96,485 coulombs will deposit 107.86/1electron = 107.86 g Ag(s). 2.61 g Ag was deposited so we must have had 96,485 coulombs x (2.64/107.86) = 2,361.58 C.
We know 2,361.58 coulombs deposited 1.61 g Au.
96,485 C will deposit 196.97/#e g Au; therefore,
(196.97/#e) x (2,361.58/96,485) = 1.61 g
#e = 2.994 = 3. The slight difference is because I rounded here and there.
Oxidation state Au is 3.
In an electrolysis experiment a student passes the same quantity of electricity
through two electrolytic cells containing silver and gold salts, respectively. Over
a certain period of time she finds that 2.64 grams of Ag and 1.61 grams of Au are
deposited at the cathodes. What is the oxidation state of gold in the gold salt?
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