Electrochemistry Practice

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NEET Chemistry - Chapter 8

Electrochemistry Practice Tests

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Cell basics
1. In a galvanic cell, oxidation occurs at:
- A. anode (Correct)
- B. cathode
- C. salt bridge
- D. voltmeter
Explanation: Oxidation always occurs at the anode.
Cell basics
2. In a galvanic cell, reduction occurs at:
- A. cathode (Correct)
- B. anode
- C. salt bridge
- D. wire
Explanation: Reduction always occurs at the cathode.
Electron flow
3. In a galvanic cell, electrons move through the external circuit from:
- A. anode to cathode (Correct)
- B. cathode to anode
- C. salt bridge to anode
- D. electrolyte to wire
Explanation: Electrons released at anode travel to cathode.
Salt bridge
4. Main role of the salt bridge is to:
- A. maintain charge balance (Correct)
- B. carry electrons
- C. increase activation energy
- D. act as oxidising agent
Explanation: It permits ion migration and completes the circuit.
Cell notation
5. In cell notation, the double vertical line denotes:
- A. salt bridge (Correct)
- B. phase boundary
- C. electron flow
- D. equilibrium
Explanation: The double line represents the junction between half-cells.
Daniell cell
6. In the Daniell cell, zinc acts as:
- A. anode (Correct)
- B. cathode
- C. electrolyte
- D. salt bridge
Explanation: Zinc is oxidised to Zn$^{2+}$.
Daniell cell
7. In the Daniell cell, copper acts as:
- A. cathode (Correct)
- B. anode
- C. oxidising agent only
- D. bridge
Explanation: Copper(II) ions are reduced at cathode.
Potential
8. Standard cell potential is calculated as:
- A. $E^\circ_{cell}=E^\circ_{cathode}-E^\circ_{anode}$ (Correct)
- B. sum of both electrode potentials
- C. $E^\circ_{anode}-E^\circ_{cathode}$
- D. always 1.10 V
Explanation: Reduction potentials are combined as cathode minus anode.
SHE
9. Standard hydrogen electrode has standard potential:
- A. 0 V (Correct)
- B. 1 V
- C. -1 V
- D. 0.5 V
Explanation: SHE is the reference electrode.
SHE
10. In SHE, hydrogen gas pressure is:
- A. 1 bar (Correct)
- B. 10 bar
- C. 0.1 bar
- D. any value
Explanation: Standard pressure is used.
SHE
11. Concentration of $H^+$ in SHE is:
- A. 1 M (Correct)
- B. 0.1 M
- C. 7 M
- D. neutral water
Explanation: Standard-state concentration is used.
Oxidising strength
12. The stronger oxidising agent generally has the:
- A. higher reduction potential (Correct)
- B. lower reduction potential
- C. higher molar mass
- D. higher conductivity
Explanation: It more readily gains electrons.
Reducing strength
13. A strong reducing agent generally has a:
- A. more negative reduction potential (Correct)
- B. more positive reduction potential
- C. zero cell potential
- D. higher osmotic pressure
Explanation: It tends to lose electrons easily.
Spontaneity
14. A galvanic cell reaction is spontaneous when $E_{cell}$ is:
- A. positive (Correct)
- B. negative
- C. zero always
- D. infinite
Explanation: Positive emf means spontaneous electrical work output.
Nernst
15. The Nernst equation is used when conditions are:
- A. non-standard (Correct)
- B. only standard
- C. only acidic
- D. only gaseous
Explanation: It corrects potential away from standard conditions.
Nernst
16. At 25$^\circ$C, the Nernst equation contains a term proportional to:
- A. $\log Q$ (Correct)
- B. $\log K_b$ only
- C. $1/T$ only
- D. $\Delta H$
Explanation: Cell potential depends on reaction quotient.
Equilibrium
17. At equilibrium, cell emf becomes:
- A. zero (Correct)
- B. maximum positive
- C. maximum negative
- D. equal to 1 faraday
Explanation: There is no net driving force at equilibrium.
Faraday
18. Faraday's first law relates deposited mass to:
- A. charge passed (Correct)
- B. pressure
- C. temperature
- D. molarity only
Explanation: More charge deposits more substance.
