Advertisements
Advertisements
Question
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.
Solution
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.
APPEARS IN
RELATED QUESTIONS
Answer the following in brief.
Using the relationship ΔG° of cell reaction and the standard potential associated with it, how will you show that the electrical potential is an intensive property?
Derive the relationship between standard cell potential and equilibrium constant of cell reaction.
Equilibrium constant of the reaction, \[\ce{2Cu^{\oplus}_{(aq)} -> Cu^{2\oplus}_{(aq)} + Cu_{(s)}}\] is 1.2 × 106. What is the standard potential of the cell in which the reaction takes place?
Write a mathematical expression for Standard Cell Potential.
Derive the relationship between Gibbs energy of cell reaction and cell potential.
If entropy of a solid is greater than zero, at T = 0, it is called ______.
Standard hydrogen electrode (SHE) is a ______.
Consider the cell \[\ce{Al | Al^{3+} (1 M) || Sn^{2+} (1 M) | Sn}\], \[\ce{E^0_{Al}}\] = −1.66 V; \[\ce{E^0_{Fe}}\] = −0.136 V, ∆G0 for the above cell is ____________.
The standard emf of Daniel cell is 1.10 volt. What is the maximum electrical work obtained from Daniel cell? (F = 96500 C)
Calculate Standard cell potential for a cell having following reaction, \[\ce{2Al(s) + 3Ni^{2+} -> 2Al^{3+} + 3Ni(s)}\]
`("E"_"Ni"^circ = - 0.25 "V" and "E"_"Al"^circ = 1.66 "V")`
Calculate standard Gibbs energy change at 25°C for the cell reaction.
\[\ce{Cd_{(s)} + Sn^{2+}_{ (aq)} -> Cd^{2+}_{ (aq)} + Sn_{(s)}}\]
\[\ce{E^0_{cd}}\] = –0.403 V, \[\ce{E^0_{Sn}}\] = –0.136 V
E0cell (Standard Potential of cell) for the following cell reaction is ______.
\[\ce{Cd_{(s)} + Sn^{2+}_{(aq)}-> Cd^{2+}_{(aq)} + Sn_{(s)}}\]
(E0Cd = − 0.403 V and E0Sn = − 0.136 V)
