02. Cell Constant
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ELECTROCHEMISTRY

276121 The products formed when an aqueous solution of $\mathrm{NaBr}$ is electrolysed in a cell having inert electrode are :

1 $\mathrm{Na}$ and $\mathrm{Br}_{2}$
2 $\mathrm{Na}$ and $\mathrm{O}_{2}$
3 $\mathrm{H}_{2} \mathrm{Br}_{2}$ and $\mathrm{NaOH}$
4 $\mathrm{H}_{2}$ and $\mathrm{O}_{2}$
AIIMS-2006
ELECTROCHEMISTRY

276103 The standard Gibbs energy for the given cell reaction in $\mathrm{kJ} \mathrm{mol}^{-1}$ at $298 \mathrm{~K}$ is
$\mathrm{Zn}(\mathrm{s})+\mathrm{Cu}^{2+}(\mathrm{aq}) \rightarrow \mathrm{Zn}^{2+}(\mathrm{aq})$
$+\mathrm{Cu}(\mathrm{s}), \mathrm{E}^{0}=2 \mathrm{~V}$ at $298 \mathrm{~K}$

1 384
2 192
3 -384
4 -192
JEE Main-2019
ELECTROCHEMISTRY

276106 According to the expression $\Delta G^{\mathbf{0}}=-\mathbf{n F E}^{\mathbf{0}}$, the cell reaction is spontaneous when (Notations and symbols carry their usual meanings)

1 $\Delta \mathrm{G}^{\circ}$ is positive
2 $\Delta \mathrm{G}^{\circ}$ is zero
3 $\mathrm{E}^{\mathrm{o}}$ is negative
4 $\mathrm{E}^{\mathrm{o}}$ is positive
J and K CET-(2017)
ELECTROCHEMISTRY

276109 Which among the following solutions is not used in determination of the cell constant?

1 $10^{-2} \mathrm{M} \mathrm{KCl}$
2 $10^{-1} \mathrm{M} \mathrm{KCl}$
3 $1 \mathrm{M} \mathrm{KCl}$
4 Saturated $\mathrm{KCl}$
MHT CET-2015
For More Updates join with Us
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ELECTROCHEMISTRY

276121 The products formed when an aqueous solution of $\mathrm{NaBr}$ is electrolysed in a cell having inert electrode are :

1 $\mathrm{Na}$ and $\mathrm{Br}_{2}$
2 $\mathrm{Na}$ and $\mathrm{O}_{2}$
3 $\mathrm{H}_{2} \mathrm{Br}_{2}$ and $\mathrm{NaOH}$
4 $\mathrm{H}_{2}$ and $\mathrm{O}_{2}$
AIIMS-2006
ELECTROCHEMISTRY

276103 The standard Gibbs energy for the given cell reaction in $\mathrm{kJ} \mathrm{mol}^{-1}$ at $298 \mathrm{~K}$ is
$\mathrm{Zn}(\mathrm{s})+\mathrm{Cu}^{2+}(\mathrm{aq}) \rightarrow \mathrm{Zn}^{2+}(\mathrm{aq})$
$+\mathrm{Cu}(\mathrm{s}), \mathrm{E}^{0}=2 \mathrm{~V}$ at $298 \mathrm{~K}$

1 384
2 192
3 -384
4 -192
JEE Main-2019
ELECTROCHEMISTRY

276106 According to the expression $\Delta G^{\mathbf{0}}=-\mathbf{n F E}^{\mathbf{0}}$, the cell reaction is spontaneous when (Notations and symbols carry their usual meanings)

1 $\Delta \mathrm{G}^{\circ}$ is positive
2 $\Delta \mathrm{G}^{\circ}$ is zero
3 $\mathrm{E}^{\mathrm{o}}$ is negative
4 $\mathrm{E}^{\mathrm{o}}$ is positive
J and K CET-(2017)
ELECTROCHEMISTRY

276109 Which among the following solutions is not used in determination of the cell constant?

1 $10^{-2} \mathrm{M} \mathrm{KCl}$
2 $10^{-1} \mathrm{M} \mathrm{KCl}$
3 $1 \mathrm{M} \mathrm{KCl}$
4 Saturated $\mathrm{KCl}$
MHT CET-2015
NEET DIGITAL LIBRARY
ELECTROCHEMISTRY

