okay, yesterday we did an experiment involving oxidation and reduction. It was one of those experiments where you make a circuit and with time notice a build up of metal in one of the two electrodes. Anyway, we used copper for the electrodes. here are the results:

 

Current: 1.0 A

Time: 900 secs

Charge: 900 coloumbs

Initial mass of cathode: 2.58 g

Final mass of cathode: 2.85 g

Mass gain: 0.27 g

 

1) Calculate the quantity of charge, measured in coulombs, required to deposit 63.5 g (1.0 mol) of copper metal.

 

pretty standard question, anyway any help would be appreciated.

both electrodes (anode and cathode) were made of copper. this was dunked into copper sulfate solution for 15 mins.

Since you know the weight of the copper and the charge required to generate that much copper you should be able to determine the total charge required to generate a different quantity by multiplying the known charge by the ratio of the mass right?

So by solving for x in:

63.5g/0.27g = x/900 C

 

we get the answer?

Does this fraction thing only work for things that are directly proportional (i.e. produces a linear graph when plotted/sketched)?