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A sculptor has asked you to help electroplate gold onto a brass statue. You know that the charge carriers in the ionic solution are singly ionized gold ions, and you've calculated that you must deposit 0.50 g of gold to reach the necessary thickness. How much current do you need, in mA, to plate the statue in 6.0 hours?

Respuesta :

Answer:

Explanation:

Mass of gold deposited = 0.5 g

Molar mass of gold = 197 g/mol

Time, t = 6 hours

= 6 × 3600

= 12600 s

Number of moles = mass/molar mass

= 0.5/197

= 0.00254 mole

Assuming

Au --> Au+ + e-

Faraday constant = 9.65 x 104 C mol-1

Q = 96500 × 0.00254

= 244.924 C

Q = I × t

I = 244.924/12600

= 0.011 A

= 11.34 mA.

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