Answer:
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
The molecular mass of Silver is mathematically given as
m = 19.55 g
Question Parameters:
mass of silver that can be plated onto an object in 33.5 minutes at 8.70 a of current.
Generally, the equation for the Faraday law is mathematically given as
q = I*t (1)
Therefore
t = 33.5* 60
t= 2,010 s
Hence
q = 8.7 * 2010
w= 17487 C
Where moles of Ag is
moles = 17487 / 96500
moles = 01812 moles
In conclusion, the molecular mass of Ag is
m = 0.1812 * 107.87
m = 19.55 g
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