Faraday
19. The relation between charge, current, and time is:
- A. $Q=It$ (Correct)
- B. $Q=I/t$
- C. $Q=V/R$
- D. $Q=RT$
Explanation: Charge equals current multiplied by time.
Faraday constant
20. One faraday corresponds approximately to:
- A. 96500 C (Correct)
- B. 8.314 C
- C. 6.022 C
- D. 22.4 C
Explanation: One mole of electrons carries about 96500 coulombs.
Deposition
21. One mole of Ag$^+$ requires how many moles of electrons for deposition?
- A. 1 (Correct)
- B. 2
- C. 3
- D. 0.5
Explanation: Ag$^+ + e^- \to Ag$.
Deposition
22. One mole of Cu$^{2+}$ requires how many moles of electrons for deposition?
- A. 2 (Correct)
- B. 1
- C. 3
- D. 4
Explanation: Cu$^{2+}+2e^-\to Cu$.
Conductance
23. Conductance is the reciprocal of:
- A. resistance (Correct)
- B. resistivity
- C. current
- D. potential
Explanation: $G=1/R$.
Molar conductivity
24. Molar conductivity is related to conductivity by:
- A. $\Lambda_m=\kappa\times1000/C$ (Correct)
- B. $\Lambda_m=\kappa C/1000$
- C. $\Lambda_m=RC$
- D. $\Lambda_m=E/k$
Explanation: For concentration in mol L$^{-1}$, this relation is used.
Electrochem idea
25. Electrochemistry connects redox change with:
- A. electrical energy or charge flow (Correct)
- B. surface tension only
- C. orbital hybridisation
- D. nuclear spin
Explanation: It is the redox-electricity bridge.
Cell basics
26. In a galvanic cell, oxidation occurs at:
- A. anode (Correct)
- B. cathode
- C. salt bridge
- D. voltmeter
Explanation: Oxidation always occurs at the anode.
Cell basics
27. In a galvanic cell, reduction occurs at:
- A. cathode (Correct)
- B. anode
- C. salt bridge
- D. wire
Explanation: Reduction always occurs at the cathode.
Electron flow
28. In a galvanic cell, electrons move through the external circuit from:
- A. anode to cathode (Correct)
- B. cathode to anode
- C. salt bridge to anode
- D. electrolyte to wire
Explanation: Electrons released at anode travel to cathode.
Salt bridge
29. Main role of the salt bridge is to:
- A. maintain charge balance (Correct)
- B. carry electrons
- C. increase activation energy
- D. act as oxidising agent
Explanation: It permits ion migration and completes the circuit.
Cell notation
30. In cell notation, the double vertical line denotes:
- A. salt bridge (Correct)
- B. phase boundary
- C. electron flow
- D. equilibrium
Explanation: The double line represents the junction between half-cells.
Daniell cell
31. In the Daniell cell, zinc acts as:
- A. anode (Correct)
- B. cathode
- C. electrolyte
- D. salt bridge
Explanation: Zinc is oxidised to Zn$^{2+}$.
Daniell cell
32. In the Daniell cell, copper acts as:
- A. cathode (Correct)
- B. anode
- C. oxidising agent only
- D. bridge
Explanation: Copper(II) ions are reduced at cathode.
Potential
33. Standard cell potential is calculated as:
- A. $E^\circ_{cell}=E^\circ_{cathode}-E^\circ_{anode}$ (Correct)
- B. sum of both electrode potentials
- C. $E^\circ_{anode}-E^\circ_{cathode}$
- D. always 1.10 V
Explanation: Reduction potentials are combined as cathode minus anode.
SHE
34. Standard hydrogen electrode has standard potential:
- A. 0 V (Correct)
- B. 1 V
- C. -1 V
- D. 0.5 V
Explanation: SHE is the reference electrode.
SHE
35. In SHE, hydrogen gas pressure is:
- A. 1 bar (Correct)
- B. 10 bar
- C. 0.1 bar
- D. any value
Explanation: Standard pressure is used.
