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In the study of d and f Block Elements, a reaction at standard temperature follows the relationship $\Delta G = \Delta H - T\Delta S$. What happens to the system if the concentration of reactants is doubled?
A
The rate constant doubles.
B
The equilibrium shifts to the right, favoring products.
C
The Gibbs free energy $\Delta G$ becomes zero.
D
The activation energy $E_a$ is halved.
Explanation
According to Le Chatelier's principle and equations like $\Delta G = \Delta H - T\Delta S$ in d and f Block Elements, increasing reactant concentration favors product formation.
Detailed Solution
In d and f Block Elements, the reaction quotient $Q$ decreases when reactant concentration increases. Based on $\Delta G = \Delta H - T\Delta S$, the system drives forward to restore equilibrium.