(A). System will towards the products.
When H₂O is removed, the concentration of products will be low. Then the equilibrium of the system will be broken. Hence, according to the Le
Chatelier's principle, system will try to
become equilibrium by enhancing the forward
reaction.
(B).
System will shift towards the products.
Addition
of O₂ will increase the
concentration of reactants. Then to maintain the
equilibrium the O₂ should be decreased. To do that the system will shift
towards the products. When products are increased, the consuming of O₂ will be high.
(C). System
will shift towards the reactants.
When pressure is decreased, according to the Le Chatelier's principle, system
will try to increase the pressure to maintain the equilibrium. There are 2 moles of H₂ and 1 mole of O₂ as reactants. Hence, altogether there are 3 moles of molecules
as reactants but 2 moles of molecules as products. When the number of moles of molecules is high,
then the pressure is high. Hence, to increase the pressure, system will shift
towards the reactants.
(D). System
will shift towards the reactants.
The given reaction is an exothermic reaction since it produces heat. When the temperature is high, system
will try to lower the temperature. Since forward reaction is exothermic, the backward
reaction is endothermic. When there is increase
in temperature, system will shift towards the
reactants because endothermic
reactions decrease the temperature.
