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It will take 9.64 minutes to deposit 1.00g of Zn metal
Convert the mass of Zn produced into moles using the molar mass of Zn.
Molar mass of Zinc = 65.38
No of moles of Zn = 1.00 × = 0.015 moles of Zinc
the half-reaction for the production of Zn at the cathode.
Zn²⁺ (aq) + 2 e⁻ → Zn(s)
the moles of e⁻ required to produce the moles of Zn using the stoichiometry of the balanced half-reaction.
According to the equation 2 moles of electrons will produce one mole of zinc.
0.015 × 2 mole e⁻ / 1 mole of Zn = 0.03 mol e⁻
Convert the moles of electrons into coulombs of charge using Faraday's constant.
1 F = 96485 C
0.03 × 1 F / 1 mole
= 0.03 × 96485 / 1
= 2894.55 C
the time using the current and the coulombs of charge.
5.00 A × t = 2894.55 C
t = 2894.55 / 5.00
t = 578.91 s
= 9.64 minutes
To learn more about electrolysis from the given link
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