Question

How many minutes will it take to electroplate 60.1 g of gold by running 5.00 a of current through a solution of au (aq?

Answer 1

Answer:

It would take 0.1 minutes (approximately 6 seconds)

Explanation:

Applying the Faraday's first law of electrolysis which states that,

    m = ZIt

where m is the mass electroplated, Z is the electrochemical equivalence of the element, I is the current and t is the time taken.

Z of gold = 2.04352g/As

Thus,

t = $\frac{m}{ZI}$

   = $\frac{60.1}{2.04352 *5}$

   = 5.882 s

To determine the time in minute, divide by 60;

t = 0.0980minute

t = 0.1 minute

Answer 2

For this problem, we use the Faradays law to relate the mass electroplated and the current passed through. We do as follows:

60.1 g (1 mol / 196.67 g) (1 mol e- / 1 mol Au) ( 96500 C / 1 mol e- ) = 29486.25 C

Q = It
29486.25 = 5t
t = 5897.85 s = 98.30 min

Hope this answers the question.