Find the emf of the following cell reaction,g | vedclass

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(C) The cell reaction is: $2Cr(s) + 3Fe^{2+}(aq) \rightarrow 2Cr^{3+}(aq) + 3Fe(s)$.Number of electrons transferred,$n = 6$.Standard cell potential: $

Vedclass · Accepted Answer

$0.26$

Vedclass · Answer

(C) The cell reaction is: $2Cr(s) + 3Fe^{2+}(aq) ightarrow 2Cr^{3+}(aq) + 3Fe(s)$.Number of electrons transferred,$n = 6$.Standard cell potential: $E^{\circ}_{cell} = E^{\circ}_{cathode} - E^{\circ}_{anode} = -0.44 - (-0.74) = 0.30 \ V$.Using the Nernst equation at $25^{\circ} C$ $(298 \ K)$:$E_{cell} = E^{\circ}_{cell} - \frac{0.0591}{n} \log \frac{[Cr^{3+}]^2}{[Fe^{2+}]^3}$.$E_{cell} = 0.30 - \frac{0.0591}{6} \log \frac{(0.1)^2}{(0.01)^3}$.$E_{cell} = 0.30 - \frac{0.0591}{6} \log \frac{10^{-2}}{10^{-6}} = 0.30 - \frac{0.0591}{6} \log(10^4)$.$E_{cell} = 0.30 - \frac{0.0591 	imes 4}{6} = 0.30 - 0.0394 = 0.2606 \ V \approx 0.26 \ V$.

$A$. $Ag^{+}(0.0001 \ M) / Ag_{(s)}$	$B$. $Ag^{+}(0.1 \ M) / Ag_{(s)}$
$C$. $Ag^{+}(0.01 \ M) / Ag_{(s)}$	$D$. $Ag^{+}(0.001 \ M) / Ag_{(s)}$

Find the $emf$ of the following cell reaction,given $E^0_{Cr^{3+}/Cr} = -0.74 \ V$ and $E^0_{Fe^{2+}/Fe} = -0.44 \ V$ at $25^{\circ} C$ for the cell: $Cr \ | \ Cr^{3+}(0.1 \ M) \ || \ Fe^{2+}(0.01 \ M) \ | \ Fe$. (in $V$)

Similar Questions

The $emf$ (in $V$) of a $Daniell$ cell containing $0.1 \ M \ ZnSO_4$ and $0.01 \ M \ CuSO_4$ solutions at their respective electrodes is $\left(E_{Cu^{2+} / Cu}^{\circ}=+0.34 \ V ; E_{Zn^{2+} / Zn}^{\circ}=-0.76 \ V\right)$

Consider the following $4$ electrodes:
$A$. $Ag^{+}(0.0001 \ M) / Ag_{(s)}$ $B$. $Ag^{+}(0.1 \ M) / Ag_{(s)}$
$C$. $Ag^{+}(0.01 \ M) / Ag_{(s)}$ $D$. $Ag^{+}(0.001 \ M) / Ag_{(s)}$

$E^{\circ}_{Ag^{+} / Ag} = +0.80 \ V$
Arrange the reduction potential of these electrodes in decreasing order.

Consider the following Galvanic cell. By what value does the cell voltage change when the concentration of ions in both the anodic and cathodic compartments is increased by a factor of $10$ at $298 \ K?$

$Cu_{(s)} | Cu^{+2}(aq, 10^{-3} M) || Ag^{+}(aq, 10^{-5} M) | Ag_{(s)}$
If $E^{o}_{Cu^{+2}/Cu} = +0.34 \ V$
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$E_{cell}$ will be

Which one of the following has a potential more than zero?

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