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Standard X

Chemistry

Electrolysis and Electrolytes

The given dia...

Question

The given diagram shows an electrochemical cell in which the respective half cells contain aqueous 1.0 M solutions of the salts $X C l_{2}$ and $Y C l_{3}$ . Given that,
$3 X_{(s)} + 2 Y_{(a q)}^{3 +} \to 3 X_{(a q)}^{2 +} + 2 Y_{(s)}, E_{c e l l} > 0$
Which of the following statement(s) is/are correct?

The electrode made from metal X has positive polarity.

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Electrode Y is the anode.

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The flow of electrons is from Y to X.

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The reaction at electrode X is an oxidation reaction.

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Solution

The correct option is D The reaction at electrode X is an oxidation reaction.
Oxidation occurs at the electrode X which is the anode and it has negative polarity.
Anode: $X \to X^{+ 2} + 2 e^{-}$
Cathode: $Y^{3 +} + 3 e^{-} \to Y$
Here, the electron is flowing from X to Y.
Option D is correct.

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Similar questions

Q. Iron and nickel are used to make an electrochemical cell by using a salt bridge to join a half-cell containing 1.0 M solution of

F e^{2 +} (a q)

in which a strip of iron has been immersed to a second half cell which contains 1.0 M

N i^{2 +} (a q)

solution in which a strip of nickel has been immersed. A voltmeter is connected between the two metal strips.
(i) In which cell does reduction occur?
(ii) Write the half-cell reactions involved.
(iii) Which metal is the anode?
(iv) In which direction are the electrons passing through the voltmeter?
(v) what would be effect on the voltmeter reading if

F e^{2 +}

concentration were increased?
(vi) what will be the voltmeter reading when the cell reaches equilibrium?

Q. (a) The cell in which the following reaction occurs:

2 F e^{3 +} (a q) + 2 I^{-} (a q) \to 2 F e^{2 +} (a q) + I_{2} (s)

has

E_{cell}^{⊝} = 0.236 V

at 298 K.
Calculate the standard Gibbs energy of the cell reaction. (Given: 2F= 96500 C

m o l^{- 1}

)
(b) How many electrons flow through a metallic wire if a current of 0.5 A is passed for 2 hours? (Given: 1F= 96500 C

m o l^{- 1}

)

The cell in which the following reaction occurs:

2 F e^{3 +} (a q) + 2 I^{-} (a q) \to 2 F e^{2 +} (a q) + I_{2} (s)

has

E_{c e l l}^{\circ} = 0.236 V

298 K

Calculate the standard Gibbs energy of the cell reaction. (Given :

1 F = 96, 500 C m o l^{- 1})

Q. Which of the following is true for the given half cell reaction?

X^{3 +} (a q) + 2 e^{-} \to X^{+} (a q); E^{o} = y V

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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The given diagram shows an electrochemical cell in which the respective half cells contain aqueous 1.0 M solutions of the salts XCl2 and YCl3. Given that, 3X(s)+2Y3+(aq)→3X2+(aq)+2Y(s), Ecell>0Which of the following statement(s) is/are correct?

The correct option is D The reaction at electrode X is an oxidation reaction.Oxidation occurs at the electrode X which is the anode and it has negative polarity.Anode: X→X+2+2e−Cathode: Y3++3e−→YHere, the electron is flowing from X to Y.Option D is correct.

The correct option is D The reaction at electrode X is an oxidation reaction.
Oxidation occurs at the electrode X which is the anode and it has negative polarity.
Anode: $X \to X^{+ 2} + 2 e^{-}$
Cathode: $Y^{3 +} + 3 e^{-} \to Y$
Here, the electron is flowing from X to Y.
Option D is correct.