A total charge of 96.5 kC is passed through an electrolytic cell. What mass of copper will be produced from a copper(II) chloride solution?
Answer in units of g.
Help please?
Answer in units of g.
Help please?
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My favourite kind of electrochemistry question!
You need to go from a total amount of charge, to a mass of Cu produced. To do this, we need to know our reduction half reaction. CuCl is Cu in a 2+ oxidation state:
Cu(2+) + 2e- ----> Cu
So, we have:
96.5 x10^3 c (1 mol e- / 96485 c) (1 mol Cu / 2 mol e-) ( 63.5 g / 1 mol Cu) = 31.75 g Cu produced
The 1 mol Cu / 2 mol e- came from my balanced reduction half reaction above
The 1 mol e- / 96485 c is Faraday's number.
Hope that clarifies things!
You need to go from a total amount of charge, to a mass of Cu produced. To do this, we need to know our reduction half reaction. CuCl is Cu in a 2+ oxidation state:
Cu(2+) + 2e- ----> Cu
So, we have:
96.5 x10^3 c (1 mol e- / 96485 c) (1 mol Cu / 2 mol e-) ( 63.5 g / 1 mol Cu) = 31.75 g Cu produced
The 1 mol Cu / 2 mol e- came from my balanced reduction half reaction above
The 1 mol e- / 96485 c is Faraday's number.
Hope that clarifies things!