Farady's law

By electrolysis of water, 11.2L of oxygen at STP was prepared. A) what charge was required? B) If a current of 0.5A was used, how long did it take? Note: please explain step by step how to get each answer.

Problem Set

I would like help with the attached assignment except for question #4,#5,#6.

Electrochemistry

1 a) A copper refining cell is operating with an electrolyte which contains 0.05 m Sn2+. At what concentration of Cu2+ will the tin start to plate out in preference to the copper? The cell temperature is 40°C. b) A polarization potential arises from a concentration difference between ions in the neighborhood of the electrode and those in the bulk of the electrolyte solution. Calculate the polarization potential in a copper electrorefining cell given the following information. Cell temperature: 40°C Cu2+ concentration in the bulk of the solution: 1.0 m Cu2+ concentration adjacent to the anode: 5.0 m Cu2+ concent... click for more

Electrochemistry

2 The following table gives some results from experiments in which the current efficiency of zinc deposition in an electrowinning operation was determined at various current densities (amperes per square meter of cathode surface area). The cathode area at the plant is 10,000 m2. Current Density Cell Voltage Current Efficiency (A/m2) (V) (%) 300 1.5 92 400 2.3 88 500 3 82 600 3.9 72 700 4.8 52 800 5.8 10 To investigate the tradeoff between increased production rate (increased current density) and cost please make a Table consisting of the following columns. Column 1 is the current... click for more

electrochemistry

3. Nickel is electrolytically refined at 40°C using an electrolyte containing 50 g/liter of nickel ion. The anodes contain copper impurities (< 2 wt.%) which may go into solution as the nickel anode dissolves. Calculate the concentration of Cu2+ ions in solution that is sufficient to result in the deposition of Cu at the cathode. Given your result, should one expect to have problems with Cu contamination in the refined Ni?