Respuesta :
Answer: Option (b) is the correct answer.
Explanation:
According to Le Chatelier's principle, any disturbance caused in an equilibrium reaction will tend to shift the equilibrium in a direction away from the disturbance.
For example, [tex]CaCO_{3}(s) + CO_{2}(aq) + H_{2}O(l) \rightleftharpoons Ca^{2+}(aq) + 2HCO^{-}_{3}(aq)[/tex]
Hence, expression for equilibrium constant will be as follows.
[tex]K_{eq} = \frac{[Ca^{2+}][HCO^{-}_{3}]^{2}}{[CO_{2}][H_{2}O]}[/tex]
Since, the concentration for a solid substance is considered as 1 or unity. Therefore, adding or removing a solid will not affect the equilibrium.
Thus, we can conclude that according to Le Châtelier’s Principle, the amount of solid reactant or product present does not have an impact on the equilibrium because the solid does not appear in the equilibrium constant, so adding or removing solid has no effect.
When there is a disturbance in reaction then the equilibrium shifts. The solid does not occur in the state of equilibrium, so addition or removal has no effect.
What is Le's principle?
According to the principle, the change in the equilibrium of the reaction due to varying the conditions will result in the shift of the equilibrium constant to balance the change made in the reaction.
The equilibrium shifts in the direction of the reaction that removes and balances the stress or the altered conditions.
The solid substances of the reaction have a concentration of 1 and their addition or removal in the reaction does not affect the equilibrium shift.
Therefore, option B. addition or removal of the solid does not have any impact on the equilibrium.
Learn more about equilibrium shift here:
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