Respuesta :
Answer: If a solute dissolves in an endothermic process the entropy of the solution must be greater than that of its pure components.
Explanation:
An endothermic process is defined as the process in which heat is absorbed by the reactant molecules taking part in a chemical reaction.
But in an endothermic process it is not possible to determine the type of bond present in the chemical atoms.
Also, we know that a spontaneous reaction between the solute and solvent leads to dissolution of solute particles. For such type of reactions, [tex]\Delta G < 0[/tex].
We know that,
[tex]\Delta G = \Delta H - T \Delta S[/tex] .......... (1)
For this, heat at constant pressure, [tex]\Delta H > 0[/tex] (for an endothermic process).
According to equation (1), more is the entropy of solution ([tex]\Delta S > 0[/tex]) more will be the negative value of [tex]\Delta G[/tex].
Thus, we can conclude that if a solute dissolves in an endothermic process the entropy of the solution must be greater than that of its pure components.
If a solute dissolves in an endothermic process: Choice B: the entropy of the solution must be greater than that of its pure components.
Discussion:
An endothermic process is characterized by the absorption of heat by the reactant molecules taking part in a chemical reaction.
But in an endothermic process it is not possible to determine the type of bond present in the chemical atoms.
The Gibb's free energy is related to the enthalpy and entropy as follows;
- Change in G = Change in H - T( Change in entropy)
A greater entropy change reduces the Gibb's free energy required for the reaction.
Ultimately, if a solute dissolves in an endothermic process, the entropy of the solution must be greater than that of its pure components.
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