Advertisements
Advertisements
प्रश्न
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?
उत्तर
Given: Equilibrium constant of the reaction (K) = 1.2 × 106.
To find: Standard potential of cell \[\ce{E^{\circ}_{cell}}\]
Formulae: \[\ce{E^{\circ}_{cell}}\] = `(0.0592 "V")/"n" log_10K`
Calculation:
For the given reaction, n = 1.
Using formula,
`("E"_"cell"^circ) = 0.0592/1 xx log_10 (1.2 xx 10^6)`
`("E"_"cell"^circ) = 0.0592 xx (6.079)` = 0.36 V
The standard cell potential of cell is 0.36 V.
APPEARS IN
संबंधित प्रश्न
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.
Write a mathematical expression for Standard Cell Potential.
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.
Derive the relationship between Gibbs energy of cell reaction and cell potential.
The standard emf of a galvanic cell involving cell reaction with n = 1 was found to be 0.592 V at 25°C. The equilibrium constant of the reaction would be ____________.
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)
