275972
What is the electrode potential (in $V$ ) of the following electrode at $25^{\circ} \mathrm{C}$ ?
$\mathrm{Ni}^{2+}(0.1 \mathrm{M}) \mid \mathrm{Ni}(\mathrm{s})$
(Standard reduction potential of $\mathrm{Ni}^{2+} \mid \mathrm{Ni}$ is)
$-0.25 \mathrm{~V}, \frac{2.303 \mathrm{RT}}{\mathrm{F}}=0.06$
275975 Two electrochemical cell $\mathrm{Fe}\left \vert\mathrm{Fe}^{2+} \ \vert \mathrm{Cu}^{2+}\right \vert \mathrm{Cu}$ and $\mathrm{Zn}\left \vert\mathrm{Zn}^{2+} \ \vert \mathrm{Cu}^{2+}\right \vert \mathrm{Cu}$ are connected in series. $\left(\mathrm{Fe}^{2+} / \mathrm{Fe}=-0.41 \mathrm{~V}, \mathrm{Zn}^{2+} / \mathrm{Zn}=-0.076 \mathrm{~V}, \mathrm{Cu}^{2+} /\right.$ $\mathrm{Cu}=+0.34 \mathrm{~V})$. The net emf of this cell is
275976
For the redox reaction
$\mathrm{Zn}(\mathrm{s})+\mathrm{Cu}^{2+}(0.1 \mathrm{M}) \rightarrow \mathrm{Zn}^{2+}(1 \mathrm{M})+\mathrm{Cu}(\mathrm{s})$
taking place in a cell, $\mathrm{E}_{\text {cell }}^{\circ}$ is $1.10 \mathrm{~V} \mathrm{E}_{\text {cell }}$ for the cell will be $\left(2 \cdot 303 \frac{\mathrm{RT}}{\mathrm{F}}=0.0591\right)$
275972
What is the electrode potential (in $V$ ) of the following electrode at $25^{\circ} \mathrm{C}$ ?
$\mathrm{Ni}^{2+}(0.1 \mathrm{M}) \mid \mathrm{Ni}(\mathrm{s})$
(Standard reduction potential of $\mathrm{Ni}^{2+} \mid \mathrm{Ni}$ is)
$-0.25 \mathrm{~V}, \frac{2.303 \mathrm{RT}}{\mathrm{F}}=0.06$
275975 Two electrochemical cell $\mathrm{Fe}\left \vert\mathrm{Fe}^{2+} \ \vert \mathrm{Cu}^{2+}\right \vert \mathrm{Cu}$ and $\mathrm{Zn}\left \vert\mathrm{Zn}^{2+} \ \vert \mathrm{Cu}^{2+}\right \vert \mathrm{Cu}$ are connected in series. $\left(\mathrm{Fe}^{2+} / \mathrm{Fe}=-0.41 \mathrm{~V}, \mathrm{Zn}^{2+} / \mathrm{Zn}=-0.076 \mathrm{~V}, \mathrm{Cu}^{2+} /\right.$ $\mathrm{Cu}=+0.34 \mathrm{~V})$. The net emf of this cell is
275976
For the redox reaction
$\mathrm{Zn}(\mathrm{s})+\mathrm{Cu}^{2+}(0.1 \mathrm{M}) \rightarrow \mathrm{Zn}^{2+}(1 \mathrm{M})+\mathrm{Cu}(\mathrm{s})$
taking place in a cell, $\mathrm{E}_{\text {cell }}^{\circ}$ is $1.10 \mathrm{~V} \mathrm{E}_{\text {cell }}$ for the cell will be $\left(2 \cdot 303 \frac{\mathrm{RT}}{\mathrm{F}}=0.0591\right)$
275972
What is the electrode potential (in $V$ ) of the following electrode at $25^{\circ} \mathrm{C}$ ?
