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.

icc, international association for cereal chemistry

nuclear fission produces elements that are heavier than helium.

the elements that are used in nuclear fission and their products are much heavier than helium.