How many minutes will be required to deposit 1.00 g of chromium metal from an aqueous?

Given:

1 g of chromium metal

CrO4 2- solution

6.0 amperes of current

Find:

Minutes required = ?

1 amp = 1 coulomb / second 
6 amps = 6 coulombs / second... 

Also:

 
Cr in CrO4(-2) is +6 so we must reduce it to 0, i.e. 6 electrons per atom 

1g Cr x (1 mole Cr / 52.00g Cr) x (6 moles electrons / 1 mole Cr) x (6.022x10^23 electrons / mole electrons) x (1.602x10^-19 coulombs / 1 electron) x (1 sec / 6.00amps) x (1 min / 60x) = 30.9 min 

Therefore, 30.9 minutes will be required to deposit 1.00 g of chromium metal from an aqueous CrO4 2- solution using a current 6.00 amperes.

answers: to make sure that all of the broken pieces of tablet were added to the water, to allow for fair comparison of all three trials, with different particle sizes to avoid experimental error

yes

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