$\mathrm{Ni}^{2+}(0.1 \mathrm{M}) \mid \mathrm{Ni}(\mathrm{s})$
(Standard reduction potential of $\mathrm{Ni}^{2+} \mid \mathrm{Ni}$ is)
$-0.25 \mathrm{~V}, \frac{2.303 \mathrm{RT}}{\mathrm{F}}=0.06$
275975 Two electrochemical cell $\mathrm{Fe}\left \vert\mathrm{Fe}^{2+} \ \vert \mathrm{Cu}^{2+}\right \vert \mathrm{Cu}$ and $\mathrm{Zn}\left \vert\mathrm{Zn}^{2+} \ \vert \mathrm{Cu}^{2+}\right \vert \mathrm{Cu}$ are connected in series. $\left(\mathrm{Fe}^{2+} / \mathrm{Fe}=-0.41 \mathrm{~V}, \mathrm{Zn}^{2+} / \mathrm{Zn}=-0.076 \mathrm{~V}, \mathrm{Cu}^{2+} /\right.$ $\mathrm{Cu}=+0.34 \mathrm{~V})$. The net emf of this cell is
275976
For the redox reaction
$\mathrm{Zn}(\mathrm{s})+\mathrm{Cu}^{2+}(0.1 \mathrm{M}) \rightarrow \mathrm{Zn}^{2+}(1 \mathrm{M})+\mathrm{Cu}(\mathrm{s})$
taking place in a cell, $\mathrm{E}_{\text {cell }}^{\circ}$ is $1.10 \mathrm{~V} \mathrm{E}_{\text {cell }}$ for the cell will be $\left(2 \cdot 303 \frac{\mathrm{RT}}{\mathrm{F}}=0.0591\right)$
275972
What is the electrode potential (in $V$ ) of the following electrode at $25^{\circ} \mathrm{C}$ ?
$\mathrm{Ni}^{2+}(0.1 \mathrm{M}) \mid \mathrm{Ni}(\mathrm{s})$
(Standard reduction potential of $\mathrm{Ni}^{2+} \mid \mathrm{Ni}$ is)
$-0.25 \mathrm{~V}, \frac{2.303 \mathrm{RT}}{\mathrm{F}}=0.06$
275975 Two electrochemical cell $\mathrm{Fe}\left \vert\mathrm{Fe}^{2+} \ \vert \mathrm{Cu}^{2+}\right \vert \mathrm{Cu}$ and $\mathrm{Zn}\left \vert\mathrm{Zn}^{2+} \ \vert \mathrm{Cu}^{2+}\right \vert \mathrm{Cu}$ are connected in series. $\left(\mathrm{Fe}^{2+} / \mathrm{Fe}=-0.41 \mathrm{~V}, \mathrm{Zn}^{2+} / \mathrm{Zn}=-0.076 \mathrm{~V}, \mathrm{Cu}^{2+} /\right.$ $\mathrm{Cu}=+0.34 \mathrm{~V})$. The net emf of this cell is
275976
For the redox reaction
$\mathrm{Zn}(\mathrm{s})+\mathrm{Cu}^{2+}(0.1 \mathrm{M}) \rightarrow \mathrm{Zn}^{2+}(1 \mathrm{M})+\mathrm{Cu}(\mathrm{s})$
taking place in a cell, $\mathrm{E}_{\text {cell }}^{\circ}$ is $1.10 \mathrm{~V} \mathrm{E}_{\text {cell }}$ for the cell will be $\left(2 \cdot 303 \frac{\mathrm{RT}}{\mathrm{F}}=0.0591\right)$
275972
What is the electrode potential (in $V$ ) of the following electrode at $25^{\circ} \mathrm{C}$ ?
$\mathrm{Ni}^{2+}(0.1 \mathrm{M}) \mid \mathrm{Ni}(\mathrm{s})$
(Standard reduction potential of $\mathrm{Ni}^{2+} \mid \mathrm{Ni}$ is)
$-0.25 \mathrm{~V}, \frac{2.303 \mathrm{RT}}{\mathrm{F}}=0.06$
275975 Two electrochemical cell $\mathrm{Fe}\left \vert\mathrm{Fe}^{2+} \ \vert \mathrm{Cu}^{2+}\right \vert \mathrm{Cu}$ and $\mathrm{Zn}\left \vert\mathrm{Zn}^{2+} \ \vert \mathrm{Cu}^{2+}\right \vert \mathrm{Cu}$ are connected in series. $\left(\mathrm{Fe}^{2+} / \mathrm{Fe}=-0.41 \mathrm{~V}, \mathrm{Zn}^{2+} / \mathrm{Zn}=-0.076 \mathrm{~V}, \mathrm{Cu}^{2+} /\right.$ $\mathrm{Cu}=+0.34 \mathrm{~V})$. The net emf of this cell is
275976
For the redox reaction
$\mathrm{Zn}(\mathrm{s})+\mathrm{Cu}^{2+}(0.1 \mathrm{M}) \rightarrow \mathrm{Zn}^{2+}(1 \mathrm{M})+\mathrm{Cu}(\mathrm{s})$
taking place in a cell, $\mathrm{E}_{\text {cell }}^{\circ}$ is $1.10 \mathrm{~V} \mathrm{E}_{\text {cell }}$ for the cell will be $\left(2 \cdot 303 \frac{\mathrm{RT}}{\mathrm{F}}=0.0591\right)$