276252
In the lead-acid battery during charging, the cathode reaction is
1 formation of $\mathrm{PbO}_{2}$
2 formation of $\mathrm{PbSO}_{4}$
3 reduction of $\mathrm{Pb}^{2+}$ to $\mathrm{Pb}$
4 decomposition of $\mathrm{Pb}$ at the anode.
Explanation:
During charging of lead-acid battery $\mathrm{Pb}^{2+}$ ions of $\mathrm{PbSO}_{4}$ are reduced to $\mathrm{Pb}$ on cathode. At Anode $\mathrm{PbSO}_{4}(\mathrm{~s})+2 \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{PbO}_{2}(\mathrm{~s})+\mathrm{SO}_{4}^{2-}(\mathrm{aq})+4 \mathrm{H}^{+}(\mathrm{aq})+2 \mathrm{e}^{-}$ At Cathode $\mathrm{PbSO}_{4}(\mathrm{~s})+2 \mathrm{e}^{-} \rightarrow \mathrm{Pb}(\mathrm{s})+\mathrm{SO}_{4}^{2-}(\mathrm{aq})$ Thus, $\mathrm{Pb}^{2+}$ ions of $\mathrm{PbSO}_{4}$ are reduced to $\mathrm{Pb}$ on the cathode while $\mathrm{PbSO}_{4}$ is oxidized to $\mathrm{PbO}_{2}$ at anode.
AMU-2015
ELECTROCHEMISTRY
276257
The electrochemical cell stops working after sometime because :
1 electrode potential of both the electrodes becomes zero
2 electrode potential of both the electrodes becomes equal
3 one of the electrodes is eaten away
4 the cell reaction gets reversed
Explanation:
As we know that, $\Delta \mathrm{E}_{\text {cell }}=\mathrm{E}_{\text {cathode }}-\mathrm{E}_{\text {anode }}$ when $\mathrm{E}_{\text {cathode }}=\mathrm{E}_{\text {anode }}$ $\Delta \mathrm{E}_{\text {cell }}=0$ If $\Delta \mathrm{E}_{\text {cell }}=0$ When electrode potential of both the electrodes becomes equal then the electrochemical cell stops working after sometime.
VITEEE- 2008
ELECTROCHEMISTRY
276258
The extent of charge of lead accumulator is determined by
1 amount of $\mathrm{PbSO}_{4}$ in the battery
2 amount of $\mathrm{PbO}_{2}$ in the battery
3 specific gravity of $\mathrm{H}_{2} \mathrm{SO}_{4}$ of the battery
4 amount of $\mathrm{Pb}$ in the battery
Explanation:
The lead accumulator refers to a secondary cell as the electrical energy does not generate itself inside the cell, but it is stored prior to an external source. The extent of charge of a lead accumulator is determined by the specific gravity of $\mathrm{H}_{2} \mathrm{SO}_{4}$ of the battery. $\begin{gathered} \mathrm{Pb}(\mathrm{s})+\mathrm{PbO}_{2}(\mathrm{~s})+4 \mathrm{H}^{+}(\mathrm{aq})+2 \mathrm{SO}_{4}{ }^{2-}(\mathrm{aq}) \longrightarrow \\ 2 \mathrm{PbSO}_{4}(\mathrm{l})+2 \mathrm{H}_{2} \mathrm{O} \end{gathered}$ The fully charged lead accumulator is $1.30 \mathrm{~g} / \mathrm{ml}$ and when it drops below $1.20 \mathrm{~g} / \mathrm{ml}$, the lead accumulator need recharging.
