Suppose the current flowing from a battery is used to electroplate an object with silver. Calculate the mass of silver that woul
d be deposited by a battery that delivers 1.65 A·hr of charge.
1 answer:
Answer:
m = 0.00659 kg = 6.59 g
Explanation:
From Faraday's Law of Electrolysis, we know that:
m = ZQ
where,
m = mass of silver deposited = ?
Q = charge supplied = (1.65 A-hr)(3600 s/1 hr) = 5940 C
Z = electrochemical equivalent of silver = 1.18 x 10⁻⁶ kg/C
Therefore,
m = (1.11 x 10⁻⁶ kg/C)(5940 C)
<u>m = 0.00659 kg = 6.59 g</u>
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