What will be the E0 value for the given half cell reaction- Fe3-aq - 3e- - FesGiven-E0 value for the half cell reaction- Fe3-aq - e- - Fe2-aq- E0 - 0-77 VFe2-aq - 2e- - Fes- E0 - -0-44 V

Δ G^0 = nFE^0 Fe^3+(aq) + e^ → Fe^2+(aq)....(1); Δ G^0_1 = 1F × 0.77 Fe^2+(aq) + 2e^ → Fe(s)......(2); Δ G^0_2 = +2F × 0.44 Adding equation (1) and (2), w ...

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Byju's Answer

Standard VII

Chemistry

Gibb's Energy and Nernst Equation

What will be ...

Question

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,
$F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q); E^{0} = 0.77 V$
$F e^{2 +} (a q) + 2 e^{-} \to F e (s); E^{0} = - 0.44 V$

0.33 V

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1.21 V

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- 0.036 V

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0.605 V

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Solution

The correct option is C $- 0.036 V$
$Δ G^{0} = - n F E^{0}$

$F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q) . . . . (1); Δ G_{1}^{0} = - 1 F \times 0.77$
$F e^{2 +} (a q) + 2 e^{-} \to F e (s) . . . . . . (2); Δ G_{2}^{0} = + 2 F \times 0.44$

Adding equation (1) and (2), we get,
$F e^{3 +} (a q) + 3 e^{-} \to F e (s) . . . . . . . (3); Δ G_{3}^{0} = - 3 F E^{0}$

Thus,
$Δ G_{3}^{0} = Δ G_{1}^{0} + Δ G_{2}^{0}$
$- 3 F E^{0} = - 1 F \times 0.77 + 2 F \times 0.44$
$- 3 E^{0} = - 1 \times 0.77 + 2 \times 0.44$
$E^{0} = \frac{0.77 - 0.88}{3}$
$E^{0} = - 0.036 V$

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Similar questions

Q. What will be the

E^{0}

value for the given half cell reaction?

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

Given:

E^{0}

value for the half cell reaction,

C r^{3 +} (a q) + e^{-} \to C r^{2 +} (a q); E^{0} = - 0.41 V

C r^{3 +} (a q) + 3 e^{-} \to C r (s); E^{0} = - 0.74 V

Q. What will be the

E^{0}

value for the given half cell reaction?

S n^{4 +} (a q) + 4 e^{-} \to S n (s)

Given:

E^{0}

value for the half cell reaction,

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

S n^{2 +} (a q) + 2 e^{-} \to S n (s); E^{0} = - 0.14 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. 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

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

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What will be the E0 value for the given half cell reaction? Fe3+(aq)+3e−→Fe(s) Given: E0 value for the half cell reaction, Fe3+(aq)+e−→Fe2+(aq); E0=0.77 V Fe2+(aq)+2e−→Fe(s); E0=−0.44 V

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,
$F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q); E^{0} = 0.77 V$
$F e^{2 +} (a q) + 2 e^{-} \to F e (s); E^{0} = - 0.44 V$