Question

An electrochemical cell is set up at 25°C based on the overall reaction represented by the balanced equation shown below. The cell initially has [Cr³⁺] = [Cu²⁺] and E°_cell = +1.08 V.

$$3Cu2+(aq)+2Cr(s)3Cu(s)+2Cr3+(aq)

How many moles of electrons are transferred per reaction cycle (i.e., for 1 cycle of the equation as written)?

6

Part 3   (1 point)

Using the relationship given in part 1, calculate E_cell if [Cu²⁺] = 1.453 M and [Cr³⁺] = 0.00176 M, assuming that the temperature remains at 25°C. Give your answer to two places after the decimal.

(R = 8.314 J/mol·K and F = 9.65 × 10⁴ C/mol e^–)
     V   

1st attempt

Using the relationship given in part 1, calculate E_cell if [Cu²⁺] = 1.453 M and [Cr³⁺] = 0.00176 M, assuming that the temperature remains at 25°C. Give your answer to two places after the decimal.

(R = 8.314 J/mol·K and F = 9.65 × 10⁴ C/mol e^–)

Answer 1

I caq? Cut 2 + ge- Gorls) - - > Cee (si ] *3 Gest3 +3 é 7x2 3 cut 2 + 6e- 26rls) - - 3 Curso 260+3 +6e- 3 Cut 2 (aq) + 260(s) - Curs) +2 65 no of moles of é transfered = 6 moll Elue = +1.08 V

[us] = [ ] = 1.453 m 0.001–6 p _ no 0+ e Ecele = Eccele -0.0593 log@ Ecce = l-- -0538 og team Feue = 1008 - 0598 vlog cocina e Elect = 108 - .059 00176) 1.453) 3 Ecece = 1:139 V