00. Electrode Potential
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NEET DIGITAL LIBRARY
ELECTROCHEMISTRY

275915 Standard electrode potentials of three metals $X, Y$ and $Z$ are $-1.2 \mathrm{~V},+0.5 \mathrm{~V}$ and $-3.0 \mathrm{~V}$ respectively. The reducing power of these metals will be

1 $Y>Z>X$
2 Y $>X>Z$
3 $Z>X>Y$
4 $\mathrm{X}>\mathrm{Y}>\mathrm{Z}$
(AIPMT -2011)
ELECTROCHEMISTRY

275918 Given $\mathrm{E}_{\mathrm{k}^{+} / \mathrm{k}}=-2.93 \mathrm{~V}$;
$\begin{aligned}
& \mathrm{E}_{\mathrm{Fe}^{2+} / \mathrm{Fe}}^{\mathrm{o}}=-0.44 \mathrm{~V} ; \mathrm{E}_{\mathrm{Zn}^{2+/ \mathrm{Zn}}}^{\mathrm{o}}=-0.76 \mathrm{~V} ; \\
& \mathrm{E}_{\mathrm{Cu}^{2+} / \mathrm{Cu}}^{\mathrm{o}}=0.34 \mathrm{~V}
\end{aligned}$
Based on this data, which of the following is the strongest reducing agent?

1 $\mathrm{Cu}_{(\mathrm{s})}$
2 $\mathrm{K}_{\text {(aq) }}^{+}$
3 $\mathrm{Zn}_{\text {(aq) }}^{2+}$
4 $\mathrm{Fe}_{(\mathrm{s})}$
AIIMS-2011
ELECTROCHEMISTRY

275923 Which one the following will increase the voltage of the cell? $(T=298 \mathrm{~K})$
$\mathrm{Sn}(\mathrm{s})+2 \mathrm{Ag}^{+}(\mathrm{aq}) \rightarrow \mathrm{Sn}^{2+}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s})$

1 Increase in the size of silver rod
2 Increasing the size of plate
3 Increase in the concentration of $\mathrm{Ag}^{+}$ions
4 Increase in the concentration of $\mathrm{Sn}^{2+}$ ions
JCECE - 2011
ELECTROCHEMISTRY

275927 Consider the following relations for emf of an electrochemical cell
(i) EMF of cell $=($ Oxidation potential of anode $)$ - (Reduction potential of cathode)
(ii) EMF of cell $=($ Oxidation potential of anode $)$ + (Reduction potential of cathode)
(iii) EMF of cell $=($ Reduction potential of anode $)$ + (Reduction potential of cathode)
(iv) EMF of cell $=($ Oxidation potential of anode $)$ - (Oxidation potential of cathode)
Which of the above relations are correct?

1 (iii) and (i)
2 (i) and (ii)
3 (iii) and (iv)
4 (ii) and (iv)
(AIPMT -Mains - 2010)
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ELECTROCHEMISTRY

275915 Standard electrode potentials of three metals $X, Y$ and $Z$ are $-1.2 \mathrm{~V},+0.5 \mathrm{~V}$ and $-3.0 \mathrm{~V}$ respectively. The reducing power of these metals will be

1 $Y>Z>X$
2 Y $>X>Z$
3 $Z>X>Y$
4 $\mathrm{X}>\mathrm{Y}>\mathrm{Z}$
(AIPMT -2011)
ELECTROCHEMISTRY

275918 Given $\mathrm{E}_{\mathrm{k}^{+} / \mathrm{k}}=-2.93 \mathrm{~V}$;
$\begin{aligned}
& \mathrm{E}_{\mathrm{Fe}^{2+} / \mathrm{Fe}}^{\mathrm{o}}=-0.44 \mathrm{~V} ; \mathrm{E}_{\mathrm{Zn}^{2+/ \mathrm{Zn}}}^{\mathrm{o}}=-0.76 \mathrm{~V} ; \\
& \mathrm{E}_{\mathrm{Cu}^{2+} / \mathrm{Cu}}^{\mathrm{o}}=0.34 \mathrm{~V}
\end{aligned}$
Based on this data, which of the following is the strongest reducing agent?

1 $\mathrm{Cu}_{(\mathrm{s})}$
2 $\mathrm{K}_{\text {(aq) }}^{+}$
3 $\mathrm{Zn}_{\text {(aq) }}^{2+}$
4 $\mathrm{Fe}_{(\mathrm{s})}$
AIIMS-2011
ELECTROCHEMISTRY

275923 Which one the following will increase the voltage of the cell? $(T=298 \mathrm{~K})$
$\mathrm{Sn}(\mathrm{s})+2 \mathrm{Ag}^{+}(\mathrm{aq}) \rightarrow \mathrm{Sn}^{2+}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s})$

1 Increase in the size of silver rod
2 Increasing the size of plate
3 Increase in the concentration of $\mathrm{Ag}^{+}$ions
4 Increase in the concentration of $\mathrm{Sn}^{2+}$ ions
JCECE - 2011
ELECTROCHEMISTRY

275927 Consider the following relations for emf of an electrochemical cell
(i) EMF of cell $=($ Oxidation potential of anode $)$ - (Reduction potential of cathode)
(ii) EMF of cell $=($ Oxidation potential of anode $)$ + (Reduction potential of cathode)
(iii) EMF of cell $=($ Reduction potential of anode $)$ + (Reduction potential of cathode)
(iv) EMF of cell $=($ Oxidation potential of anode $)$ - (Oxidation potential of cathode)
Which of the above relations are correct?

