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11 Dec 2019

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12. A voltaic cell utilizes the following redoxreaction:

Cr(s) + 2Fe³⁺(aq) Â® 2Fe²⁺(aq) +Cr²⁺(aq)

a. Identify the oxidizing agent in the reaction.

b. How many electrons are transferred in the redox reaction

c. Calculate the standard cell potential, EÂ°_cell and DG forthis electrochemical cell.

d. Calculate the equilibrium constant for the redox reaction.

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Jarrod RobelLv2

13 Dec 2019

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Answer the following questions

H3AsO3(aq) --> As(s) + O2(g) (acidic and 25Â°C)

a. Balance the following redox reaction.

b. Calculate the EÂ° cell. (Use EÂ° cell = EÂ° red + EÂ° ox)

c. Would this reaction occur in an electrolytic cell or a voltaic cell?

d. Calculate the ï²GÂ° rxn. (Use ï²GÂ° rxn = -nF EÂ° cell) e. Calculate the equilibrium constant. (Use ï²GÂ° rxn = âRT lnK) Given the EÂ°red of the arsenic reaction is -0.58V and the acidic reduction value for O2 is +1.23V.

Part A and B please

A) Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25Â°C. (The equation is balanced.)
2F₂(g) + Mn(s) â 4 F^-(aq) + Mn²⁺(aq)

F₂(g) + e^- â 2 F^-(aq)	EÂ° = +2.87 V
Mn²⁺(aq) + 2 e^- â Mn(s)	EÂ° = -1.18 V

e)1.69 V

B) Balance the following redox reaction if it occurs in H₂SO₄. What are the coefficients in front of H₂O and Cr₂(SO₄)₃ in the balanced reaction?

C₃H₈O₂(aq) + K₂Cr₂O₇(aq) â C₃H₄O₄(aq) + Cr₂(SO₄)₃(aq)

a) H₂O = 22, Cr₂(SO₄)₃ = 4

b) H₂O = 5, Cr₂(SO₄)₃ = 2

c) H₂O = 8, Cr₂(SO₄)₃ = 2

d) H₂O = 11, Cr₂(SO₄)₃ = 4

e) H₂O = 1, Cr₂(SO₄)₃ = 5

Given the folloiwng two half-reactions:

Fe3+ (aq) + 3 eâ --> Fe (s) E0 = â0.036 V

Mg2+(aq) + 2 eâ --> Mg (s) E0 = â2.37 V

Calculate cell potential (Ecell) for a voltaic cell when [Fe3+] = 1.0 *10-3 M, [Mg2+] = 2.50 M at 25 oC

Hint: (1) Write the overall redox reaction and count the number of electrons transferred; (2) determine the cell potential for a voltaic cell; (3) Calculate Q; (4) Plug in the values into Nernst equation.