AP-EAMCET (Engg.) 2013
ELECTROCHEMISTRY
276262
Other things being equal, the EMF of a Daniel cell may be increased by
1 keeping low temperature
2 using large copper electrodes
3 using large zinc electrodes
4 decreasing concentration of $\mathrm{Cu}^{2+}$ ions
Explanation:
For Daniel cell $\mathrm{Zn}+\mathrm{Cu}^{2+} \rightarrow \mathrm{Zn}^{2+}+\mathrm{Cu}$ $\mathrm{E}_{\text {cell }}=\mathrm{E}_{\text {cell }}^{\mathrm{o}}-\frac{\mathrm{RT}}{\mathrm{nF}} \ln \frac{\left[\mathrm{Zn}^{2+}\right]}{\left[\mathrm{Cu}^{2+}\right]}$ The decrease in temperature and increase in $\left[\mathrm{Cu}^{2+}\right]$ will increase the EMF. Thus, low temperature will increases EMF of Daniel cell.
BCECE-2011
ELECTROCHEMISTRY
276264
In a Daniell cell constructed in the laboratory, the voltage observed was $0.9 \mathrm{~V}$ instead of $1.1 \mathrm{~V}$ of the standard cell. A possible explanation is-
276252
In the lead-acid battery during charging, the cathode reaction is
1 formation of $\mathrm{PbO}_{2}$
2 formation of $\mathrm{PbSO}_{4}$
3 reduction of $\mathrm{Pb}^{2+}$ to $\mathrm{Pb}$
4 decomposition of $\mathrm{Pb}$ at the anode.
Explanation:
During charging of lead-acid battery $\mathrm{Pb}^{2+}$ ions of $\mathrm{PbSO}_{4}$ are reduced to $\mathrm{Pb}$ on cathode. At Anode $\mathrm{PbSO}_{4}(\mathrm{~s})+2 \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{PbO}_{2}(\mathrm{~s})+\mathrm{SO}_{4}^{2-}(\mathrm{aq})+4 \mathrm{H}^{+}(\mathrm{aq})+2 \mathrm{e}^{-}$ At Cathode $\mathrm{PbSO}_{4}(\mathrm{~s})+2 \mathrm{e}^{-} \rightarrow \mathrm{Pb}(\mathrm{s})+\mathrm{SO}_{4}^{2-}(\mathrm{aq})$ Thus, $\mathrm{Pb}^{2+}$ ions of $\mathrm{PbSO}_{4}$ are reduced to $\mathrm{Pb}$ on the cathode while $\mathrm{PbSO}_{4}$ is oxidized to $\mathrm{PbO}_{2}$ at anode.
AMU-2015
ELECTROCHEMISTRY
276257
The electrochemical cell stops working after sometime because :
1 electrode potential of both the electrodes becomes zero
2 electrode potential of both the electrodes becomes equal
3 one of the electrodes is eaten away
4 the cell reaction gets reversed
Explanation:
As we know that, $\Delta \mathrm{E}_{\text {cell }}=\mathrm{E}_{\text {cathode }}-\mathrm{E}_{\text {anode }}$ when $\mathrm{E}_{\text {cathode }}=\mathrm{E}_{\text {anode }}$ $\Delta \mathrm{E}_{\text {cell }}=0$ If $\Delta \mathrm{E}_{\text {cell }}=0$ When electrode potential of both the electrodes becomes equal then the electrochemical cell stops working after sometime.
VITEEE- 2008
ELECTROCHEMISTRY
276258
The extent of charge of lead accumulator is determined by
1 amount of $\mathrm{PbSO}_{4}$ in the battery
2 amount of $\mathrm{PbO}_{2}$ in the battery
3 specific gravity of $\mathrm{H}_{2} \mathrm{SO}_{4}$ of the battery
4 amount of $\mathrm{Pb}$ in the battery
Explanation:
The lead accumulator refers to a secondary cell as the electrical energy does not generate itself inside the cell, but it is stored prior to an external source. The extent of charge of a lead accumulator is determined by the specific gravity of $\mathrm{H}_{2} \mathrm{SO}_{4}$ of the battery. $\begin{gathered} \mathrm{Pb}(\mathrm{s})+\mathrm{PbO}_{2}(\mathrm{~s})+4 \mathrm{H}^{+}(\mathrm{aq})+2 \mathrm{SO}_{4}{ }^{2-}(\mathrm{aq}) \longrightarrow \\ 2 \mathrm{PbSO}_{4}(\mathrm{l})+2 \mathrm{H}_{2} \mathrm{O} \end{gathered}$ The fully charged lead accumulator is $1.30 \mathrm{~g} / \mathrm{ml}$ and when it drops below $1.20 \mathrm{~g} / \mathrm{ml}$, the lead accumulator need recharging.