SHE
36. Concentration of $H^+$ in SHE is:
- A. 1 M (Correct)
- B. 0.1 M
- C. 7 M
- D. neutral water
Explanation: Standard-state concentration is used.
Oxidising strength
37. The stronger oxidising agent generally has the:
- A. higher reduction potential (Correct)
- B. lower reduction potential
- C. higher molar mass
- D. higher conductivity
Explanation: It more readily gains electrons.
Reducing strength
38. A strong reducing agent generally has a:
- A. more negative reduction potential (Correct)
- B. more positive reduction potential
- C. zero cell potential
- D. higher osmotic pressure
Explanation: It tends to lose electrons easily.
Spontaneity
39. A galvanic cell reaction is spontaneous when $E_{cell}$ is:
- A. positive (Correct)
- B. negative
- C. zero always
- D. infinite
Explanation: Positive emf means spontaneous electrical work output.
Nernst
40. The Nernst equation is used when conditions are:
- A. non-standard (Correct)
- B. only standard
- C. only acidic
- D. only gaseous
Explanation: It corrects potential away from standard conditions.
Nernst
41. At 25$^\circ$C, the Nernst equation contains a term proportional to:
- A. $\log Q$ (Correct)
- B. $\log K_b$ only
- C. $1/T$ only
- D. $\Delta H$
Explanation: Cell potential depends on reaction quotient.
Equilibrium
42. At equilibrium, cell emf becomes:
- A. zero (Correct)
- B. maximum positive
- C. maximum negative
- D. equal to 1 faraday
Explanation: There is no net driving force at equilibrium.
Faraday
43. Faraday's first law relates deposited mass to:
- A. charge passed (Correct)
- B. pressure
- C. temperature
- D. molarity only
Explanation: More charge deposits more substance.
Faraday
44. The relation between charge, current, and time is:
- A. $Q=It$ (Correct)
- B. $Q=I/t$
- C. $Q=V/R$
- D. $Q=RT$
Explanation: Charge equals current multiplied by time.
Faraday constant
45. One faraday corresponds approximately to:
- A. 96500 C (Correct)
- B. 8.314 C
- C. 6.022 C
- D. 22.4 C
Explanation: One mole of electrons carries about 96500 coulombs.
Deposition
46. One mole of Ag$^+$ requires how many moles of electrons for deposition?
- A. 1 (Correct)
- B. 2
- C. 3
- D. 0.5
Explanation: Ag$^+ + e^- \to Ag$.
Deposition
47. One mole of Cu$^{2+}$ requires how many moles of electrons for deposition?
- A. 2 (Correct)
- B. 1
- C. 3
- D. 4
Explanation: Cu$^{2+}+2e^-\to Cu$.
Conductance
48. Conductance is the reciprocal of:
- A. resistance (Correct)
- B. resistivity
- C. current
- D. potential
Explanation: $G=1/R$.
Molar conductivity
49. Molar conductivity is related to conductivity by:
- A. $\Lambda_m=\kappa\times1000/C$ (Correct)
- B. $\Lambda_m=\kappa C/1000$
- C. $\Lambda_m=RC$
- D. $\Lambda_m=E/k$
Explanation: For concentration in mol L$^{-1}$, this relation is used.
Electrochem idea
50. Electrochemistry connects redox change with:
- A. electrical energy or charge flow (Correct)
- B. surface tension only
- C. orbital hybridisation
- D. nuclear spin
Explanation: It is the redox-electricity bridge.
Cell basics
51. In a galvanic cell, oxidation occurs at:
- A. anode (Correct)
- B. cathode
- C. salt bridge
- D. voltmeter
Explanation: Oxidation always occurs at the anode.
Cell basics
52. In a galvanic cell, reduction occurs at:
- A. cathode (Correct)
- B. anode
- C. salt bridge
- D. wire
Explanation: Reduction always occurs at the cathode.
Electron flow
53. In a galvanic cell, electrons move through the external circuit from:
- A. anode to cathode (Correct)
- B. cathode to anode
- C. salt bridge to anode
- D. electrolyte to wire
Explanation: Electrons released at anode travel to cathode.
