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Factors Affecting Electrolysis

Consider a ce...

Question

Consider a cell given below
$C u ∣ C u^{2} + ∣∣ C l^{-} ∣∣ C l_{2}, P t$
Write the reactions that occur at
anode and cathode.

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Solution

Cell representation for the given cell -
$C u | C u^{2 +} | | C l^{-} | C l_{2}, P t$

We know that in an electrolytic cell, oxidation
occurs at anode and reduction occurs at cathode. Hence the reaction are-

At anode: $C u \to C u^{2 +} + 2 e -$

At Cathode: $C l_{2} + 2 e^{-} \to 2 C l -$

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Similar questions

The cell potential for the electrochemical reaction shown below depends upon the

C l^{-}

C u^{2 +}

concentrations. Calculate the cell potential (in V) at

25^{0} C

C u^{2 +}

] = 3.5 M and [

C l^{-}

C u^{2 +}

C l^{-}

\Leftrightarrow

Cu(s) + 2AgCl(s) ; E = 0.12 V

Consider the cell:

Z n | Z n^{2 +} (a q) (1.0 M) | | C u^{2 +} (a q) (1.0 M) | | C u

The standard reduction potential are

0.350

C u^{2 +} (a q) + 2 e^{-} \to C u

- 0.763

Z n^{2 +} (a q) + 2 e^{-} \to Z n

The cell reaction is:

write down the cell reactions occuring in following cells?

1)(Pt)H₂/H⁺//Cu²⁺/Cu 2)Cd/Cd²⁺//Cl^-/AgCl/Ag 3)Pt/ClO₃^-_,Cl^-//ClO₂^-/Cl₂(Pt)

Q. The cell reaction for the given cell is spontaneous if:

P t | C l_{2} | P_{1} | C l^{-} (1 M) | | C l^{-} (1 M) | P t | C l_{2} P_{2}

Q. 20. The cell reaction for the given cell is spontaneous if pt | Cl2(p1atm) | Cl-1(1M) | Cl2(P2atm) | Pt

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Factors Affecting Electrolysis

Standard X Chemistry

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