Question

For which of the following le-chatelier’s principle is not applicable.\
$A){C_g}_{(s)} \rightleftharpoons {C_d}_{(s)}$
$B)PC{l_{5(g)}} \rightleftharpoons PC{l_{3(g)}} + C{l_{2(G)}}$
$C)RCOO{H_{(l)}} + R'O{H_{(l)}} \rightleftharpoons RCOOR{'_{(l)}} + {H_2}{O_{(l)}}$
$D)$ All of these

Answer 1

Le Chatelier's principle expresses that when a system encounters an unsettling influence, it will react to reestablish another balance state. For instance, if more reactants are added to a system, Le Chatelier's principle predicts that the response will create more products to balance the change and reestablish balance.

Complete step by step solution:
If we change the concentration of a compound will move the balance to the side that would counter that adjustment in fixation. The chemical system will endeavor to incompletely go against the change influenced to the first condition of equilibrium. Thus, the rate of response, degree, and yield of products will be modified relating to the effect on the system.
-The impact of changing the temperature in the balance can be clarified by joining heat as either a reactant or an product and, accepting that an increment in temperature expands the heat content of a system. At the point when the response is exothermic, heat is incorporated as a product, and when the response is endothermic, heat is incorporated as a reactant. Thus, regardless of whether expanding or decreasing the temperature would support the forward or the opposite response can be determined by applying a similar principle likewise with concentration changes.
Because Le-chatelier’s does apply to pure solids and liquids. During chemical equilibrium they experience no change in their concentration.
Correct option is $(A)$ .

Note:
Remember Le Chatelier's principle does apply to solids and fluids - what happens is that pure solids and fluids experience basically no change in concentration in chemical equilibrium.