# Problem: Gold is electroplated by a current of 0.5 A for a period of 35 minutes from a solution containing the Au3+ ion.  What is the mass of gold deposited on the electrode during this period. (At Wt Au = 197 g/mol)            A)        2.143 g            B)        0.0119 g            C)        0.01088 g            D)        0.715 g            E)         0.036 g

###### FREE Expert Solution

We’re being asked to calculate the mass of the gold (Au) deposited on the electrode after 35 minutes. Gold is electroplated from a solution containing Au3+ ion.

Let’s first determine what happens to Au3+:

Au(s) must be formed from Au3+(aq)
Au3+ needs to gain 3 e- in order to become Au(s)

###### Problem Details

Gold is electroplated by a current of 0.5 A for a period of 35 minutes from a solution containing the Au3+ ion.  What is the mass of gold deposited on the electrode during this period. (At Wt Au = 197 g/mol)

A)        2.143 g

B)        0.0119 g

C)        0.01088 g

D)        0.715 g

E)         0.036 g

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Electroplating concept. If you need more Electroplating practice, you can also practice Electroplating practice problems.

What is the difficulty of this problem?

Our tutors rated the difficulty ofGold is electroplated by a current of 0.5 A for a period of ...as medium difficulty.