NEET 2027
HIGH-WEIGHTAGE CHEMISTRY
PART 2
ELECTROCHEMISTRY • KINETICS • SOLUTIONS COORDINATION COMPOUNDS • GOC •
HYDROCARBONS
150 Unique High-Probability Practice Questions
Accurate • Most Expected in NEET 2027 • Professional
Special Features
✓ 150 fresh questions – no overlap with Part 1
✓ Topics with highest chance of appearing in NEET 2027
✓ Short theory + detailed why-correct / why-wrong
✓ Numerical + conceptual mix as per latest pattern
✓ Professional colourful layout for focused study
, CONTENTS
1. Electrochemistry — Theory + Q1 to Q30
2. Chemical Kinetics — Theory + Q31 to Q55
3. Solutions — Theory + Q56 to Q80
4. Coordination Compounds — Theory + Q81 to Q105
5. General Organic Chemistry + Hydrocarbons — Theory + Q106 to Q150
Quick Revision Sheet — Last page
How to Use
1. Read the short theory first.
2. Attempt questions without looking at answers.
3. Study both why the correct option is right and why others are wrong.
4. Revise the formula sheet before the exam.
NEET 2027 | High-Weightage Chemistry | Part 2 Page 2
, 1. ELECTROCHEMISTRY
Electrochemical cells convert chemical energy into electrical energy (Galvanic) or vice versa (Electrolytic).
Standard electrode potential E° is measured with respect to SHE (E° = 0). Nernst equation: E = E° – (RT/nF) ln Q =
E° – (0.059/n) log Q at 298 K. ∆G° = –nFE°_cell. Faraday’s laws: mass deposited ∝ charge passed; m = (E × I ×
t)/96500. Conductance: κ (kappa) = conductivity; Λ■ = molar conductivity = κ × 1000 / M. Kohlrausch’s law: Λ■° =
ν■λ■° + ν■λ■°. Strong electrolytes: Λ■ decreases slowly with √c; weak electrolytes show sharp rise on dilution.
Q1. The standard electrode potential of SHE is taken as:
A. +1.00 V
B. 0.00 V
C. –1.00 V
D. +0.76 V
✓ Correct Answer: B
Why this is correct: By convention the standard hydrogen electrode is assigned a potential of exactly 0.00 V at all
temperatures.
✗ Why the other options are wrong:
• A, C and D are potentials of other electrodes, not the reference value of SHE.
Q2. For the cell reaction Zn + Cu²■ → Zn²■ + Cu, if E°_cell = 1.10 V, the value of ∆G° is:
A. –212.3 kJ mol■¹
B. +212.3 kJ mol■¹
C. –106.15 kJ mol■¹
D. Zero
✓ Correct Answer: A
Why this is correct: n = 2. ∆G° = –nFE° = –2 × 96500 × 1.10 = –212300 J mol■¹ ≈ –212.3 kJ mol■¹.
✗ Why the other options are wrong:
• B has the wrong sign.
• C corresponds to n=1.
• D would mean E°=0.
Q3. Nernst equation for the electrode reaction M■■ + ne■ → M is:
A. E = E° + (0.059/n) log [M■■]
B. E = E° – (0.059/n) log [M■■]
C. E = E° + (0.059/n) log 1/[M■■]
D. E = E° – 0.059 log [M■■]
✓ Correct Answer: A
Why this is correct: E = E° – (0.059/n) log (1/[M■■]) which rearranges to E = E° + (0.059/n) log [M■■].
✗ Why the other options are wrong:
• B has the wrong sign.
• C is the same as A but written differently; the conventional form is A.
• D omits n.
Q4. In an electrolytic cell, the electrode at which oxidation occurs is called:
A. Cathode
B. Anode
C. Both
D. Neither
✓ Correct Answer: B
Why this is correct: Oxidation always occurs at the anode (whether the cell is galvanic or electrolytic).
✗ Why the other options are wrong:
• A is the site of reduction.
NEET 2027 | High-Weightage Chemistry | Part 2 Page 3
, • C and D are incorrect.
Q5. Faraday’s first law of electrolysis states that the mass of a substance deposited is proportional to:
A. Time only
B. Current only
C. Quantity of electricity passed
D. Resistance of the solution
✓ Correct Answer: C
Why this is correct: m ∝ Q (charge), where Q = I × t. Hence mass is proportional to the total quantity of electricity passed.
✗ Why the other options are wrong:
• A and B are incomplete.
• D does not appear in Faraday’s law.
