Chemistry carries the highest scoring potential in JEE for anyone who keeps the three branches separate in revision. This set covers physical chemistry numericals, organic reaction mechanisms and named reactions, and inorganic chemistry including periodic trends, chemical bonding and coordination compounds. Organic questions show the mechanism arrow by arrow, so the reasoning transfers to reactions you have not seen before.
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.102Easy
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.103Easy
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.104Easy
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.105Easy
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.106Easy
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.107Easy
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.108Easy
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.109Easy
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.110Easy
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.111Easy
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.112Easy
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.113Easy
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.114Easy
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.115Easy
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.
Q.116Easy
In a galvanic cell, if the standard cell potential E°cell is negative, which statement is true?
Answer: B
Negative E°cell indicates non-spontaneous reaction with positive ΔG°. The relationship is ΔG° = -nFE°cell.
Q.117Easy
Which electrodes combination gives the maximum EMF in a galvanic cell at 25°C?
Answer: B
Maximum EMF = E°cathode - E°anode = 0.80 - (-0.76) = 1.56 V for Zn-Ag cell.
Q.118Easy
The conductivity of a solution decreased upon dilution. This is because:
Answer: B
Conductivity (κ) = concentration × molar conductivity. Upon dilution, concentration decreases faster than molar conductivity increases.
Q.119Easy
In the electrolysis of molten NaCl using inert electrodes, what is produced at the cathode?
Answer: B
At cathode: Na⁺ + e⁻ → Na (reduction). At anode: 2Cl⁻ → Cl₂ + 2e⁻ (oxidation).
Q.120Easy
In a Daniel cell, the mass of zinc electrode decreases and copper electrode increases. This indicates:
