Which of the following statements is true for the following half cell reactions- F2g - 2e- - 2F-aq- E0 - 2-87 VCl2g - 2e- - Cl-aq- E0 - 1-36 VFe3-aq - e- - Fe2-aq- E0 - 0-77 V

Standard reduction potentials (SRP) of the half cell electrodes are calculated and arranged nbsp;in nbsp;a series of increasing order which is known as elec ...

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Standard X

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Application of Electrolysis

Which of the ...

Question

Which of the following statements is true for the following half cell reactions?

$F_{2} (g) + 2 e^{-} \to 2 F^{-} (a q); E^{0} = 2.87 V C l_{2} (g) + 2 e^{-} \to C l^{-} (a q); E^{0} = 1.36 V F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q); E^{0} = 0.77 V$

F_{2}

is the strongest oxidising agent

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F^{-}

gets oxidised to

F_{2}

C l_{2}

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F^{-}

gets oxidised to

F_{2}

F e^{3 +}

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All of the above

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Solution

The correct option is A $F_{2}$ is the strongest oxidising agent
Standard reduction potentials (SRP) of the half cell electrodes are calculated and arranged in a series of increasing order which is known as electrochemical series.
The standard electrode potential of $H^{+} / H_{2}$ couple is zero.

Here, a negative $E^{0}$ signifies that it has high tendency to get oxidised and the redox couple is a stronger reducing agent than the $H^{+} / H_{2}$ couple.

A positive $E^{0}$ signifies that it has high tendency to get reduced and the redox couple is a stronger oxidising agent than the $H^{+} / H_{2}$ couple.

Going down the electrochemical series, the $E^{0}$ value decrease i.e., the strength of oxidising agent gets reduced.

In the given half cell reactions,
$F_{2} / F^{-}$ couple has the highest $E^{0}$ value.
Hence, it is the strongest oxidising agent.
It oxidise both $C l^{-}$ and $F e^{2 +}$ to $C l_{2}$ and $F e^{3 +}$ respectively.

Since, $F_{2} / F^{-}$ couple has the highest $E^{0}$ value, it can't be oxidised by both $C l_{2} / C l^{-}$ and $F e^{3 +} / F e^{2 +}$ couples.

Hence, statement (a) is correct.

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Similar questions

Q. Which of the following statement(s) is/are true for the following half cell reactions?

F_{2} (g) + 2 e^{-} \to 2 F^{-} (a q); E^{0} = 2.87 V C l_{2} (g) + 2 e^{-} \to C l^{-} (a q); E^{0} = 1.36 V F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q); E^{0} = 0.77 V

Q. Choose the correct statement among the following for the given half cell reaction:

F_{2} (g) + 2 e^{-} \to 2 F^{-} (a q); E^{0} = 2.87 V C l_{2} (g) + 2 e^{-} \to C l^{-} (a q); E^{0} = 1.36 V F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q); E^{0} = 0.77 V

Q. Choose the correct option(s) for the given half cell reactions:

F_{2} (g) + 2 e^{-} \to 2 F^{-} (a q); E^{0} = 2.87 V C l_{2} (g) + 2 e^{-} \to 2 C l^{-} (a q); E^{0} = 1.36 V F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q); E^{0} = 0.77 V

Q. The values of

E^{0}

of some of the reactions are given below:

I_{2} (g) + 2 e^{-} \to 2 I^{-} (a q); E^{0} = + 0.54 V

C l_{2} (g) + 2 e^{-} \to 2 C l^{-} (a q); E^{0} = + 1.36 V

F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q); E^{0} = + 0.76 V

C e^{4 +} (a q) + e^{-} \to C e^{3 +} (a q); E^{0} = + 1.60 V

S n^{4 +} (a q) + 2 e^{-} \to S n^{2 +} (a q); E^{0} = + 0.15 V

Which of the following statement is/are true?

Q. What will be the

E^{0}

value for the given half cell reaction?

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

Given:

E^{0}

value for the half cell reaction,

F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q); E^{0} = 0.77 V

F e^{2 +} (a q) + 2 e^{-} \to F e (s); E^{0} = - 0.44 V

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Which of the following statements is true for the following half cell reactions? F2(g)+2e−→2F−(aq);E0=2.87 VCl2(g)+2e−→Cl−(aq);E0=1.36 VFe3+(aq)+e−→Fe2+(aq);E0=0.77 V

Which of the following statements is true for the following half cell reactions?

$F_{2} (g) + 2 e^{-} \to 2 F^{-} (a q); E^{0} = 2.87 V C l_{2} (g) + 2 e^{-} \to C l^{-} (a q); E^{0} = 1.36 V F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q); E^{0} = 0.77 V$