How many moles are in 117.30 grams of KCLO3?
1 answer:
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Answer:
It will take 5492 seconds to electroplate 0.5 mm of gold on an object .
Explanation:
Mass of gold = m
Volume of gold = v
Surface area on which gold is plated =
Thickness of the gold plating = h = 0.5 mm = 0.05 cm
1 mm = 0.1 cm
Density of the gold =
Moles of gold =
According to reaction, 1 mole of gold required 3 moles of electrons,then 0.152 moles of gold will require :
of electrons
Number of electrons = N =
Charge on single electron =
Total charge required = Q
Amount of current passes = I = 8 Ampere
Duration of time = T
It will take 5492 seconds to electroplate 0.5 mm of gold on an object .