For the exercise in this topic, base your answers on the potentials listed in Table 6M.1 or Appendix 2B, with the exception of the reduction and oxidation of water at pH = 7:

(a) How much time is required to electroplate 1.50 g of silver from a silver nitrate solution by using a current of 13.6 mA?

(b) If the same current is used for the same length of time, what mass of copper can be electroplated from a copper(II) sulfate solution?

Transcribed Image Text:

2 H₂O(1) + 2 e →H₂(g) + 2 OH¯ (aq), E = O₂(g) + 4H+ (aq) + 4e¯ 2 H₂O (1), E = -0.42 V at pH = 7 +0.82 V at pH = 7