Faraday Calculation!

A current of 6.00 A is applied to the chromium(III) nitrate solution for 75.0 minutes. What mass of chromium is plated onto the part?

 

 

 

 

 

 

3) The voltaic cell described by the cell notation has an Eo of 0.68 V. Calculate the Wmax (kJ) the cell has done if 6.4700 mol of MnO4-(aq) (Molar Mass - 118.94 g/mol) reacts. Round your answer to 3 significant figures.

Pt(s) l VO2+(aq), VO2+(aq), H+(aq) ll H+(aq), MnO4-(aq) l MnO2(s) l Pt(s)

St. Red. Pot. (V)

VO2+/VO2+: +1.00

MnO4-/MnO2 :+1.68

Faraday's Constant

F = 96485 C

4) The galvanic cell described by the cell notation has an Eo of 1.23 V. Calculate the value (kJ) for the ΔG˚ of the cell. Round your answer to 3 significant figures.

Pt(s), H2(g) l H2O(l), OH-(aq) ll O2(g) l OH-(aq) l Pt(s)

St. Red. Pot. (V)

H2O/H2: -0.83

O2/OH- : +0.40

Faraday's Constant

F = 96485 C

5) The electrochemical cell described by the balanced chemical equation has a standard cell potential of -0.37 V. Calculate the value (kJ) for the standard free energy change of the cell. Round your answer to 3 significant figures.

Sn4+(aq) + 2Cu(s) → Sn2+(aq) + 2Cu+(aq)

St. Red. Pot. (V)

Cu+/Cu: +0.52

Sn4+/Sn2+: +0.15

Faraday's Constant

F = 96485 C

6)The electrochemical cell described by the cell notation has an Eocell of 4.05 V. Calculate the maximum electrical work (kJ) the cell has done if 375.44 g of F2(g) (Molar Mass - 38.00 g/mol) reacts. Round your answer to 3 significant figures.

Mn(s) l Mn2+(aq) ll F2(g) l F-(aq) l Pt(s)

St. Red. Pot. (V)

Mn2+/Mn: -1.18

F2/F- : +2.87

Faraday's Constant

F = 96485 C

Which statement about the Faraday is False?
1. one Faraday = quantity of electricity required to reduce oneequivalent weight of a substance at the cathode
2. one Faraday = 96487 amperes x s
3. one Faraday = quantity of electricity required to reduce oneformula weight of a substance
4. one Faraday = 96487 Coulombs
5. one Faraday = 6.02 x 10^23