H₂O
Quantity: Amount of SiCl₄
As we are adding reactant to the equilibrium, the equilibrium will shift towards product side thus the amount of SiCl₄ will decrease
f) Change : Add SiO₂
Quantity: Amount of HCl
As we are adding product, the equilibrium will shift in reactant side and thus there will be decrease in amount of HCl.
g) Change : Add HCl
Quantity: Amount of SiO₂
As we are adding product to the equilibrium the equilibrium will shift in reactant side and thus there will be decrease in amount of SiO₂
