Question

What is the power dissipated by this "resistor" when connected to the 24 V ? A sculptor has asked you to help electroplate gold onto a brass statue. You know that the charge carriers in the ionic solution are gold ions (singly ionized charge: 1.6×10⁻¹⁹ , and you've calculated that you must deposit 0.212 g of gold to reach the necessary thickness. How much current do you need to plate the statue in 8.0 hours? Gold is 197 g/mol and 1 mol=6.022×10²³ ions.

Answer 1

To calculate the current required to plate the statue with gold, we can use Faraday's law of electrolysis. The current required to plate the statue in 8.0 hours is approximately 0.495 Amperes.

Step-by-step explanation:

To calculate the current required to plate the statue with gold, we can use Faraday's law of electrolysis. According to Faraday's law, the amount of substance deposited at an electrode is directly proportional to the amount of charge passed through the electrode. The equation to calculate the current required is:

I = (m*n*F)/(t*Z)

Where:

• I is the current in Amperes
• m is the mass of gold to be deposited in grams
• n is the number of electrons per gold ion (1 in this case)
• F is Faraday's constant (96,485 C/mol)
• t is the time in seconds
• Z is the molar mass of gold in grams/mol

Let's plug in the values:

I = (0.212 g * 1 * 96,485 C/mol) / (8.0 hours * 3600 seconds/hour * 197 g/mol)

I = 0.495 A

Therefore, the current required to plate the statue in 8.0 hours is approximately 0.495 Amperes.