The time that is required to deposit the certain grams of copper is 34 min.
The charge that is carried by 2 moles of electrons is 96500 C. The amount of copper deposited is 1.36 g.
Thus, the charge required to deposit 1.36 g copper is calculated as follows:
=1.36 g*63.55 g/mol*96500 C
=4130 C
The current passing in an aqueous solution is 2.00 A.
Thus, the time required to deposit the amount of copper is calculated as follows:
t=q/C
t=4130 C/2.00 A
t=34 min
Thus, the time needed is 34 min.
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