A current of 3.45 A is passed through a Ni(NO3)2 solution for 1.80 h. How much nickel is plated out of the solution?
What is the mass of nickel in grams?
Chemistry Question? Nickel Plating?
2020-05-25 11:33 pm
回答 (2)
2020-05-26 12:01 am
Amount of electricity = (3.45 C/s) × (1.80 × 3600 s) = 22356 C
Each mole of e⁻ carries 96485 C of electricity.
Moles of e⁻ = (22356 C) / (96485 C/mol) = 0.23170 mol
Ni²⁺(aq) + 2e⁻ → Ni(s)
Mole ratio e⁻ : Ni = 2 : 1
Moles of Ni plated = (0.23170 mol) × (1/2) = 0.11585 mol
Molar mass of Ni = 58.70 g/mol
Mass of Ni plated = (0.11585 mol) × (58.70 mol) = 6.80 g
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OR:
(3.45 C / 1 s) × (1.80 × 3600 s) × (1 mol e⁻ / 96485 C) × (1 mol Ni / 2 mol e⁻) × (58.70 g Ni / 1 mol Ni)
= 6.80 g Ni
Each mole of e⁻ carries 96485 C of electricity.
Moles of e⁻ = (22356 C) / (96485 C/mol) = 0.23170 mol
Ni²⁺(aq) + 2e⁻ → Ni(s)
Mole ratio e⁻ : Ni = 2 : 1
Moles of Ni plated = (0.23170 mol) × (1/2) = 0.11585 mol
Molar mass of Ni = 58.70 g/mol
Mass of Ni plated = (0.11585 mol) × (58.70 mol) = 6.80 g
====
OR:
(3.45 C / 1 s) × (1.80 × 3600 s) × (1 mol e⁻ / 96485 C) × (1 mol Ni / 2 mol e⁻) × (58.70 g Ni / 1 mol Ni)
= 6.80 g Ni
2020-05-26 12:03 am
Coulombs = 3.45 A X (1.80 hr) X 60 min/hr X 60 sec/min = 22356 C
Moles electrons = 22356 C / 96485 C/mol e- = 0.232 mol e-
Each mole of Ni2+ requires 2 moles of electrons to reduce it to Ni(s). So,
Moles Ni = 0.232 mol e- / 2 = 0.116 mol Ni(s)
Mass Ni = 0.116 mol X 58.69 g/mol = 6.80 g Ni(s)
Moles electrons = 22356 C / 96485 C/mol e- = 0.232 mol e-
Each mole of Ni2+ requires 2 moles of electrons to reduce it to Ni(s). So,
Moles Ni = 0.232 mol e- / 2 = 0.116 mol Ni(s)
Mass Ni = 0.116 mol X 58.69 g/mol = 6.80 g Ni(s)
收錄日期: 2021-04-18 18:30:03
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