AP-EAMCET (Engg.) 2013
ELECTROCHEMISTRY
276262
Other things being equal, the EMF of a Daniel cell may be increased by
1 keeping low temperature
2 using large copper electrodes
3 using large zinc electrodes
4 decreasing concentration of $\mathrm{Cu}^{2+}$ ions
Explanation:
For Daniel cell $\mathrm{Zn}+\mathrm{Cu}^{2+} \rightarrow \mathrm{Zn}^{2+}+\mathrm{Cu}$ $\mathrm{E}_{\text {cell }}=\mathrm{E}_{\text {cell }}^{\mathrm{o}}-\frac{\mathrm{RT}}{\mathrm{nF}} \ln \frac{\left[\mathrm{Zn}^{2+}\right]}{\left[\mathrm{Cu}^{2+}\right]}$ The decrease in temperature and increase in $\left[\mathrm{Cu}^{2+}\right]$ will increase the EMF. Thus, low temperature will increases EMF of Daniel cell.
BCECE-2011
ELECTROCHEMISTRY
276264
In a Daniell cell constructed in the laboratory, the voltage observed was $0.9 \mathrm{~V}$ instead of $1.1 \mathrm{~V}$ of the standard cell. A possible explanation is-
NEET Test Series from KOTA - 10 Papers In MS WORD
WhatsApp Here
ELECTROCHEMISTRY
276252
In the lead-acid battery during charging, the cathode reaction is
1 formation of $\mathrm{PbO}_{2}$
2 formation of $\mathrm{PbSO}_{4}$
3 reduction of $\mathrm{Pb}^{2+}$ to $\mathrm{Pb}$
4 decomposition of $\mathrm{Pb}$ at the anode.
Explanation:
During charging of lead-acid battery $\mathrm{Pb}^{2+}$ ions of $\mathrm{PbSO}_{4}$ are reduced to $\mathrm{Pb}$ on cathode. At Anode $\mathrm{PbSO}_{4}(\mathrm{~s})+2 \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{PbO}_{2}(\mathrm{~s})+\mathrm{SO}_{4}^{2-}(\mathrm{aq})+4 \mathrm{H}^{+}(\mathrm{aq})+2 \mathrm{e}^{-}$ At Cathode $\mathrm{PbSO}_{4}(\mathrm{~s})+2 \mathrm{e}^{-} \rightarrow \mathrm{Pb}(\mathrm{s})+\mathrm{SO}_{4}^{2-}(\mathrm{aq})$ Thus, $\mathrm{Pb}^{2+}$ ions of $\mathrm{PbSO}_{4}$ are reduced to $\mathrm{Pb}$ on the cathode while $\mathrm{PbSO}_{4}$ is oxidized to $\mathrm{PbO}_{2}$ at anode.
AMU-2015
ELECTROCHEMISTRY
276257
The electrochemical cell stops working after sometime because :
1 electrode potential of both the electrodes becomes zero
2 electrode potential of both the electrodes becomes equal
3 one of the electrodes is eaten away
4 the cell reaction gets reversed
Explanation:
As we know that, $\Delta \mathrm{E}_{\text {cell }}=\mathrm{E}_{\text {cathode }}-\mathrm{E}_{\text {anode }}$ when $\mathrm{E}_{\text {cathode }}=\mathrm{E}_{\text {anode }}$ $\Delta \mathrm{E}_{\text {cell }}=0$ If $\Delta \mathrm{E}_{\text {cell }}=0$ When electrode potential of both the electrodes becomes equal then the electrochemical cell stops working after sometime.
