A electrolytic cell is set up as was done in this experiment but with a differen

Question

A electrolytic cell is set up as was done in this experiment but with a different metal. An average current of 135.4 mA is delivered for 15 minutes and 23 seconds. The cathode gains 0.0728 g in mass. If there are two moles of electrons transferred per mole of the metal, what is the molar mass of the metal? What mass of sodium metal can be obtained from the electrolysis of molten sodium chloride if a current of 10.0 amps is allowed to pass though the cell for 45 minutes? How many hours are required to obtain 150.0 g of chromium metal from a solution of chromium(III) nitrate if a current of 2.50 amps Is passing through the cell?

Explanation / Answer

amount of charge passed through the cell = 135.4 *10^-3 A * 15.23 min * 60 = 12.372 c = 12.372c/96500 c/F

=1.29*10^-3 F

molar mass of the metal = 0.0728 gm/0.5mole metal/F * 1.29*10^-3 F =112.87 gm/mol

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m = (Q/F)(M/z)

m = (10 amp * 45 min * 60/ 96500) (58.5/1) =

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m = (Q/F)(M/z)

or, Q = m *z *F/M

= 150 gm * 3 *96500/238.011 gm/mol = 182449.55

Q = C *t = 182449.55

or, t = 182449.55/ 2.5 amp= 72979.82 sec = 20.27 hr.   

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