# Problem: The following half-reactions combine to make an electrolytic cell: K+ (aq) + e- → K (s)                                       E° = −2.93 Li+ (aq) + e- → Li (s)                                      E° = −3.05 If a current of 1.5 Amps is placed on this cell for 5 minutes, which of the following describes the mass of solid formed (in grams) and the voltage required of the current. [1 Amp = 1 coul/s;    96500 coul = 1 mol e-] A.  0.0324 g;  - 0.12 V             B. 0.000539 g ; - 0.12 V                      C. 0.00466 g;  0.12 V                    D. 0.0324 g;  5.98 V                           E.  0.00466 g;  5.98 V

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The following half-reactions combine to make an electrolytic cell:

K+ (aq) + e- → K (s)                                       E° = −2.93

Li+ (aq) + e- → Li (s)                                      E° = −3.05

If a current of 1.5 Amps is placed on this cell for 5 minutes, which of the following describes the mass of solid formed (in grams) and the voltage required of the current.

[1 Amp = 1 coul/s;    96500 coul = 1 mol e-]

A.  0.0324 g;  - 0.12 V

B. 0.000539 g ; - 0.12 V

C. 0.00466 g;  0.12 V

D. 0.0324 g;  5.98 V

E.  0.00466 g;  5.98 V

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Faraday's Constant concept. You can view video lessons to learn Faraday's Constant. Or if you need more Faraday's Constant practice, you can also practice Faraday's Constant practice problems.

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