276121 The products formed when an aqueous solution of $\mathrm{NaBr}$ is electrolysed in a cell having inert electrode are :

1 $\mathrm{Na}$ and $\mathrm{Br}_{2}$
2 $\mathrm{Na}$ and $\mathrm{O}_{2}$
3 $\mathrm{H}_{2} \mathrm{Br}_{2}$ and $\mathrm{NaOH}$
4 $\mathrm{H}_{2}$ and $\mathrm{O}_{2}$
AIIMS-2006
ELECTROCHEMISTRY

276103 The standard Gibbs energy for the given cell reaction in $\mathrm{kJ} \mathrm{mol}^{-1}$ at $298 \mathrm{~K}$ is
$\mathrm{Zn}(\mathrm{s})+\mathrm{Cu}^{2+}(\mathrm{aq}) \rightarrow \mathrm{Zn}^{2+}(\mathrm{aq})$
$+\mathrm{Cu}(\mathrm{s}), \mathrm{E}^{0}=2 \mathrm{~V}$ at $298 \mathrm{~K}$

1 384
2 192
3 -384
4 -192
JEE Main-2019
ELECTROCHEMISTRY

276106 According to the expression $\Delta G^{\mathbf{0}}=-\mathbf{n F E}^{\mathbf{0}}$, the cell reaction is spontaneous when (Notations and symbols carry their usual meanings)

1 $\Delta \mathrm{G}^{\circ}$ is positive
2 $\Delta \mathrm{G}^{\circ}$ is zero
3 $\mathrm{E}^{\mathrm{o}}$ is negative
4 $\mathrm{E}^{\mathrm{o}}$ is positive
J and K CET-(2017)
ELECTROCHEMISTRY

276109 Which among the following solutions is not used in determination of the cell constant?

1 $10^{-2} \mathrm{M} \mathrm{KCl}$
2 $10^{-1} \mathrm{M} \mathrm{KCl}$
3 $1 \mathrm{M} \mathrm{KCl}$
4 Saturated $\mathrm{KCl}$
MHT CET-2015
Join With Us for More Updates
ELECTROCHEMISTRY

276121 The products formed when an aqueous solution of $\mathrm{NaBr}$ is electrolysed in a cell having inert electrode are :

1 $\mathrm{Na}$ and $\mathrm{Br}_{2}$
2 $\mathrm{Na}$ and $\mathrm{O}_{2}$
3 $\mathrm{H}_{2} \mathrm{Br}_{2}$ and $\mathrm{NaOH}$
4 $\mathrm{H}_{2}$ and $\mathrm{O}_{2}$
AIIMS-2006
ELECTROCHEMISTRY

276103 The standard Gibbs energy for the given cell reaction in $\mathrm{kJ} \mathrm{mol}^{-1}$ at $298 \mathrm{~K}$ is
$\mathrm{Zn}(\mathrm{s})+\mathrm{Cu}^{2+}(\mathrm{aq}) \rightarrow \mathrm{Zn}^{2+}(\mathrm{aq})$
$+\mathrm{Cu}(\mathrm{s}), \mathrm{E}^{0}=2 \mathrm{~V}$ at $298 \mathrm{~K}$

1 384
2 192
3 -384
4 -192
JEE Main-2019
ELECTROCHEMISTRY

276106 According to the expression $\Delta G^{\mathbf{0}}=-\mathbf{n F E}^{\mathbf{0}}$, the cell reaction is spontaneous when (Notations and symbols carry their usual meanings)

1 $\Delta \mathrm{G}^{\circ}$ is positive
2 $\Delta \mathrm{G}^{\circ}$ is zero
3 $\mathrm{E}^{\mathrm{o}}$ is negative
4 $\mathrm{E}^{\mathrm{o}}$ is positive
J and K CET-(2017)
ELECTROCHEMISTRY

276109 Which among the following solutions is not used in determination of the cell constant?

1 $10^{-2} \mathrm{M} \mathrm{KCl}$
2 $10^{-1} \mathrm{M} \mathrm{KCl}$
3 $1 \mathrm{M} \mathrm{KCl}$
4 Saturated $\mathrm{KCl}$
MHT CET-2015
For More Updates join with Us