VITEEE- 2008
ELECTROCHEMISTRY
276258
The extent of charge of lead accumulator is determined by
1 amount of $\mathrm{PbSO}_{4}$ in the battery
2 amount of $\mathrm{PbO}_{2}$ in the battery
3 specific gravity of $\mathrm{H}_{2} \mathrm{SO}_{4}$ of the battery
4 amount of $\mathrm{Pb}$ in the battery
Explanation:
The lead accumulator refers to a secondary cell as the electrical energy does not generate itself inside the cell, but it is stored prior to an external source. The extent of charge of a lead accumulator is determined by the specific gravity of $\mathrm{H}_{2} \mathrm{SO}_{4}$ of the battery. $\begin{gathered} \mathrm{Pb}(\mathrm{s})+\mathrm{PbO}_{2}(\mathrm{~s})+4 \mathrm{H}^{+}(\mathrm{aq})+2 \mathrm{SO}_{4}{ }^{2-}(\mathrm{aq}) \longrightarrow \\ 2 \mathrm{PbSO}_{4}(\mathrm{l})+2 \mathrm{H}_{2} \mathrm{O} \end{gathered}$ The fully charged lead accumulator is $1.30 \mathrm{~g} / \mathrm{ml}$ and when it drops below $1.20 \mathrm{~g} / \mathrm{ml}$, the lead accumulator need recharging.
AP-EAMCET (Engg.) 2013
ELECTROCHEMISTRY
276262
Other things being equal, the EMF of a Daniel cell may be increased by
1 keeping low temperature
2 using large copper electrodes
3 using large zinc electrodes
4 decreasing concentration of $\mathrm{Cu}^{2+}$ ions
Explanation:
For Daniel cell $\mathrm{Zn}+\mathrm{Cu}^{2+} \rightarrow \mathrm{Zn}^{2+}+\mathrm{Cu}$ $\mathrm{E}_{\text {cell }}=\mathrm{E}_{\text {cell }}^{\mathrm{o}}-\frac{\mathrm{RT}}{\mathrm{nF}} \ln \frac{\left[\mathrm{Zn}^{2+}\right]}{\left[\mathrm{Cu}^{2+}\right]}$ The decrease in temperature and increase in $\left[\mathrm{Cu}^{2+}\right]$ will increase the EMF. Thus, low temperature will increases EMF of Daniel cell.
BCECE-2011
ELECTROCHEMISTRY
276264
In a Daniell cell constructed in the laboratory, the voltage observed was $0.9 \mathrm{~V}$ instead of $1.1 \mathrm{~V}$ of the standard cell. A possible explanation is-
276252
In the lead-acid battery during charging, the cathode reaction is
1 formation of $\mathrm{PbO}_{2}$
2 formation of $\mathrm{PbSO}_{4}$
3 reduction of $\mathrm{Pb}^{2+}$ to $\mathrm{Pb}$
4 decomposition of $\mathrm{Pb}$ at the anode.
Explanation:
During charging of lead-acid battery $\mathrm{Pb}^{2+}$ ions of $\mathrm{PbSO}_{4}$ are reduced to $\mathrm{Pb}$ on cathode. At Anode $\mathrm{PbSO}_{4}(\mathrm{~s})+2 \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{PbO}_{2}(\mathrm{~s})+\mathrm{SO}_{4}^{2-}(\mathrm{aq})+4 \mathrm{H}^{+}(\mathrm{aq})+2 \mathrm{e}^{-}$ At Cathode $\mathrm{PbSO}_{4}(\mathrm{~s})+2 \mathrm{e}^{-} \rightarrow \mathrm{Pb}(\mathrm{s})+\mathrm{SO}_{4}^{2-}(\mathrm{aq})$ Thus, $\mathrm{Pb}^{2+}$ ions of $\mathrm{PbSO}_{4}$ are reduced to $\mathrm{Pb}$ on the cathode while $\mathrm{PbSO}_{4}$ is oxidized to $\mathrm{PbO}_{2}$ at anode.
