What mass of silver can be plated onto an object in 33.5 minutes at 8.70 a of current? ag (aq e- ? ag(s what mass of silver can be plated onto an object in 33.5 minutes at 8.70 a of current? ag (aq e- ? ag(s 9.78 g 0.102 g 3.07 g 0.326 g 19.6 g?

Last option 19.6 g

Explanation:

In order to do this, we need to apply the Faraday law which is the following:

q = I*t (1)

Where:

I: current in Amperius

t: time in seconds

q: charge in Coulombs

the time in seconds is:

t = 33.5 min * 60 s/min = 2,010 s

Replacing in (1):

q = 8.7 * 2,010 = 17,487 C

With this value, we need to calculate the moles of Ag. This can be done dividing this value with the respective charge in one mole:

moles = q/n

n: value of 1 mole of electron / C = 96500 C/mol e

Replacing we have:

moles = 17.487 / 96,500

moles = 0,1812 moles e

Remember now that each mole of Ag+ can only catch one electron at a time, so, 0.1812 moles e, would be 0.1812 moles.

Finally, we need the molecular mass of Ag, which is 107.87 g/mol so:

m = 0.1812 * 107.87

m = 19.55 g or 19.6 g

c) up

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