Salt bridge
54. Main role of the salt bridge is to:
- A. maintain charge balance (Correct)
- B. carry electrons
- C. increase activation energy
- D. act as oxidising agent
Explanation: It permits ion migration and completes the circuit.
Cell notation
55. In cell notation, the double vertical line denotes:
- A. salt bridge (Correct)
- B. phase boundary
- C. electron flow
- D. equilibrium
Explanation: The double line represents the junction between half-cells.
Daniell cell
56. In the Daniell cell, zinc acts as:
- A. anode (Correct)
- B. cathode
- C. electrolyte
- D. salt bridge
Explanation: Zinc is oxidised to Zn$^{2+}$.
Daniell cell
57. In the Daniell cell, copper acts as:
- A. cathode (Correct)
- B. anode
- C. oxidising agent only
- D. bridge
Explanation: Copper(II) ions are reduced at cathode.
Potential
58. Standard cell potential is calculated as:
- A. $E^\circ_{cell}=E^\circ_{cathode}-E^\circ_{anode}$ (Correct)
- B. sum of both electrode potentials
- C. $E^\circ_{anode}-E^\circ_{cathode}$
- D. always 1.10 V
Explanation: Reduction potentials are combined as cathode minus anode.
SHE
59. Standard hydrogen electrode has standard potential:
- A. 0 V (Correct)
- B. 1 V
- C. -1 V
- D. 0.5 V
Explanation: SHE is the reference electrode.
SHE
60. In SHE, hydrogen gas pressure is:
- A. 1 bar (Correct)
- B. 10 bar
- C. 0.1 bar
- D. any value
Explanation: Standard pressure is used.
SHE
61. Concentration of $H^+$ in SHE is:
- A. 1 M (Correct)
- B. 0.1 M
- C. 7 M
- D. neutral water
Explanation: Standard-state concentration is used.
Oxidising strength
62. The stronger oxidising agent generally has the:
- A. higher reduction potential (Correct)
- B. lower reduction potential
- C. higher molar mass
- D. higher conductivity
Explanation: It more readily gains electrons.
Reducing strength
63. A strong reducing agent generally has a:
- A. more negative reduction potential (Correct)
- B. more positive reduction potential
- C. zero cell potential
- D. higher osmotic pressure
Explanation: It tends to lose electrons easily.
Spontaneity
64. A galvanic cell reaction is spontaneous when $E_{cell}$ is:
- A. positive (Correct)
- B. negative
- C. zero always
- D. infinite
Explanation: Positive emf means spontaneous electrical work output.
Nernst
65. The Nernst equation is used when conditions are:
- A. non-standard (Correct)
- B. only standard
- C. only acidic
- D. only gaseous
Explanation: It corrects potential away from standard conditions.
Nernst
66. At 25$^\circ$C, the Nernst equation contains a term proportional to:
- A. $\log Q$ (Correct)
- B. $\log K_b$ only
- C. $1/T$ only
- D. $\Delta H$
Explanation: Cell potential depends on reaction quotient.
Equilibrium
67. At equilibrium, cell emf becomes:
- A. zero (Correct)
- B. maximum positive
- C. maximum negative
- D. equal to 1 faraday
Explanation: There is no net driving force at equilibrium.
Faraday
68. Faraday's first law relates deposited mass to:
- A. charge passed (Correct)
- B. pressure
- C. temperature
- D. molarity only
Explanation: More charge deposits more substance.
Faraday
69. The relation between charge, current, and time is:
- A. $Q=It$ (Correct)
- B. $Q=I/t$
- C. $Q=V/R$
- D. $Q=RT$
Explanation: Charge equals current multiplied by time.
Faraday constant
70. One faraday corresponds approximately to:
- A. 96500 C (Correct)
- B. 8.314 C
- C. 6.022 C
- D. 22.4 C
Explanation: One mole of electrons carries about 96500 coulombs.
Deposition
71. One mole of Ag$^+$ requires how many moles of electrons for deposition?
- A. 1 (Correct)
- B. 2
- C. 3
- D. 0.5
Explanation: Ag$^+ + e^- \to Ag$.
Deposition
72. One mole of Cu$^{2+}$ requires how many moles of electrons for deposition?
- A. 2 (Correct)
- B. 1
- C. 3
- D. 4
Explanation: Cu$^{2+}+2e^-\to Cu$.
