What mass (in g) of silver can be electroplated when 0.385 amps are used for 1.259 hours using a solution of silver nitrate?

1.96 grams

Explanation:

where Q= quantity of electricity in coloumbs

I = current in amperes = 0.385 A

t= time in seconds = 1.259 hours = 4532.4 sec  (1hour =3600 s)

96500C of electricity deposits 1 mole of Ag

1755 C of electricity deposits = of Ag

Thus 1.96 g of silver can be electroplated when 0.385 amps are used for 1.259 hours using a solution of silver nitrate.

chemistry sucks a**

explanation:

there are no statements provided but here is why:

sulfur belongs to group 16 because it can be found in nature whether it is in a free or combined state.

hope this