00. Electrode Potential
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ELECTROCHEMISTRY

275981 What is the emf of the cell, whose half cells are given below $\mathrm{Mg}^{2+}+2 \mathrm{e}^{-} \rightarrow \operatorname{Mg}(\mathrm{s}) \mathrm{E}=-2.37 \mathrm{~V}$
$\mathrm{Cu}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Cu}(\mathrm{s}) \mathrm{E}=+\mathbf{0 . 3 4} \mathrm{V}$

1 $-2.30 \mathrm{~V}$
2 $1.336 \mathrm{~V}$
3 $2.71 \mathrm{~V}$
4 $2.03 \mathrm{~V}$
CG PET -2005
ELECTROCHEMISTRY

275982 For the feasibility of a redox reaction in a cell, the emf should be

1 positive
2 fixed
3 zero
4 negative
J and K CET-(2005)
ELECTROCHEMISTRY

275992 Which of the following reaction is possible at anode?

1 $\mathrm{Fe}_{2}+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{~F}^{-}$
2 $2 \mathrm{H}^{+}+\frac{1}{2} \mathrm{O}_{2}+2 \mathrm{e}^{-} \rightarrow \mathrm{H}_{2} \mathrm{O}$
3 $2 \mathrm{Cr}_{2}^{3+}+7 \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}+14 \mathrm{H}^{+}+6 \mathrm{e}^{-}$
4 None of the above
VITEEE-2016
ELECTROCHEMISTRY

275950 The standard reduction electrode potentials of the three electrodes $P, Q$ and $R$ are respectively $-1.76 \mathrm{~V}, 0.34 \mathrm{~V}$ and $0.8 \mathrm{~V}$. Then

1 metal $\mathrm{Q}$ will displace the cation of $\mathrm{P}$ from its aqueous solution and deposit the metal $P$
2 both metals $\mathrm{Q}$ and $\mathrm{R}$ will displace the cation of $\mathrm{P}$ from its aqueous solution and deposit the metal $P$
3 metal $\mathrm{R}$ will displace the cation of $\mathrm{P}$ from its aqueous solution and deposit the metal $\mathrm{P}$
4 metal $\mathrm{P}$ will displace the cation of $\mathrm{R}$ from its aqueous solution and deposit the metal R.
J and K CET-(2009)
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ELECTROCHEMISTRY

275981 What is the emf of the cell, whose half cells are given below $\mathrm{Mg}^{2+}+2 \mathrm{e}^{-} \rightarrow \operatorname{Mg}(\mathrm{s}) \mathrm{E}=-2.37 \mathrm{~V}$
$\mathrm{Cu}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Cu}(\mathrm{s}) \mathrm{E}=+\mathbf{0 . 3 4} \mathrm{V}$

1 $-2.30 \mathrm{~V}$
2 $1.336 \mathrm{~V}$
3 $2.71 \mathrm{~V}$
4 $2.03 \mathrm{~V}$
CG PET -2005
ELECTROCHEMISTRY

275982 For the feasibility of a redox reaction in a cell, the emf should be

1 positive
2 fixed
3 zero
4 negative
J and K CET-(2005)
ELECTROCHEMISTRY

275992 Which of the following reaction is possible at anode?

1 $\mathrm{Fe}_{2}+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{~F}^{-}$
2 $2 \mathrm{H}^{+}+\frac{1}{2} \mathrm{O}_{2}+2 \mathrm{e}^{-} \rightarrow \mathrm{H}_{2} \mathrm{O}$
3 $2 \mathrm{Cr}_{2}^{3+}+7 \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}+14 \mathrm{H}^{+}+6 \mathrm{e}^{-}$
4 None of the above
VITEEE-2016
ELECTROCHEMISTRY

275950 The standard reduction electrode potentials of the three electrodes $P, Q$ and $R$ are respectively $-1.76 \mathrm{~V}, 0.34 \mathrm{~V}$ and $0.8 \mathrm{~V}$. Then

1 metal $\mathrm{Q}$ will displace the cation of $\mathrm{P}$ from its aqueous solution and deposit the metal $P$
2 both metals $\mathrm{Q}$ and $\mathrm{R}$ will displace the cation of $\mathrm{P}$ from its aqueous solution and deposit the metal $P$
3 metal $\mathrm{R}$ will displace the cation of $\mathrm{P}$ from its aqueous solution and deposit the metal $\mathrm{P}$
4 metal $\mathrm{P}$ will displace the cation of $\mathrm{R}$ from its aqueous solution and deposit the metal R.
J and K CET-(2009)
NEET DIGITAL LIBRARY
ELECTROCHEMISTRY

