275761 Given ${\mathrm{E}}_{{\mathrm{Mn}}^{7+}/{\mathrm{Mn}}^{2+}}^0=1.51\mathrm{V},{\mathrm{E}}^{\mathbf{0}}{}_{{\mathrm{nn}}^{4+}/{\mathrm{Mn}}^{2+}}=1.23\mathrm{V}$
Calculate the ${\mathbf{E}}^{\mathbf{0}}{\mathrm{Mn}}^{{\mathbf{n}}^{+}/{\mathbf{M}\mathbf{n}}^{4+}}$

275764 The standard reduction potentials for ${\mathrm{Zn}}^{2+}/\mathrm{Zn}$, ${\mathrm{Ni}}^{2+}/\mathrm{Ni}$ and ${\mathrm{Fe}}^{2+}/\mathrm{Fe}$ are $-0.76,-0.23$ and -0.44 $\mathrm{V}$, respectively. The reaction $\mathrm{X}+{\mathrm{Y}}^{2+}\to {\mathrm{X}}^{2+}+\mathrm{Y}$ will be spontaneous when

275765 During the electrolysis of copper sulphate aqueous solution using copper electrode, the reaction taking place at the cathode is

275761 Given ${\mathrm{E}}_{{\mathrm{Mn}}^{7+}/{\mathrm{Mn}}^{2+}}^0=1.51\mathrm{V},{\mathrm{E}}^{\mathbf{0}}{}_{{\mathrm{nn}}^{4+}/{\mathrm{Mn}}^{2+}}=1.23\mathrm{V}$
Calculate the ${\mathbf{E}}^{\mathbf{0}}{\mathrm{Mn}}^{{\mathbf{n}}^{+}/{\mathbf{M}\mathbf{n}}^{4+}}$

275762 The cell potential, $E_{\text{cell }}$ the following cell notation (in Volts) is
$\begin{array}{rl}& \mathrm{A}(\mathrm{s})\mid {\mathrm{A}}^{+}(\mathrm{aq},0.1\mathrm{M}|{\mathrm{B}}^{2+}(\mathrm{aq},0.01\mathrm{M})\mid \mathrm{B}(\mathrm{s})\\ & {\mathrm{E}}_{{\mathrm{A}}^{+}/\mathrm{A}}^0=\mathbf{1}\mathbf{V}\text{ and }{\mathrm{E}}_{{\mathrm{B}}^{2+}\mathrm{B}}^0=3\mathrm{V}\end{array}$

275764 The standard reduction potentials for ${\mathrm{Zn}}^{2+}/\mathrm{Zn}$, ${\mathrm{Ni}}^{2+}/\mathrm{Ni}$ and ${\mathrm{Fe}}^{2+}/\mathrm{Fe}$ are $-0.76,-0.23$ and -0.44 $\mathrm{V}$, respectively. The reaction $\mathrm{X}+{\mathrm{Y}}^{2+}\to {\mathrm{X}}^{2+}+\mathrm{Y}$ will be spontaneous when

275765 During the electrolysis of copper sulphate aqueous solution using copper electrode, the reaction taking place at the cathode is

275761 Given ${\mathrm{E}}_{{\mathrm{Mn}}^{7+}/{\mathrm{Mn}}^{2+}}^0=1.51\mathrm{V},{\mathrm{E}}^{\mathbf{0}}{}_{{\mathrm{nn}}^{4+}/{\mathrm{Mn}}^{2+}}=1.23\mathrm{V}$
Calculate the ${\mathbf{E}}^{\mathbf{0}}{\mathrm{Mn}}^{{\mathbf{n}}^{+}/{\mathbf{M}\mathbf{n}}^{4+}}$

275762 The cell potential, $E_{\text{cell }}$ the following cell notation (in Volts) is
$\begin{array}{rl}& \mathrm{A}(\mathrm{s})\mid {\mathrm{A}}^{+}(\mathrm{aq},0.1\mathrm{M}|{\mathrm{B}}^{2+}(\mathrm{aq},0.01\mathrm{M})\mid \mathrm{B}(\mathrm{s})\\ & {\mathrm{E}}_{{\mathrm{A}}^{+}/\mathrm{A}}^0=\mathbf{1}\mathbf{V}\text{ and }{\mathrm{E}}_{{\mathrm{B}}^{2+}\mathrm{B}}^0=3\mathrm{V}\end{array}$

275764 The standard reduction potentials for ${\mathrm{Zn}}^{2+}/\mathrm{Zn}$, ${\mathrm{Ni}}^{2+}/\mathrm{Ni}$ and ${\mathrm{Fe}}^{2+}/\mathrm{Fe}$ are $-0.76,-0.23$ and -0.44 $\mathrm{V}$, respectively. The reaction $\mathrm{X}+{\mathrm{Y}}^{2+}\to {\mathrm{X}}^{2+}+\mathrm{Y}$ will be spontaneous when

275765 During the electrolysis of copper sulphate aqueous solution using copper electrode, the reaction taking place at the cathode is

275761 Given ${\mathrm{E}}_{{\mathrm{Mn}}^{7+}/{\mathrm{Mn}}^{2+}}^0=1.51\mathrm{V},{\mathrm{E}}^{\mathbf{0}}{}_{{\mathrm{nn}}^{4+}/{\mathrm{Mn}}^{2+}}=1.23\mathrm{V}$
Calculate the ${\mathbf{E}}^{\mathbf{0}}{\mathrm{Mn}}^{{\mathbf{n}}^{+}/{\mathbf{M}\mathbf{n}}^{4+}}$

275762 The cell potential, $E_{\text{cell }}$ the following cell notation (in Volts) is
$\begin{array}{rl}& \mathrm{A}(\mathrm{s})\mid {\mathrm{A}}^{+}(\mathrm{aq},0.1\mathrm{M}|{\mathrm{B}}^{2+}(\mathrm{aq},0.01\mathrm{M})\mid \mathrm{B}(\mathrm{s})\\ & {\mathrm{E}}_{{\mathrm{A}}^{+}/\mathrm{A}}^0=\mathbf{1}\mathbf{V}\text{ and }{\mathrm{E}}_{{\mathrm{B}}^{2+}\mathrm{B}}^0=3\mathrm{V}\end{array}$

275764 The standard reduction potentials for ${\mathrm{Zn}}^{2+}/\mathrm{Zn}$, ${\mathrm{Ni}}^{2+}/\mathrm{Ni}$ and ${\mathrm{Fe}}^{2+}/\mathrm{Fe}$ are $-0.76,-0.23$ and -0.44 $\mathrm{V}$, respectively. The reaction $\mathrm{X}+{\mathrm{Y}}^{2+}\to {\mathrm{X}}^{2+}+\mathrm{Y}$ will be spontaneous when

275765 During the electrolysis of copper sulphate aqueous solution using copper electrode, the reaction taking place at the cathode is