The standard reaction Gibbs energy for the electrochemical reaction-Cr2 O2-7 - 2Fe - 14H- - 2 Cr3- - 2Fe3- - 2H2O- is -793 kJ mol-1- The standard cell potential is Volts-

Δ G^∘ = nFE^∘_cell Here n = 6, 793 × 10^3 = 6 × 96500 × E^∘_cell E^∘_cell = + 1.3696 ≈1.37V ...

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Standard XII

Chemistry

Equilibrium Constant and Standard Free Energy Change

The standard ...

Question

The standard reaction Gibbs energy for the electrochemical reaction,

$C r_{2} O_{7}^{2 -} + 2 F e + 14 H^{+} \to 2 C r^{3 +} + 2 F e^{3 +} + 2 H_{2} O$ , is $- 793 k J m o l^{- 1}$ . The standard cell potential is Volts.

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Solution

$Δ G^{\circ} = - n F E_{c e l l}^{\circ}$

Here $n = 6$ ,

$- 793 \times 10^{3} = - 6 \times 96500 \times E_{c e l l}^{\circ}$

$E_{c e l l}^{\circ} = + 1.3696$

$\approx 1.37 V$

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Similar questions

The standard reaction gibbs energy for the electrochemical reaction.

$C r_{2} O_{7}^{2 -} + 2 F e + 14 H^{+} \to 2 C r^{3 +} + 2 F e^{3 +} + 2 H_{2} O$ is $- 793 k J m o l^{- 1}$ . The standard cell potential is:

Q. The standard reaction, Gibbs energy for the electrochemical reaction.

C r_{2} O_{7}^{2 -} + 6 F e^{2 +} + 14 H^{+} \to 2 C r^{3 +} + 6 F e^{3 +} + 7 H_{2} O i s - 793 k J m o l^{- 1}

The standard cell potential is:

The standard electrode potential for an electrochemical cell is $2.2 V$ . Calculate the standard Gibbs energy change for reaction:
$X (s) + Y^{2 +} (a q) \to X^{2 +} (a q) + Y (s)$
(Given, $1 F = 96500 C m o l^{- 1}$ )
(correct answer +1, wrong answer -0.25)

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

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Q. Standard enthalpy and standard entropy changes for the oxidation of ammonia at 298 K are382.64 kJ mol

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The standard reaction Gibbs energy for the electrochemical reaction, Cr2O2−7+2Fe+14H+→2Cr3++2Fe3++2H2O, is −793 kJ mol−1. The standard cell potential is Volts.

ΔG∘=−nFE∘cell Here n=6, −793×103=−6×96500×E∘cell E∘cell=+1.3696 ≈1.37V

The standard reaction Gibbs energy for the electrochemical reaction,

$C r_{2} O_{7}^{2 -} + 2 F e + 14 H^{+} \to 2 C r^{3 +} + 2 F e^{3 +} + 2 H_{2} O$ , is $- 793 k J m o l^{- 1}$ . The standard cell potential is Volts.

$Δ G^{\circ} = - n F E_{c e l l}^{\circ}$

Here $n = 6$ ,

$- 793 \times 10^{3} = - 6 \times 96500 \times E_{c e l l}^{\circ}$

$E_{c e l l}^{\circ} = + 1.3696$

$\approx 1.37 V$