275860 For the cell $\operatorname{Ag}(\mathrm{s})\left \vert\operatorname{Ag}^{+}(\mathrm{aq}) \ \vert \mathrm{Cu}^{2+}(\mathrm{aq})\right \vert \mathrm{Cu}(\mathrm{s})$, the reduction potentials of the left and right hand electrodes are 0.337 and 0.799 volts, the cell e.m.f. is

275861 Given $\mathrm{E}_{\mathrm{Cr}^{3+} / \mathrm{Cr}}^{0}=-0.72 \mathrm{~V}, \mathrm{E}_{\mathrm{Fe}^{2+} / \mathrm{Fe}}^{0}=-0.42 \mathrm{~V}$.
The potential for the cell
$\mathrm{Cr}_{2}\left \vert\mathrm{Cr}^{3+}(0.1 \mathrm{M}) \ \vert \mathrm{Fe}^{2+}(0.01 \mathrm{M})\right \vert \mathrm{Fe}$ is

275862 The $\mathrm{E}_{\mathrm{M}^{3+} / \mathrm{M}^{2+}}^{0}$ values for $\mathrm{Cr}, \mathrm{Mn}, \mathrm{Fe}$ and $\mathrm{Co}$ are $-0.41,+1.57,+0.77$, and $+1.97 \mathrm{~V}$, respectively. For which one of these metals the change in oxidation state from +2 to +3 is easiest?

275863 At temperature of $298 \mathrm{~K}$, the emf of the following electrochemical cell, $\operatorname{Ag}(\mathrm{s})\left \vert\operatorname{Ag}^{+}(0.1 \mathrm{M}) \ \vert \mathrm{Zn}^{2+}\right \vert \mathrm{Zn}(\mathrm{s})(0.1 \mathrm{M})$
Will be (Given, $\mathrm{E}_{\text {cell }}^{0}=-1.562 \mathrm{~V}$ )

275860 For the cell $\operatorname{Ag}(\mathrm{s})\left \vert\operatorname{Ag}^{+}(\mathrm{aq}) \ \vert \mathrm{Cu}^{2+}(\mathrm{aq})\right \vert \mathrm{Cu}(\mathrm{s})$, the reduction potentials of the left and right hand electrodes are 0.337 and 0.799 volts, the cell e.m.f. is

275861 Given $\mathrm{E}_{\mathrm{Cr}^{3+} / \mathrm{Cr}}^{0}=-0.72 \mathrm{~V}, \mathrm{E}_{\mathrm{Fe}^{2+} / \mathrm{Fe}}^{0}=-0.42 \mathrm{~V}$.
The potential for the cell
$\mathrm{Cr}_{2}\left \vert\mathrm{Cr}^{3+}(0.1 \mathrm{M}) \ \vert \mathrm{Fe}^{2+}(0.01 \mathrm{M})\right \vert \mathrm{Fe}$ is

275862 The $\mathrm{E}_{\mathrm{M}^{3+} / \mathrm{M}^{2+}}^{0}$ values for $\mathrm{Cr}, \mathrm{Mn}, \mathrm{Fe}$ and $\mathrm{Co}$ are $-0.41,+1.57,+0.77$, and $+1.97 \mathrm{~V}$, respectively. For which one of these metals the change in oxidation state from +2 to +3 is easiest?

275863 At temperature of $298 \mathrm{~K}$, the emf of the following electrochemical cell, $\operatorname{Ag}(\mathrm{s})\left \vert\operatorname{Ag}^{+}(0.1 \mathrm{M}) \ \vert \mathrm{Zn}^{2+}\right \vert \mathrm{Zn}(\mathrm{s})(0.1 \mathrm{M})$
Will be (Given, $\mathrm{E}_{\text {cell }}^{0}=-1.562 \mathrm{~V}$ )

275860 For the cell $\operatorname{Ag}(\mathrm{s})\left \vert\operatorname{Ag}^{+}(\mathrm{aq}) \ \vert \mathrm{Cu}^{2+}(\mathrm{aq})\right \vert \mathrm{Cu}(\mathrm{s})$, the reduction potentials of the left and right hand electrodes are 0.337 and 0.799 volts, the cell e.m.f. is

275861 Given $\mathrm{E}_{\mathrm{Cr}^{3+} / \mathrm{Cr}}^{0}=-0.72 \mathrm{~V}, \mathrm{E}_{\mathrm{Fe}^{2+} / \mathrm{Fe}}^{0}=-0.42 \mathrm{~V}$.
The potential for the cell
$\mathrm{Cr}_{2}\left \vert\mathrm{Cr}^{3+}(0.1 \mathrm{M}) \ \vert \mathrm{Fe}^{2+}(0.01 \mathrm{M})\right \vert \mathrm{Fe}$ is

275862 The $\mathrm{E}_{\mathrm{M}^{3+} / \mathrm{M}^{2+}}^{0}$ values for $\mathrm{Cr}, \mathrm{Mn}, \mathrm{Fe}$ and $\mathrm{Co}$ are $-0.41,+1.57,+0.77$, and $+1.97 \mathrm{~V}$, respectively. For which one of these metals the change in oxidation state from +2 to +3 is easiest?

275863 At temperature of $298 \mathrm{~K}$, the emf of the following electrochemical cell, $\operatorname{Ag}(\mathrm{s})\left \vert\operatorname{Ag}^{+}(0.1 \mathrm{M}) \ \vert \mathrm{Zn}^{2+}\right \vert \mathrm{Zn}(\mathrm{s})(0.1 \mathrm{M})$
Will be (Given, $\mathrm{E}_{\text {cell }}^{0}=-1.562 \mathrm{~V}$ )

275860 For the cell $\operatorname{Ag}(\mathrm{s})\left \vert\operatorname{Ag}^{+}(\mathrm{aq}) \ \vert \mathrm{Cu}^{2+}(\mathrm{aq})\right \vert \mathrm{Cu}(\mathrm{s})$, the reduction potentials of the left and right hand electrodes are 0.337 and 0.799 volts, the cell e.m.f. is

275861 Given $\mathrm{E}_{\mathrm{Cr}^{3+} / \mathrm{Cr}}^{0}=-0.72 \mathrm{~V}, \mathrm{E}_{\mathrm{Fe}^{2+} / \mathrm{Fe}}^{0}=-0.42 \mathrm{~V}$.
The potential for the cell
$\mathrm{Cr}_{2}\left \vert\mathrm{Cr}^{3+}(0.1 \mathrm{M}) \ \vert \mathrm{Fe}^{2+}(0.01 \mathrm{M})\right \vert \mathrm{Fe}$ is

275862 The $\mathrm{E}_{\mathrm{M}^{3+} / \mathrm{M}^{2+}}^{0}$ values for $\mathrm{Cr}, \mathrm{Mn}, \mathrm{Fe}$ and $\mathrm{Co}$ are $-0.41,+1.57,+0.77$, and $+1.97 \mathrm{~V}$, respectively. For which one of these metals the change in oxidation state from +2 to +3 is easiest?

275863 At temperature of $298 \mathrm{~K}$, the emf of the following electrochemical cell, $\operatorname{Ag}(\mathrm{s})\left \vert\operatorname{Ag}^{+}(0.1 \mathrm{M}) \ \vert \mathrm{Zn}^{2+}\right \vert \mathrm{Zn}(\mathrm{s})(0.1 \mathrm{M})$
Will be (Given, $\mathrm{E}_{\text {cell }}^{0}=-1.562 \mathrm{~V}$ )