AMU-2015
ELECTROCHEMISTRY
276257
The electrochemical cell stops working after sometime because :
1 electrode potential of both the electrodes becomes zero
2 electrode potential of both the electrodes becomes equal
3 one of the electrodes is eaten away
4 the cell reaction gets reversed
Explanation:
As we know that, $\Delta \mathrm{E}_{\text {cell }}=\mathrm{E}_{\text {cathode }}-\mathrm{E}_{\text {anode }}$ when $\mathrm{E}_{\text {cathode }}=\mathrm{E}_{\text {anode }}$ $\Delta \mathrm{E}_{\text {cell }}=0$ If $\Delta \mathrm{E}_{\text {cell }}=0$ When electrode potential of both the electrodes becomes equal then the electrochemical cell stops working after sometime.
VITEEE- 2008
ELECTROCHEMISTRY
276258
The extent of charge of lead accumulator is determined by
1 amount of $\mathrm{PbSO}_{4}$ in the battery
2 amount of $\mathrm{PbO}_{2}$ in the battery
3 specific gravity of $\mathrm{H}_{2} \mathrm{SO}_{4}$ of the battery
4 amount of $\mathrm{Pb}$ in the battery
Explanation:
The lead accumulator refers to a secondary cell as the electrical energy does not generate itself inside the cell, but it is stored prior to an external source. The extent of charge of a lead accumulator is determined by the specific gravity of $\mathrm{H}_{2} \mathrm{SO}_{4}$ of the battery. $\begin{gathered} \mathrm{Pb}(\mathrm{s})+\mathrm{PbO}_{2}(\mathrm{~s})+4 \mathrm{H}^{+}(\mathrm{aq})+2 \mathrm{SO}_{4}{ }^{2-}(\mathrm{aq}) \longrightarrow \\ 2 \mathrm{PbSO}_{4}(\mathrm{l})+2 \mathrm{H}_{2} \mathrm{O} \end{gathered}$ The fully charged lead accumulator is $1.30 \mathrm{~g} / \mathrm{ml}$ and when it drops below $1.20 \mathrm{~g} / \mathrm{ml}$, the lead accumulator need recharging.
AP-EAMCET (Engg.) 2013
ELECTROCHEMISTRY
276262
Other things being equal, the EMF of a Daniel cell may be increased by
1 keeping low temperature
2 using large copper electrodes
3 using large zinc electrodes
4 decreasing concentration of $\mathrm{Cu}^{2+}$ ions
Explanation:
For Daniel cell $\mathrm{Zn}+\mathrm{Cu}^{2+} \rightarrow \mathrm{Zn}^{2+}+\mathrm{Cu}$ $\mathrm{E}_{\text {cell }}=\mathrm{E}_{\text {cell }}^{\mathrm{o}}-\frac{\mathrm{RT}}{\mathrm{nF}} \ln \frac{\left[\mathrm{Zn}^{2+}\right]}{\left[\mathrm{Cu}^{2+}\right]}$ The decrease in temperature and increase in $\left[\mathrm{Cu}^{2+}\right]$ will increase the EMF. Thus, low temperature will increases EMF of Daniel cell.
BCECE-2011
ELECTROCHEMISTRY
276264
In a Daniell cell constructed in the laboratory, the voltage observed was $0.9 \mathrm{~V}$ instead of $1.1 \mathrm{~V}$ of the standard cell. A possible explanation is-
276252
In the lead-acid battery during charging, the cathode reaction is
1 formation of $\mathrm{PbO}_{2}$
2 formation of $\mathrm{PbSO}_{4}$
3 reduction of $\mathrm{Pb}^{2+}$ to $\mathrm{Pb}$
4 decomposition of $\mathrm{Pb}$ at the anode.