275981 What is the emf of the cell, whose half cells are given below $\mathrm{Mg}^{2+}+2 \mathrm{e}^{-} \rightarrow \operatorname{Mg}(\mathrm{s}) \mathrm{E}=-2.37 \mathrm{~V}$
$\mathrm{Cu}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Cu}(\mathrm{s}) \mathrm{E}=+\mathbf{0 . 3 4} \mathrm{V}$

1 $-2.30 \mathrm{~V}$
2 $1.336 \mathrm{~V}$
3 $2.71 \mathrm{~V}$
4 $2.03 \mathrm{~V}$
CG PET -2005
ELECTROCHEMISTRY

275982 For the feasibility of a redox reaction in a cell, the emf should be

1 positive
2 fixed
3 zero
4 negative
J and K CET-(2005)
ELECTROCHEMISTRY

275992 Which of the following reaction is possible at anode?

1 $\mathrm{Fe}_{2}+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{~F}^{-}$
2 $2 \mathrm{H}^{+}+\frac{1}{2} \mathrm{O}_{2}+2 \mathrm{e}^{-} \rightarrow \mathrm{H}_{2} \mathrm{O}$
3 $2 \mathrm{Cr}_{2}^{3+}+7 \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}+14 \mathrm{H}^{+}+6 \mathrm{e}^{-}$
4 None of the above
VITEEE-2016
ELECTROCHEMISTRY

275950 The standard reduction electrode potentials of the three electrodes $P, Q$ and $R$ are respectively $-1.76 \mathrm{~V}, 0.34 \mathrm{~V}$ and $0.8 \mathrm{~V}$. Then

1 metal $\mathrm{Q}$ will displace the cation of $\mathrm{P}$ from its aqueous solution and deposit the metal $P$
2 both metals $\mathrm{Q}$ and $\mathrm{R}$ will displace the cation of $\mathrm{P}$ from its aqueous solution and deposit the metal $P$
3 metal $\mathrm{R}$ will displace the cation of $\mathrm{P}$ from its aqueous solution and deposit the metal $\mathrm{P}$
4 metal $\mathrm{P}$ will displace the cation of $\mathrm{R}$ from its aqueous solution and deposit the metal R.
J and K CET-(2009)
Join With Us for More Updates
ELECTROCHEMISTRY

275981 What is the emf of the cell, whose half cells are given below $\mathrm{Mg}^{2+}+2 \mathrm{e}^{-} \rightarrow \operatorname{Mg}(\mathrm{s}) \mathrm{E}=-2.37 \mathrm{~V}$
$\mathrm{Cu}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Cu}(\mathrm{s}) \mathrm{E}=+\mathbf{0 . 3 4} \mathrm{V}$

1 $-2.30 \mathrm{~V}$
2 $1.336 \mathrm{~V}$
3 $2.71 \mathrm{~V}$
4 $2.03 \mathrm{~V}$
CG PET -2005
ELECTROCHEMISTRY

275982 For the feasibility of a redox reaction in a cell, the emf should be

1 positive
2 fixed
3 zero
4 negative
J and K CET-(2005)
ELECTROCHEMISTRY

275992 Which of the following reaction is possible at anode?

1 $\mathrm{Fe}_{2}+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{~F}^{-}$
2 $2 \mathrm{H}^{+}+\frac{1}{2} \mathrm{O}_{2}+2 \mathrm{e}^{-} \rightarrow \mathrm{H}_{2} \mathrm{O}$
3 $2 \mathrm{Cr}_{2}^{3+}+7 \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}+14 \mathrm{H}^{+}+6 \mathrm{e}^{-}$
4 None of the above
VITEEE-2016
ELECTROCHEMISTRY

275950 The standard reduction electrode potentials of the three electrodes $P, Q$ and $R$ are respectively $-1.76 \mathrm{~V}, 0.34 \mathrm{~V}$ and $0.8 \mathrm{~V}$. Then

1 metal $\mathrm{Q}$ will displace the cation of $\mathrm{P}$ from its aqueous solution and deposit the metal $P$
2 both metals $\mathrm{Q}$ and $\mathrm{R}$ will displace the cation of $\mathrm{P}$ from its aqueous solution and deposit the metal $P$
3 metal $\mathrm{R}$ will displace the cation of $\mathrm{P}$ from its aqueous solution and deposit the metal $\mathrm{P}$
4 metal $\mathrm{P}$ will displace the cation of $\mathrm{R}$ from its aqueous solution and deposit the metal R.
J and K CET-(2009)
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