Calculate the Ecell value at 298K for the cell based on the reaction Fe3+(aq)+ Cr2+(aq) --> Fe2+(aq)+Cr3+(aq) when [Fe3+] = [Cr2+] = 1.50x10-3 M and [Fe2+]= [Cr3+] = 2.5x10-4 M?

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13 Dec 2019

Calculate the Ecell value at 298K for the cell based on the reaction

Fe³⁺(aq)+ Cr²⁺(aq) --> Fe²⁺(aq)+Cr³⁺(aq)

when [Fe³⁺] = [Cr²⁺] = 1.50x10^-3 M and [Fe²⁺]= [Cr³⁺] = 2.5x10^-4 M?

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The equilibrium constant for the reaction below is Kc = 9.1multiplied by 10-6 at 298 K.

2 Fe3+(aq) + Hg22+(aq) reverse reaction arrow 2 Fe2+(aq) + 2Hg2+(aq)

(a) Calculate ?G when [Fe3+] = 0.20 M, [Hg22+] = 0.016 M, [Fe2+] =0.024 M, and [Hg2+] = 0.030 M.

amberelephant556

The equilibrium constant for the reaction,

2 Fe³⁺(aq) + Hg₂²⁺(aq)<=>2 Fe²⁺(aq) +2Hg²⁺(aq)
is 9.1 x 10^-6(aq) at 298 K. Calculate ÎG inkJ when

[Fe³⁺(aq)] = 0.807
[Hg₂²⁺(aq)] = 0.0130
[Fe²⁺(aq)] = 0.0644
[Hg²⁺(aq)] = 0.0165

PLEASE EXPLAIN WHY .

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Calculate the Ecell value at 298K for the cell based on the reaction

Fe³⁺(aq)+ Cr²⁺(aq) --> Fe²⁺(aq)+Cr³⁺(aq)

when [Fe³⁺] = [Cr²⁺] = 1.50x10^-3 M and [Fe²⁺]= [Cr³⁺] = 2.5x10^-4 M?

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