Explanation:
During charging of lead-acid battery $\mathrm{Pb}^{2+}$ ions of $\mathrm{PbSO}_{4}$ are reduced to $\mathrm{Pb}$ on cathode. At Anode $\mathrm{PbSO}_{4}(\mathrm{~s})+2 \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{PbO}_{2}(\mathrm{~s})+\mathrm{SO}_{4}^{2-}(\mathrm{aq})+4 \mathrm{H}^{+}(\mathrm{aq})+2 \mathrm{e}^{-}$ At Cathode $\mathrm{PbSO}_{4}(\mathrm{~s})+2 \mathrm{e}^{-} \rightarrow \mathrm{Pb}(\mathrm{s})+\mathrm{SO}_{4}^{2-}(\mathrm{aq})$ Thus, $\mathrm{Pb}^{2+}$ ions of $\mathrm{PbSO}_{4}$ are reduced to $\mathrm{Pb}$ on the cathode while $\mathrm{PbSO}_{4}$ is oxidized to $\mathrm{PbO}_{2}$ at anode.
AMU-2015
ELECTROCHEMISTRY
276257
The electrochemical cell stops working after sometime because :
1 electrode potential of both the electrodes becomes zero
2 electrode potential of both the electrodes becomes equal
3 one of the electrodes is eaten away
4 the cell reaction gets reversed
Explanation:
As we know that, $\Delta \mathrm{E}_{\text {cell }}=\mathrm{E}_{\text {cathode }}-\mathrm{E}_{\text {anode }}$ when $\mathrm{E}_{\text {cathode }}=\mathrm{E}_{\text {anode }}$ $\Delta \mathrm{E}_{\text {cell }}=0$ If $\Delta \mathrm{E}_{\text {cell }}=0$ When electrode potential of both the electrodes becomes equal then the electrochemical cell stops working after sometime.
VITEEE- 2008
ELECTROCHEMISTRY
276258
The extent of charge of lead accumulator is determined by
1 amount of $\mathrm{PbSO}_{4}$ in the battery
2 amount of $\mathrm{PbO}_{2}$ in the battery
3 specific gravity of $\mathrm{H}_{2} \mathrm{SO}_{4}$ of the battery
4 amount of $\mathrm{Pb}$ in the battery
Explanation:
The lead accumulator refers to a secondary cell as the electrical energy does not generate itself inside the cell, but it is stored prior to an external source. The extent of charge of a lead accumulator is determined by the specific gravity of $\mathrm{H}_{2} \mathrm{SO}_{4}$ of the battery. $\begin{gathered} \mathrm{Pb}(\mathrm{s})+\mathrm{PbO}_{2}(\mathrm{~s})+4 \mathrm{H}^{+}(\mathrm{aq})+2 \mathrm{SO}_{4}{ }^{2-}(\mathrm{aq}) \longrightarrow \\ 2 \mathrm{PbSO}_{4}(\mathrm{l})+2 \mathrm{H}_{2} \mathrm{O} \end{gathered}$ The fully charged lead accumulator is $1.30 \mathrm{~g} / \mathrm{ml}$ and when it drops below $1.20 \mathrm{~g} / \mathrm{ml}$, the lead accumulator need recharging.
AP-EAMCET (Engg.) 2013
ELECTROCHEMISTRY
276262
Other things being equal, the EMF of a Daniel cell may be increased by
1 keeping low temperature
2 using large copper electrodes
3 using large zinc electrodes
4 decreasing concentration of $\mathrm{Cu}^{2+}$ ions
Explanation:
For Daniel cell $\mathrm{Zn}+\mathrm{Cu}^{2+} \rightarrow \mathrm{Zn}^{2+}+\mathrm{Cu}$ $\mathrm{E}_{\text {cell }}=\mathrm{E}_{\text {cell }}^{\mathrm{o}}-\frac{\mathrm{RT}}{\mathrm{nF}} \ln \frac{\left[\mathrm{Zn}^{2+}\right]}{\left[\mathrm{Cu}^{2+}\right]}$ The decrease in temperature and increase in $\left[\mathrm{Cu}^{2+}\right]$ will increase the EMF. Thus, low temperature will increases EMF of Daniel cell.
BCECE-2011
ELECTROCHEMISTRY
276264
In a Daniell cell constructed in the laboratory, the voltage observed was $0.9 \mathrm{~V}$ instead of $1.1 \mathrm{~V}$ of the standard cell. A possible explanation is-