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Karnataka Board PUCPUC Science 2nd PUC Class 12
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पाठ्यक्रम

Electrochemical Cells

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Estimated time: 12 minutes

Electrochemical Cells

Daniell Cell Interactive
Select operating mode:
Eext < 1.1V ZnSO₄ (aq) CuSO₄ (aq) Zn (anode, −ve) Cu (cathode, +ve) Salt bridge e⁻ → ← current I = 0
⚡ Galvanic Cell — spontaneous reaction
Zn anodeZn dissolves → Zn²⁺ ions released into solution
Cu cathodeCu²⁺ gains electrons → Cu deposits on electrode
e⁻ flowElectrons travel Zn → Cu through external wire
currentConventional current flows Cu → Zn (opposite to e⁻)
Reaction: Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s)  |  Cell potential = 1.1 V
Concept connections
Redox reaction Zn→Zn²⁺, Cu²⁺→Cu Electron flow Zn → Cu (galvanic) Salt bridge Maintains charge balance Electrolytic cell E_ext > 1.1V Cell potential 1.1 V (standard)
Click any concept box to learn more
Maharashtra State Board: Class 12

Key Points: Electrochemical Cells

Type Electrolytic Cell Galvanic (Voltaic) Cell
Energy conversion Electrical → Chemical Chemical → Electrical
Nature of reaction Non-spontaneous Spontaneous
Anode Positive Negative
Cathode Negative Positive
Electron flow Cathode → Anode Anode → Cathode
Salt bridge Not required Required

Electrolysis of NaCl

1. Molten NaCl:

  • Oxidation: Cl⁻ → Cl₂ (gas)

  • Reduction: Na⁺ → Na (metal)

  • Products: Na (cathode), Cl₂ (anode)

2. Aqueous NaCl:

  • Oxidation: Cl⁻ → Cl₂

  • Reduction: H₂O → H₂ + OH⁻

  • Products: H₂ (cathode), Cl₂ (anode), NaOH formed

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Electrochemistry [00:35:33]
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Series: Electrochemical Cells
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Electrochemistry
00:35:33  undefined
Electrochemistry part 2 (History, Voltaic Pile)
00:14:31  undefined
Electrochemistry part 3 (Concepts, Reactivity series)
00:12:49  undefined
Electrochemistry part 4 (Daniell Cell)
00:16:18  undefined

Related QuestionsVIEW ALL [73]

`E_(cell)^Θ` for some half cell reactions are given below. On the basis of these mark the correct answer.

(a) \[\ce{H^{+} (aq) + e^{-} -> 1/2 H_2 (g); E^Θ_{cell} = 0.00V}\]

(b) \[\ce{2H2O (1) -> O2 (g) + 4H^{+} (aq) + 4e^{-}; E^Θ_{cell} = 1.23V}\]

(c) \[\ce{2SO^{2-}_{4} (aq) -> S2O^{2-}_{8} (aq) + 2e^{-}; E^Θ_{cell} = 1.96V}\]

(i) In dilute sulphuric acid solution, hydrogen will be reduced at cathode.

(ii) In concentrated sulphuric acid solution, water will be oxidised at anode.

(iii) In dilute sulphuric acid solution, water will be oxidised at anode.

(iv) In dilute sulphuric acid solution, \[\ce{SO4^{2-}}\] ion will be oxidised to tetrathionate ion at anode.

Why is anode in galvanic cell considered to be negative and cathode positive electrode?

How will the pH of brine (aq. \[\ce{NaCl}\] solution) be affected when it is electrolysed?

Electrode potential for Mg electrode varies according to the equation

`E_(Mg^(2+)  |  Mg) = E_(Mg^(2+)  |  Mg)^Θ - 0.059/2 log  1/([Mg^(2+)])`. The graph of `E_(Mg^(2+)  |  Mg)` vs `log [Mg^(2+)]` is ______.

A gas X at 1 atm is bubbled through a solution containing a mixture of 1 MY− and 1 MZ− at 25°C. If the reduction potential of Z > Y > X, then ______.

`E_(cell)^Θ` = 1.1V for Daniel cell. Which of the following expressions are correct description of state of equilibrium in this cell?

(i) 1.1 = `K_c`

(ii) `(2.303RT)/(2F) logK_c` = 1.1

(iii) `log K_c = 2.2/0.059`

(iv) `log K_c` = 1.1

Reduction potential of two metals M1 and M2 are \[\ce{E^0_{{M_1^{2+}|M_1}}}\] = −2.3 V and \[\ce{E^0_{{M_2^{2+}|M_2}}}\] = 0.2 V. Predict which one is better for coating the surface of iron.
Given: \[\ce{E^0_{{Fe^{2+}|Fe}}}\] = −0.44 V

The number of moles of electrons passed when the current of 2 A is passed through a solution of electrolyte for 20 minutes is ______.

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