Standard Reduction electrode potential of three metals X, Y, and Z are -1.2 V, +0.5 V and -3 V respectively. The reducing power of these metals will be : 

1. Y > X >Z 2. Z > X > Y
3. X > Y > Z 4. Y > Z > X
Subtopic:  Electrochemical Series |
 82%
From NCERT
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When a copper wire is immersed in a solution of AgNO3, the colour of the solution becomes blue because copper:

1. Forms a soluble complex with \(AgNO_3\)
2. Is oxidised to \(Cu^{2+}\)
3. Is reduced to \(Cu^{2-}\)
4. Splits up into atomic form and dissolves

Subtopic:  Electrochemical Series |
 80%
From NCERT
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Without losing it's concentration, ZnCl2 solution cannot be kept in contact with :

1. Au

2. Al

3. Pb

4. Ag

Subtopic:  Electrochemical Series |
 74%
From NCERT
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A hypothetical electrochemical cell is shown below.
A|A+(x M) || B+(y M)|B
The Emf measured is +0.20 V. The cell reaction is:

1. A+ + B → A + B+

2.  A+ + e- → A ; B+ + e- → B

3. The cell reaction cannot be predicted.

4. A + B+ → A+ + B

Subtopic:  Electrochemical Series | Nernst Equation |
 75%
From NCERT
AIPMT - 2006
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The negative sign in the expression EoZn2+/Zn = -0.76 V indicates : 

1. Metal reactivity increases.

2. Metal reactivity decreases.

3. No effect on metal.

4. None of the above.

Subtopic:  Electrochemical Series |
 58%
From NCERT
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The most stable oxidized species among the following is: 
\(E_{{\mathrm{Cr}_2 \mathrm{O}_7^2}/ \mathrm{Cr}^{3+}}^{o} =1.33 \mathrm{~V} ; E_{\mathrm{Cl}_2 / \mathrm{Cl}^{-}}^{o}=1.36 \mathrm{~V} \)
\( E_{\mathrm{MnO_{4}}^{-} / \mathrm{Mn}^{2+}}^{o}=1.51 \mathrm{~V} ; E_{\mathrm{Cr}^{3+} / \mathrm{Cr}}^{o}=-0.74 \mathrm{~V}\)

1. Cr3+  2. MnO4-
3. Cr2O72- 4. Mn2+ 
Subtopic:  Electrochemical Series |
 59%
From NCERT
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If an iron rod is dipped in CuSO4 solution, then:

1. Blue colour of the solution turns red.

2. Brown layer is deposited on iron rod.

3. No change occurs in the colour of the solution.

4. None of the above.

Subtopic:  Electrochemical Series |
From NCERT
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A solution containing one mole per litre each of Cu(NO3)2, AgNO3, Hg2(NO3)2 and Mg(NO3)2 is being electrolyzed by using inert electrodes. The values of standard electrode potentials in volt (reduction potentials) are,

Ag/Ag = 0.80 V, Hg22+/2Hg = 0.79 V,

Cu2+/Cu = +0.34 V and Mg2+/Mg = -2.37 V

With increasing voltage, the sequence of deposition of metals on the cathode will be:

1. Ag, Hg, Cu, Mg

2. Mg, Cu, Hg, Ag

3. Ag, Hg, Cu

4. Cu, Hg, Ag

Subtopic:  Electrochemical Series |
From NCERT
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