A certain salt has a negative Enthalpy of Solution (i.e. Delta H_soln = -), and

Question

A certain salt has a negative Enthalpy of Solution (i.e. Delta H_soln = -), and a positive Entropy of Solution (Delta S_so ln = +). Upon increasing the temperature of the water solvent, you would expect: The solubility of the salt to increase The solubility of the salt to decrease The solubility to remain unchanged, as Delta H_soln & Delta S_soln have opposite signs The effect on the solubility cannot be determined Which of the following is the correct cell diagram for the reaction: 2 Fe^2+(aq) + Cl_2 (g) rightarrow 2 Fe^3+(aq) + 2 Cl^-(aq) Fe^3+ (1.0M) | Fe^2+(1.0M) || Cl_2(g) | Cl^-(I.0M) Fe(s) | Fe^3+ (1.0M), Fe^2+(1.0M) || Cl_2(g) | Cl^- (1.0M) | Pt(s) Pt(s), Fe^3+ (1.0M), Fe^2+(1.0M) || Cl_2(g). Cl^-(1.0M) | Pt(s) Fe(s) | Fe^3+(1.0M) | Fe^2+ (1.0M) || Cl_2(g) | Cl^-(1.0M) | Pt(s) Pt(s) | Fe^3+ (1-0M), Fe^2+(1.0M) || Cl_2(g) | Cl^-(1.0M) | Pt(s)

Explanation / Answer

As H is negative and entropy is positive, with temperature to be high, the free energy term becomes more negative and hence the solubility of salt increases.

7)The answer will be 5th option.Anode at left and cathode at right. We can't use iron electrode since it will also take part in the reaction. Phases are separated by slash and half cell by double slash

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