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प्रश्न
What is the mass of copper metal produced at cathode during the passage of 2.03 A current through the CuSO4 solution for 1 hour. Molar mass of Cu = 63.5 g mol–1.
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उत्तर
Given: Current strength = 2.03 A, Molar mass of Cu = 63.5 g mol–1
1 hours = 1 × 60 × 60 s = 3600 s
To find: Mass of copper metal produced at cathode
Formulae:
- Mole ratio = `"Moles of product formed in half-reaction"/"Moles of electrons required in half-reaction"`
- W = `("I"("A") xx "t" ("s"))/(96500 ("C"//"mol e"^-)) xx "mole ratio" xx "molar mass"`
Calculation:
Stoichiometry for the formation of Cu is
\[\ce{Cu^{2+}_{ (s)} + 2e^- -> Cu_{(s)}}\]
Using formula (i),
Mole ratio = `"1 mol"/"2 mol e"^-`
Using formula (ii),
W = `("I"("A") xx "t" ("s"))/(96500 ("C"//"mol e"^-)) xx "mole ratio" xx "molar mass"`
`= (2.03 "A" xx 3600)/(96500 ("C"//"mol e"^-1)) xx (1 "mol")/("2 mol e"^-) xx 63.5 "g mol"^-1`
= 2.4 g
Mass of copper metal produced at cathode is 2.4 g.
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