Which of the following relations about E^{cir | vedclass

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(D) The standard cell potential is given by $E^{\circ}_{cell} = E^{\circ}_{cathode} - E^{\circ}_{anode}$.From the Nernst equation at equilibrium,$\Del

Vedclass · Accepted Answer

$E^{\circ}_{cell} = E^{\circ}_{anode} + E^{\circ}_{cathode}$

Vedclass · Answer

(D) The standard cell potential is given by $E^{\circ}_{cell} = E^{\circ}_{cathode} - E^{\circ}_{anode}$.From the Nernst equation at equilibrium,$\Delta G^{\circ} = -nFE^{\circ}_{cell}$,which implies $E^{\circ}_{cell} = \frac{-\Delta G^{\circ}}{nF}$.Also,$E^{\circ}_{cell} = \frac{RT}{nF} \ln K_{c} = \frac{0.0592}{n} \log_{10} K_{c}$ at $298 \ K$.Option $D$ is false because the standard cell potential is the difference between the reduction potentials of the cathode and the anode,not the sum.

Element	$M^{3+}/M$	$M^{+}/M$
$Al$	$-1.66$	$+0.55$
$Tl$	$+1.26$	$-0.34$

Which of the following relations about $E^{\circ}_{cell}$ is false?

Similar Questions

Consider the following standard electrode potentials ($E^0$ in volts) in aqueous solution. Based on this data,which of the following statements is correct?
Element $M^{3+}/M$ $M^{+}/M$
$Al$ $-1.66$ $+0.55$
$Tl$ $+1.26$ $-0.34$

Hydrogen gas is not liberated when the following metal is added to dil $HCl$.

The standard Gibbs energy for the given cell reaction in $kJ \, mol^{-1}$ at $298 \, K$ is $Zn_{(s)} + Cu^{2+}_{(aq)} \to Zn^{2+}_{(aq)} + Cu_{(s)}$,given $E^o = 2 \, V$ at $298 \, K$ [Faraday's constant $F = 96500 \, C \, mol^{-1}$].

If $E^0_{Fe^{3+}/Fe} = x \ V$ and $E^0_{Fe^{2+}/Fe} = y \ V$,then what will be the value of $E^0_{Fe^{3+}/Fe^{2+}}$?

Consult the table of standard electrode potentials and suggest three substances that can oxidise ferrous ions under suitable conditions.

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