How many minutes will it take to plate out 4.50 g of Cu from a solution of Cu(NO3)2 (aq) onto the cathode of an electrolytic cell when 8.00 A of current are used? a. 28.5 min. b. 3.06 × 10^−9 min. c. 14.2 min. d. 1.82 × 10^3 min.

a. 28.5 min

Explanation:

The computation of the number of minutes would it take to plate out is as follows:

Cu+2 +2e Cu

 The two moles of electrons could be generated for the copper i.e. deposited

Now

moles of copper is

= 4.5 ÷ 63.5

= 0.071

The 63.5 represents the atomic copper weight

Now mole of electrons deposited is

= 0.071 × 2

= 0.142

Now

quantitiy of electricity needed

= moles of electrons deposited × 96500

= 0.142 × 96500

= 13703 coulums

As per electricity quantity needed

=  current ×  time(seconds)

= 13703 = 8 × t

t = 13703 ÷ 8

= 1713 seconds

= 1713 ÷ 60 minutes

=28.5 min

hence, the correct option is a.

metals are good conductor of electricity. it has free electrons on their surface. according to electron pool theory, each atom present in a metal crystal losses all of its valence electron and as a result a pool of free is form. these pool of electrons are free to move and   conduct electricity easily   while making metal as good conductor.

the correct answer is a. the ability of electrons to flow throughout the metal.

if it's not useful, feel free to report for mistake in answer.

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