Electrochemistry (Part 2)

In the Nernst Equation, at standard temperature condition, what is the value of [(R)(T)]/F? (Indicate the Unit with 3 sig figs)

Using the Nernst Equation, calculate for the cell potential at standard temperature;

2Ag⁺(aq) [0.50 M] + Ni (s) ---> 2Ag (s) + Ni²⁺(aq) [0.20 M]

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Ni (s) ---> Ni²⁺(aq) [0.20 M] +2e^- = E^o_red = -0.25 V

Ag⁺(aq) [0.50 M] + e^- ---> Ag (s) = E^o_red = +0.799 V

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Answer with 4 sig figs, Values and UNIT

Cell potentials should be _______________, for the reaction to be spontaneous. (Answer in all CAPS)

Delta Gibbs Free Energy should be _______________, for the reaction to be spontaneous. (Answer in all CAPS)

Calculate for the Gibbs free energy, answer in kJ.

Type of galvanic cell, that is made of electrochemical cells that cannot be reversed.

• Primary Cells

• Secondary Cells

• Voltaic Cells

Type of galvanic cell, that is made of electrochemical cells that can be reversed.

• Primary Cells

• Secondary Cells

• Voltaic Cells

It is a process of depositing thin coat metal on other metal by using electrolysis. (Answer in All Caps)

In a copper plating experiment in which copper metal is deposited from copper (II) ion solution, the system is run for 2.600 hours at a current of 12.00 A. What mass of copper is deposited?

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NOTE: Use Farad Constant Value 96, 485 C

(Answer with "g Cu" as a UNIT, 4 sig figs)

If a current of 15.0 A is run through electrolysis cell for 2.00 hours, how many moles of electrons have moved? (Answer with "moles of e" as a UNIT, 3 sig figs)