Suppose a similar electroplating experiment as the ones conducted in this lab is

Question

Suppose a similar electroplating experiment as the ones conducted in this lab is conducted to purify copper metal from 200 ml. of a 1.5 M copper sulfate solution (CuSO_4) You used a battery whose energy capacity is listed as 2500 mAh (milli-ampere hours) and you can assume that the entire battery charge is useable for electroplating You completely drain the battery during the experiment How much copper (g) was pulled out of solution? Note that copper ions have a +2 charge and thus need two electrons to make it a neutral metal atom (Show your work for full credit)

Explanation / Answer

2500 mAH of a 1.5V cell is equal to

So watt-hour is equal to milliamp-hour times volts divided by 1000:

watt-hours = milliampere-hours × volts / 1000

or

Wh = mAh × V / 1000 = (2500 x1.5)/1000 = 3.75 Wh

No of joules of energy produces = 3.75 x 3.6 x 103 J=13500 J

E/V = Q = 13500/1.5 = 9000 Coulombs

Q = n(e-) x F where F = 96500 coulombs mol-1

9000 = n(e-) x 96500

n(e-) = 9000/96500 = 0.0932 moles of electrons

each copper needs 2e- so amount of copper atoms produced is 0.0932/2 = 0.0466 moles = 2.96 g

a 200 mL 1.5M CuSO4 solution has 47.7 g CuSO4 so it has 18.9 g of copper

2.96 g of copper is pulled out of the solution containing 18.9 g of copper(II)

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