How will the following reaction equilibrium be affected if the volume of each reaction system is increased at constant temperature?
(1) `2SO_(2)(g)+O_(2)(g)hArr 2SO_(3)(g)`
(2) `C(s)+(1)/(2)O_(2)(g)hArr CO(g)`

Explanation

At constant temperature, if the volume of the reaction systemm be increased, then the total pressure at equilibrium will be decreased. Thus, the equilibrium of the system will be disturbed. According to Le chatelier's principle, equilibrium will be shifted in a direction that results in increase in the total number of molecules.
(1) In case of the first reaction, the equilibrium will shift to the left side. as a result, the yield of the product, `[SO_(3)(g)]` will decrease.
(2) On the other hand, in case of the second reaction, the equilibrium will shift to the right side and thereby increasing the yield of the product `[CO(g)]`.