Statement 1: The standard electrode potential of the system Mg2+ | Mg can be measured with respect to hydrogen electrode.
Statement 2: The standard electrode potential for hydrogen electrode is zero.


1. Statement 1 is true, statement 2 is false.
2. Statement 1 is false, statement 1 is true.
3. Both statements are true.
4. Both statements are false.
Subtopic:  Electrode & Electrode Potential |
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Given below are two statements: 
 
Assertion (A): Copper sulphate solutions can be store in a zinc pot.
Reason (R): Zinc is more reactive than copper. 

1. Both (A) and (R) are true and (R) is the correct explanation of (A).
2. Both (A) and (R) are true but (R) is not the correct explanation of (A).
3. (A) is true but (R) is false.
4. (A) is false but (R) is true.
Subtopic:  Electrochemical Series |
 63%
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Substances that can oxidise ferrous ions under suitable conditions among the following is-
(Given: \(E_{Fe^{2+}/Fe^{+3}}^{o}\)=−0.77 V, \(E_{F_{2}/F^{-}}^{o}\)=2.87 V, \(E_{Cl_{2}/Cl^{-}}^{o}\) = 1.36 V, \(E_{O_{2}/H_{2}O}^{o}\) = 1.23V)

1. F2
2. Cl2
3. O2
4. All of the above
 
Subtopic:  Electrochemical Series |
 72%
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The potential of hydrogen electrode in contact with a solution with pH =10, is -


1. −0.0591 V
2. −5.91 V
2. 0.0591 V
4. −0.591 V
Subtopic:  Relation between Emf, G, Kc & pH |
 73%
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The emf of the cell in which the following reaction takes place is:

Ni(s)+2Ag+(0.002 M) →Ni2+(0.160 M) + 2Ag(s)
( Given that \(E_{cell}^{o}\)= 1.05 V)

1. Ecell= 9.14 V
2. Ecell= 0.0914 V
3. Ecell= 0.00914 V
4. Ecell= 0.914 V

Subtopic:  Nernst Equation |
 72%
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The cell in which the following reactions occurs:

2Fe3+(aq)+2I-(aq)→2Fe2+(aq)+I2(s) has \(E_{cell}^{o}\)= 0.236 V at 298 K.

The standard Gibbs energy of the cell reaction is -

1.   41.14 kJ mol−1
2.   45.54 kJ mol−1
3. −49.94 kJ mol−1
4. −45.54 kJ mol−1

 

Subtopic:  Relation between Emf, G, Kc & pH |
 74%
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Given below are two statements: 
 
Assertion (A): The conductivity of a solution decreases with dilution.
Reason (R): Conductivity of a solution depends on the number of ions and the number of ions
decreases when the solution is diluted.

1. Both (A) and (R) are true and (R) is the correct explanation of (A).
2. Both (A) and (R) are true but (R) is not the correct explanation of (A).
3. (A) is true but (R) is false.
4. (A) is false but (R) is true.
 

 
Subtopic:  Conductance & Conductivity |
 67%
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The molar conductivity of 0.025 mol L−1 methanoic acid is 46.1 S cm2 mol−1.

The dissociation constant of methanoic acid is-

 Given λ°(H+)= 349.6 S cm2 mol−1 and λ°(HCOO) = 54.6 S cm2 mol

1. \(1.27×10^{-4}mol ~L^{−1}\)
2. \(5.17×10^{-5}mol ~L^{−1}\)
3. \(3.67×10^{-4}mol ~L^{−1}\)
4. \(4.87×10^{-5}mol ~L^{−1}\)

Subtopic:   Kohlrausch Law & Cell Constant |
 57%
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The number of electrons flow through the wire when a current of 0.5 ampere flows through a metallic wire for 2 hours, is-

1. \(6.25×10^{22}\)
2. \(2.25×10^{22}\)
3 \(8.25×10^{22}\)
4. \(4.25×10^{22}\)

Subtopic:  Faraday’s Law of Electrolysis |
 74%
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The metals among the following that can be  extracted electrolytically is -
1. K
2. Na
3. Al
4. All of the above

 

Subtopic:  Electrochemical Series |
 82%
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