Which of the following is the SI unit of electrical conductivity?
Answer: A
Electrical conductivity is measured in Siemens per meter (S·m⁻¹). Ω·m is the unit of resistivity, which is the reciprocal of conductivity.
Q.2Easy
In a galvanic cell, which electrode acts as the anode?
Answer: B
In a galvanic cell, oxidation occurs at the anode. The anode is the negative electrode where electrons are released.
Q.3Easy
What is the charge on one mole of electrons?
Answer: C
One mole of electrons carries a charge equal to Faraday's constant, which is approximately 96485 C/mol or 96500 C/mol.
Q.4Easy
The Nernst equation relates cell potential to concentration. At 25°C, which form is correct?
Answer: C
The Nernst equation at 25°C is E = E° + (0.0592/n) log Q, where Q is the reaction quotient and n is the number of electrons transferred.
Q.5Easy
Which of the following statements about electrolysis is INCORRECT?
Answer: B
In electrolysis, oxidation occurs at the ANODE, not the cathode. The cathode is where reduction occurs. At the anode, electrons are removed from species.
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Q.6Easy
What is the SI unit of electrical conductivity?
Answer: A
Electrical conductivity is measured in Siemens per meter (S·m⁻¹). Ω·m is the unit of resistivity, which is the inverse of conductivity.
Q.7Easy
In a galvanic cell, which electrode acts as the negative terminal?
Answer: B
In a galvanic cell, the anode is the negative electrode where oxidation occurs. The cathode is positive where reduction occurs.
Q.8Easy
What does Faraday's first law of electrolysis state?
Answer: A
Faraday's first law states that the mass of substance deposited/dissolved during electrolysis is directly proportional to the quantity of electricity (charge) passed through the electrolyte.
Q.9Easy
The Nernst equation is used to calculate:
Answer: A
The Nernst equation: E = E° - (RT/nF)ln(Q) calculates the cell potential when concentrations are not at standard state (1 M).
Q.10Easy
Which of the following is a primary cell (non-rechargeable)?
Answer: B
A dry cell or Leclanche cell is a primary cell that cannot be recharged. Lead-acid and Ni-Cd are secondary cells; Li-ion is rechargeable.
Q.11Easy
In electroplating, the object to be plated is connected to which terminal?
Answer: B
In electroplating, the object to be plated is made the cathode (negative terminal) where reduction occurs, causing metal deposition.
Q.12Easy
In a galvanic cell, oxidation occurs at which electrode?
Answer: B
In a galvanic cell, oxidation occurs at the anode. The anode is the negative electrode where electrons are released and the species loses electrons.
Q.13Easy
The Faraday constant (F) is approximately equal to:
Answer: A
Faraday constant (F) = 96485 Coulombs per mole of electrons. This represents the charge carried by one mole of electrons.
Q.14Easy
Which statement is correct regarding electrode potentials?
Answer: B
By international convention, the standard reduction potential of H⁺/H₂ couple is taken as 0.00 V at 25°C. This serves as the reference electrode for all other electrode potentials.
Q.15Easy
For a spontaneous electrochemical cell, the cell potential (E°cell) should be:
Answer: C
For a spontaneous cell reaction, E°cell > 0 (positive). When E°cell is negative, the reaction is non-spontaneous. E°cell = E°cathode - E°anode.
Q.16Easy
In a galvanic cell, the electrode where oxidation occurs is called:
Answer: A
In a galvanic cell, oxidation occurs at the anode (negative electrode), while reduction occurs at the cathode (positive electrode).
Q.17Easy
The standard cell potential (E°cell) for a reaction is -0.45 V at 25°C. What can be concluded about the reaction?
Answer: B
When E°cell is negative, ΔG° = -nFE°cell will be positive, indicating a non-spontaneous reaction under standard conditions.
Q.18Easy
Which of the following is NOT an application of electrochemistry?
Answer: C
Rusting of iron is a corrosion process (galvanic corrosion) and not a direct application like electroplating, electrolysis, or electrorefining.
Q.19Easy
The Faraday constant (F) is numerically equal to:
Answer: A
F = N_A × e = 6.022 × 10²³ × 1.602 × 10⁻¹⁹ C = 96485 C/mol, which equals Avogadro's number times the charge of one electron.
Q.20Easy
In the electrochemical series, which metal is most easily oxidized?
Answer: C
Potassium (K) has the most negative standard reduction potential and is most easily oxidized among the given options. The order of ease of oxidation is K > Cu > Ag > Au.