1 (iii) and (i)
2 (i) and (ii)
3 (iii) and (iv)
4 (ii) and (iv)
(AIPMT -Mains - 2010)
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ELECTROCHEMISTRY

275915 Standard electrode potentials of three metals $X, Y$ and $Z$ are $-1.2 \mathrm{~V},+0.5 \mathrm{~V}$ and $-3.0 \mathrm{~V}$ respectively. The reducing power of these metals will be

1 $Y>Z>X$
2 Y $>X>Z$
3 $Z>X>Y$
4 $\mathrm{X}>\mathrm{Y}>\mathrm{Z}$
(AIPMT -2011)
ELECTROCHEMISTRY

275918 Given $\mathrm{E}_{\mathrm{k}^{+} / \mathrm{k}}=-2.93 \mathrm{~V}$;
$\begin{aligned}
& \mathrm{E}_{\mathrm{Fe}^{2+} / \mathrm{Fe}}^{\mathrm{o}}=-0.44 \mathrm{~V} ; \mathrm{E}_{\mathrm{Zn}^{2+/ \mathrm{Zn}}}^{\mathrm{o}}=-0.76 \mathrm{~V} ; \\
& \mathrm{E}_{\mathrm{Cu}^{2+} / \mathrm{Cu}}^{\mathrm{o}}=0.34 \mathrm{~V}
\end{aligned}$
Based on this data, which of the following is the strongest reducing agent?

1 $\mathrm{Cu}_{(\mathrm{s})}$
2 $\mathrm{K}_{\text {(aq) }}^{+}$
3 $\mathrm{Zn}_{\text {(aq) }}^{2+}$
4 $\mathrm{Fe}_{(\mathrm{s})}$
AIIMS-2011
ELECTROCHEMISTRY

275923 Which one the following will increase the voltage of the cell? $(T=298 \mathrm{~K})$
$\mathrm{Sn}(\mathrm{s})+2 \mathrm{Ag}^{+}(\mathrm{aq}) \rightarrow \mathrm{Sn}^{2+}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s})$

1 Increase in the size of silver rod
2 Increasing the size of plate
3 Increase in the concentration of $\mathrm{Ag}^{+}$ions
4 Increase in the concentration of $\mathrm{Sn}^{2+}$ ions
JCECE - 2011
ELECTROCHEMISTRY

275927 Consider the following relations for emf of an electrochemical cell
(i) EMF of cell $=($ Oxidation potential of anode $)$ - (Reduction potential of cathode)
(ii) EMF of cell $=($ Oxidation potential of anode $)$ + (Reduction potential of cathode)
(iii) EMF of cell $=($ Reduction potential of anode $)$ + (Reduction potential of cathode)
(iv) EMF of cell $=($ Oxidation potential of anode $)$ - (Oxidation potential of cathode)
Which of the above relations are correct?

1 (iii) and (i)
2 (i) and (ii)
3 (iii) and (iv)
4 (ii) and (iv)
(AIPMT -Mains - 2010)
NEET DIGITAL LIBRARY
ELECTROCHEMISTRY

275915 Standard electrode potentials of three metals $X, Y$ and $Z$ are $-1.2 \mathrm{~V},+0.5 \mathrm{~V}$ and $-3.0 \mathrm{~V}$ respectively. The reducing power of these metals will be

1 $Y>Z>X$
2 Y $>X>Z$
3 $Z>X>Y$
4 $\mathrm{X}>\mathrm{Y}>\mathrm{Z}$
(AIPMT -2011)
ELECTROCHEMISTRY

275918 Given $\mathrm{E}_{\mathrm{k}^{+} / \mathrm{k}}=-2.93 \mathrm{~V}$;
$\begin{aligned}
& \mathrm{E}_{\mathrm{Fe}^{2+} / \mathrm{Fe}}^{\mathrm{o}}=-0.44 \mathrm{~V} ; \mathrm{E}_{\mathrm{Zn}^{2+/ \mathrm{Zn}}}^{\mathrm{o}}=-0.76 \mathrm{~V} ; \\
& \mathrm{E}_{\mathrm{Cu}^{2+} / \mathrm{Cu}}^{\mathrm{o}}=0.34 \mathrm{~V}
\end{aligned}$
Based on this data, which of the following is the strongest reducing agent?

1 $\mathrm{Cu}_{(\mathrm{s})}$
2 $\mathrm{K}_{\text {(aq) }}^{+}$
3 $\mathrm{Zn}_{\text {(aq) }}^{2+}$
4 $\mathrm{Fe}_{(\mathrm{s})}$
AIIMS-2011
ELECTROCHEMISTRY

275923 Which one the following will increase the voltage of the cell? $(T=298 \mathrm{~K})$
$\mathrm{Sn}(\mathrm{s})+2 \mathrm{Ag}^{+}(\mathrm{aq}) \rightarrow \mathrm{Sn}^{2+}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s})$

1 Increase in the size of silver rod
2 Increasing the size of plate
3 Increase in the concentration of $\mathrm{Ag}^{+}$ions
4 Increase in the concentration of $\mathrm{Sn}^{2+}$ ions
JCECE - 2011
ELECTROCHEMISTRY

275927 Consider the following relations for emf of an electrochemical cell
(i) EMF of cell $=($ Oxidation potential of anode $)$ - (Reduction potential of cathode)
(ii) EMF of cell $=($ Oxidation potential of anode $)$ + (Reduction potential of cathode)
(iii) EMF of cell $=($ Reduction potential of anode $)$ + (Reduction potential of cathode)
(iv) EMF of cell $=($ Oxidation potential of anode $)$ - (Oxidation potential of cathode)
Which of the above relations are correct?

1 (iii) and (i)
2 (i) and (ii)
3 (iii) and (iv)
4 (ii) and (iv)
(AIPMT -Mains - 2010)
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