Conductance
73. Conductance is the reciprocal of:
- A. resistance (Correct)
- B. resistivity
- C. current
- D. potential
Explanation: $G=1/R$.
Molar conductivity
74. Molar conductivity is related to conductivity by:
- A. $\Lambda_m=\kappa\times1000/C$ (Correct)
- B. $\Lambda_m=\kappa C/1000$
- C. $\Lambda_m=RC$
- D. $\Lambda_m=E/k$
Explanation: For concentration in mol L$^{-1}$, this relation is used.
Electrochem idea
75. Electrochemistry connects redox change with:
- A. electrical energy or charge flow (Correct)
- B. surface tension only
- C. orbital hybridisation
- D. nuclear spin
Explanation: It is the redox-electricity bridge.
Cell basics
76. In a galvanic cell, oxidation occurs at:
- A. anode (Correct)
- B. cathode
- C. salt bridge
- D. voltmeter
Explanation: Oxidation always occurs at the anode.
Cell basics
77. In a galvanic cell, reduction occurs at:
- A. cathode (Correct)
- B. anode
- C. salt bridge
- D. wire
Explanation: Reduction always occurs at the cathode.
Electron flow
78. In a galvanic cell, electrons move through the external circuit from:
- A. anode to cathode (Correct)
- B. cathode to anode
- C. salt bridge to anode
- D. electrolyte to wire
Explanation: Electrons released at anode travel to cathode.
Salt bridge
79. Main role of the salt bridge is to:
- A. maintain charge balance (Correct)
- B. carry electrons
- C. increase activation energy
- D. act as oxidising agent
Explanation: It permits ion migration and completes the circuit.
Cell notation
80. In cell notation, the double vertical line denotes:
- A. salt bridge (Correct)
- B. phase boundary
- C. electron flow
- D. equilibrium
Explanation: The double line represents the junction between half-cells.
Daniell cell
81. In the Daniell cell, zinc acts as:
- A. anode (Correct)
- B. cathode
- C. electrolyte
- D. salt bridge
Explanation: Zinc is oxidised to Zn$^{2+}$.
Daniell cell
82. In the Daniell cell, copper acts as:
- A. cathode (Correct)
- B. anode
- C. oxidising agent only
- D. bridge
Explanation: Copper(II) ions are reduced at cathode.
Potential
83. Standard cell potential is calculated as:
- A. $E^\circ_{cell}=E^\circ_{cathode}-E^\circ_{anode}$ (Correct)
- B. sum of both electrode potentials
- C. $E^\circ_{anode}-E^\circ_{cathode}$
- D. always 1.10 V
Explanation: Reduction potentials are combined as cathode minus anode.
SHE
84. Standard hydrogen electrode has standard potential:
- A. 0 V (Correct)
- B. 1 V
- C. -1 V
- D. 0.5 V
Explanation: SHE is the reference electrode.
SHE
85. In SHE, hydrogen gas pressure is:
- A. 1 bar (Correct)
- B. 10 bar
- C. 0.1 bar
- D. any value
Explanation: Standard pressure is used.
SHE
86. Concentration of $H^+$ in SHE is:
- A. 1 M (Correct)
- B. 0.1 M
- C. 7 M
- D. neutral water
Explanation: Standard-state concentration is used.
Oxidising strength
87. The stronger oxidising agent generally has the:
- A. higher reduction potential (Correct)
- B. lower reduction potential
- C. higher molar mass
- D. higher conductivity
Explanation: It more readily gains electrons.
Reducing strength
88. A strong reducing agent generally has a:
- A. more negative reduction potential (Correct)
- B. more positive reduction potential
- C. zero cell potential
- D. higher osmotic pressure
Explanation: It tends to lose electrons easily.
Spontaneity
89. A galvanic cell reaction is spontaneous when $E_{cell}$ is:
- A. positive (Correct)
- B. negative
- C. zero always
- D. infinite
Explanation: Positive emf means spontaneous electrical work output.
