The electrode with reactionCr2O72-aq-14H-aq-6e- 2Cr3-aq-7H2Olcan be represented as-If needed- use platinum as an inert electrode-

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Representation of Cell

The electrode...

Question

The electrode with reaction
$C r_{2} O_{7}^{2 -} (a q) + 14 H^{+} (a q) + 6 e^{-} \to 2 C r^{3 +} (a q) + 7 H_{2} O (l)$
can be represented as:
[If needed, use platinum as an inert electrode]

P t (s) | H^{+} (a q), C r_{2} O_{7}^{2 -} (a q)

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P t (s) | H^{+} (a q) | | C r_{2} O_{7}^{2 -} (a q), C r^{3 +} (a q)

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P t (s), H_{2} (g) | H^{+} (a q), C r_{2} O_{7}^{2 -}

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H^{+} (a q), C r_{2} O_{7}^{2 -} (a q), C r^{3 +} (a q) | P t (s)

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Solution

The correct option is D $H^{+} (a q), C r_{2} O_{7}^{2 -} (a q), C r^{3 +} (a q) | P t (s)$
It is a redox electrode.
Here,
$C r_{2} O_{7}^{- 2}$ is reduce to $2 C r^{3 +}$ , so it must be represented at cathode.
It is a single electrode. Thus, there is no salt bridge.

Rules for Cell representation:
1. Anode half cell should be on left side and cathode half cell should be on right side.

2. Separation of two phase should be shown by vertical line $(∣)$ . This line indicates phase boundary.

3. If various material present in the same phase, it should be shown together with commas (,).

4. The salt bridge is represented by double slash $(∣∣)$ between the two half cells.

5. The significant features of the substance like pressure of a gas, concentration of ions, etc. should be indicated in brackets immediately after writing the substance.

6. For gas electrode, gas should be indicated after electrode for anode and should be indicated before electrode for cathode.

So, the cell representation is:
$H^{+} (a q), C r_{2} O_{7}^{- 2} (a q), C r^{3 +} (a q) | P t (s)$

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Similar questions

Q. The electrode with reaction :

C r_{2} O_{7}^{2 -} (a q) + 14 H^{\oplus} (a q) + 6 e^{-} \to 2 C r^{3 +} (a q) + 7 H_{2} O

can be represented as:

Q. The half cell involving the reaction

C r_{2} O_{7}^{2 -} (a q) + 14 H^{+} (a q) + 6 e \to 2 C r^{3 +} (a q) + 7 H_{2} O

can be represented as :

C r_{2} O_{7}^{2 -} (a q, 1 M) + 14 H^{+} (a q) + 6 e^{-} \to 2 C r^{3 +} (a q, 1 M) + 7 H_{2} O

. The standard electrode potential for the following reaction is + 1.33V. what is the potential at

p H = 2.0

C r_{2} O_{7}^{2 -} (a q, 1 M) + 14 H^{+} (a q) + 6 e^{-} \to 2 C r^{3 +} (a q, 1 M) + 7 H_{2} O

. The standard electrode potential for the following reaction is + 1.33V. what is the potential at

p H = 2.0

Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox Titration. Some half – cell reactions and their standard potential are given below:
$M n O_{4}^{-} (a q) + 8 H^{+} (a q) + 5 e^{-} \to M n^{2 +} (a q) + 4 H_{2} O (I); E^{\circ} = 1.51 V$
$C r_{2} O_{7}^{2 -} (a q) + 14 H^{+} (a q) + 6 e^{-} \to 2 C r^{3 +} (a q) + 7 H_{2} O (I); E^{\circ} = 1.38 V$
$F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q); E^{\circ} = 0.77 V$
$C l_{2} (g) + 2 e^{-} \to 2 C l^{-} (a q); E^{\circ} = 1.40 V$

Identify the only incorrect statement regarding the quantitative estimation of aqueous $F e (N O_{3})_{2}$ .

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Representation of Cell

Standard VII Chemistry

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The electrode with reaction Cr2O2−7(aq)+14H+(aq)+6e−→2Cr3+(aq)+7H2O(l) can be represented as: [If needed, use platinum as an inert electrode]

The electrode with reaction
$C r_{2} O_{7}^{2 -} (a q) + 14 H^{+} (a q) + 6 e^{-} \to 2 C r^{3 +} (a q) + 7 H_{2} O (l)$
can be represented as:
[If needed, use platinum as an inert electrode]