Nernst
90. The Nernst equation is used when conditions are:
- A. non-standard (Correct)
- B. only standard
- C. only acidic
- D. only gaseous
Explanation: It corrects potential away from standard conditions.
Nernst
91. At 25$^\circ$C, the Nernst equation contains a term proportional to:
- A. $\log Q$ (Correct)
- B. $\log K_b$ only
- C. $1/T$ only
- D. $\Delta H$
Explanation: Cell potential depends on reaction quotient.
Equilibrium
92. At equilibrium, cell emf becomes:
- A. zero (Correct)
- B. maximum positive
- C. maximum negative
- D. equal to 1 faraday
Explanation: There is no net driving force at equilibrium.
Faraday
93. Faraday's first law relates deposited mass to:
- A. charge passed (Correct)
- B. pressure
- C. temperature
- D. molarity only
Explanation: More charge deposits more substance.
Faraday
94. The relation between charge, current, and time is:
- A. $Q=It$ (Correct)
- B. $Q=I/t$
- C. $Q=V/R$
- D. $Q=RT$
Explanation: Charge equals current multiplied by time.
Faraday constant
95. One faraday corresponds approximately to:
- A. 96500 C (Correct)
- B. 8.314 C
- C. 6.022 C
- D. 22.4 C
Explanation: One mole of electrons carries about 96500 coulombs.
Deposition
96. One mole of Ag$^+$ requires how many moles of electrons for deposition?
- A. 1 (Correct)
- B. 2
- C. 3
- D. 0.5
Explanation: Ag$^+ + e^- \to Ag$.
Deposition
97. One mole of Cu$^{2+}$ requires how many moles of electrons for deposition?
- A. 2 (Correct)
- B. 1
- C. 3
- D. 4
Explanation: Cu$^{2+}+2e^-\to Cu$.
Conductance
98. Conductance is the reciprocal of:
- A. resistance (Correct)
- B. resistivity
- C. current
- D. potential
Explanation: $G=1/R$.
Molar conductivity
99. Molar conductivity is related to conductivity by:
- A. $\Lambda_m=\kappa\times1000/C$ (Correct)
- B. $\Lambda_m=\kappa C/1000$
- C. $\Lambda_m=RC$
- D. $\Lambda_m=E/k$
Explanation: For concentration in mol L$^{-1}$, this relation is used.
Electrochem idea
100. Electrochemistry connects redox change with:
- A. electrical energy or charge flow (Correct)
- B. surface tension only
- C. orbital hybridisation
- D. nuclear spin
Explanation: It is the redox-electricity bridge.
Cell basics
101. In a galvanic cell, oxidation occurs at:
- A. anode (Correct)
- B. cathode
- C. salt bridge
- D. voltmeter
Explanation: Oxidation always occurs at the anode.
Cell basics
102. In a galvanic cell, reduction occurs at:
- A. cathode (Correct)
- B. anode
- C. salt bridge
- D. wire
Explanation: Reduction always occurs at the cathode.
Electron flow
103. In a galvanic cell, electrons move through the external circuit from:
- A. anode to cathode (Correct)
- B. cathode to anode
- C. salt bridge to anode
- D. electrolyte to wire
Explanation: Electrons released at anode travel to cathode.
Salt bridge
104. Main role of the salt bridge is to:
- A. maintain charge balance (Correct)
- B. carry electrons
- C. increase activation energy
- D. act as oxidising agent
Explanation: It permits ion migration and completes the circuit.
Cell notation
105. In cell notation, the double vertical line denotes:
- A. salt bridge (Correct)
- B. phase boundary
- C. electron flow
- D. equilibrium
Explanation: The double line represents the junction between half-cells.
Daniell cell
106. In the Daniell cell, zinc acts as:
- A. anode (Correct)
- B. cathode
- C. electrolyte
- D. salt bridge
Explanation: Zinc is oxidised to Zn$^{2+}$.
Daniell cell
107. In the Daniell cell, copper acts as:
- A. cathode (Correct)
- B. anode
- C. oxidising agent only
- D. bridge
Explanation: Copper(II) ions are reduced at cathode.
Potential
108. Standard cell potential is calculated as:
- A. $E^\circ_{cell}=E^\circ_{cathode}-E^\circ_{anode}$ (Correct)
- B. sum of both electrode potentials
- C. $E^\circ_{anode}-E^\circ_{cathode}$
- D. always 1.10 V
Explanation: Reduction potentials are combined as cathode minus anode.
SHE
109. Standard hydrogen electrode has standard potential:
- A. 0 V (Correct)
- B. 1 V
- C. -1 V
- D. 0.5 V
Explanation: SHE is the reference electrode.
SHE
110. In SHE, hydrogen gas pressure is:
- A. 1 bar (Correct)
- B. 10 bar
- C. 0.1 bar
- D. any value
Explanation: Standard pressure is used.
SHE
111. Concentration of $H^+$ in SHE is:
- A. 1 M (Correct)
- B. 0.1 M
- C. 7 M
- D. neutral water
Explanation: Standard-state concentration is used.
Oxidising strength
112. The stronger oxidising agent generally has the:
- A. higher reduction potential (Correct)
- B. lower reduction potential
- C. higher molar mass
- D. higher conductivity
Explanation: It more readily gains electrons.
Reducing strength
113. A strong reducing agent generally has a:
- A. more negative reduction potential (Correct)
- B. more positive reduction potential
- C. zero cell potential
- D. higher osmotic pressure
Explanation: It tends to lose electrons easily.
Spontaneity
114. A galvanic cell reaction is spontaneous when $E_{cell}$ is:
- A. positive (Correct)
- B. negative
- C. zero always
- D. infinite
Explanation: Positive emf means spontaneous electrical work output.
Nernst
115. The Nernst equation is used when conditions are:
- A. non-standard (Correct)
- B. only standard
- C. only acidic
- D. only gaseous
Explanation: It corrects potential away from standard conditions.
Nernst
116. At 25$^\circ$C, the Nernst equation contains a term proportional to:
- A. $\log Q$ (Correct)
- B. $\log K_b$ only
- C. $1/T$ only
- D. $\Delta H$
Explanation: Cell potential depends on reaction quotient.
Equilibrium
117. At equilibrium, cell emf becomes:
- A. zero (Correct)
- B. maximum positive
- C. maximum negative
- D. equal to 1 faraday
Explanation: There is no net driving force at equilibrium.
Faraday
118. Faraday's first law relates deposited mass to:
- A. charge passed (Correct)
- B. pressure
- C. temperature
- D. molarity only
Explanation: More charge deposits more substance.
Faraday
119. The relation between charge, current, and time is:
- A. $Q=It$ (Correct)
- B. $Q=I/t$
- C. $Q=V/R$
- D. $Q=RT$
Explanation: Charge equals current multiplied by time.
Faraday constant
120. One faraday corresponds approximately to:
- A. 96500 C (Correct)
- B. 8.314 C
- C. 6.022 C
- D. 22.4 C
Explanation: One mole of electrons carries about 96500 coulombs.
Deposition
121. One mole of Ag$^+$ requires how many moles of electrons for deposition?
- A. 1 (Correct)
- B. 2
- C. 3
- D. 0.5
Explanation: Ag$^+ + e^- \to Ag$.
Deposition
122. One mole of Cu$^{2+}$ requires how many moles of electrons for deposition?
- A. 2 (Correct)
- B. 1
- C. 3
- D. 4
Explanation: Cu$^{2+}+2e^-\to Cu$.
Conductance
123. Conductance is the reciprocal of:
- A. resistance (Correct)
- B. resistivity
- C. current
- D. potential
Explanation: $G=1/R$.
Molar conductivity
124. Molar conductivity is related to conductivity by:
- A. $\Lambda_m=\kappa\times1000/C$ (Correct)
- B. $\Lambda_m=\kappa C/1000$
- C. $\Lambda_m=RC$
- D. $\Lambda_m=E/k$
Explanation: For concentration in mol L$^{-1}$, this relation is used.
Electrochem idea
125. Electrochemistry connects redox change with:
- A. electrical energy or charge flow (Correct)
- B. surface tension only
- C. orbital hybridisation
- D. nuclear spin
Explanation: It is the redox-electricity bridge.

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