Q6. The amount of electricity required to deposit 1 mol of Al from Al³■ is:
A. 1 F
B. 2 F
C. 3 F
D. 0.5 F
✓ Correct Answer: C
Why this is correct: Al³■ + 3e■ → Al. Three moles of electrons (3 F) are required to deposit 1 mol of Al.
✗ Why the other options are wrong:
• A and B are insufficient charge.
• D is far too little.
Q7. Molar conductivity of a strong electrolyte:
A. Increases sharply with dilution
B. Decreases with dilution
C. Increases slowly with dilution and approaches a limiting value
D. Remains constant
✓ Correct Answer: C
Why this is correct: For strong electrolytes Λ■ increases slowly on dilution because of decrease in inter-ionic attraction and
approaches Λ■° at infinite dilution.
✗ Why the other options are wrong:
• A describes weak electrolytes.
• B is opposite of the observed trend.
• D is incorrect.
Q8. Kohlrausch’s law is used to determine Λ■° of:
A. Only strong electrolytes
B. Only weak electrolytes
C. Both strong and weak electrolytes
D. Only solids
✓ Correct Answer: C
Why this is correct: Kohlrausch’s law of independent migration of ions allows calculation of Λ■° for both strong and weak
electrolytes from ionic conductivities.
✗ Why the other options are wrong:
• A and B are incomplete.
• D is irrelevant.
Q9. The SI unit of conductivity (κ) is:
A. S m■¹
B. S m² mol■¹
C. S cm² mol■¹
NEET 2027 | High-Weightage Chemistry | Part 2 Page 4
HIGH-WEIGHTAGE CHEMISTRY
PART 2
ELECTROCHEMISTRY • KINETICS • SOLUTIONS COORDINATION COMPOUNDS • GOC •
HYDROCARBONS
150 Unique High-Probability Practice Questions
Accurate • Most Expected in NEET 2027 • Professional
Special Features
✓ 150 fresh questions – no overlap with Part 1
✓ Topics with highest chance of appearing in NEET 2027
✓ Short theory + detailed why-correct / why-wrong
✓ Numerical + conceptual mix as per latest pattern
✓ Professional colourful layout for focused study
, CONTENTS
1. Electrochemistry — Theory + Q1 to Q30
2. Chemical Kinetics — Theory + Q31 to Q55
3. Solutions — Theory + Q56 to Q80
4. Coordination Compounds — Theory + Q81 to Q105
5. General Organic Chemistry + Hydrocarbons — Theory + Q106 to Q150
Quick Revision Sheet — Last page
How to Use
1. Read the short theory first.
2. Attempt questions without looking at answers.
3. Study both why the correct option is right and why others are wrong.
4. Revise the formula sheet before the exam.
NEET 2027 | High-Weightage Chemistry | Part 2 Page 2
, 1. ELECTROCHEMISTRY
Electrochemical cells convert chemical energy into electrical energy (Galvanic) or vice versa (Electrolytic).
Standard electrode potential E° is measured with respect to SHE (E° = 0). Nernst equation: E = E° – (RT/nF) ln Q =
E° – (0.059/n) log Q at 298 K. ∆G° = –nFE°_cell. Faraday’s laws: mass deposited ∝ charge passed; m = (E × I ×
t)/96500. Conductance: κ (kappa) = conductivity; Λ■ = molar conductivity = κ × 1000 / M. Kohlrausch’s law: Λ■° =
ν■λ■° + ν■λ■°. Strong electrolytes: Λ■ decreases slowly with √c; weak electrolytes show sharp rise on dilution.
Q1. The standard electrode potential of SHE is taken as:
A. +1.00 V
B. 0.00 V
C. –1.00 V
D. +0.76 V
✓ Correct Answer: B
Why this is correct: By convention the standard hydrogen electrode is assigned a potential of exactly 0.00 V at all
temperatures.
✗ Why the other options are wrong:
• A, C and D are potentials of other electrodes, not the reference value of SHE.
Q2. For the cell reaction Zn + Cu²■ → Zn²■ + Cu, if E°_cell = 1.10 V, the value of ∆G° is:
A. –212.3 kJ mol■¹
B. +212.3 kJ mol■¹
C. –106.15 kJ mol■¹
D. Zero
✓ Correct Answer: A
Why this is correct: n = 2. ∆G° = –nFE° = –2 × 96500 × 1.10 = –212300 J mol■¹ ≈ –212.3 kJ mol■¹.
✗ Why the other options are wrong:
• B has the wrong sign.
• C corresponds to n=1.
• D would mean E°=0.
Q3. Nernst equation for the electrode reaction M■■ + ne■ → M is:
A. E = E° + (0.059/n) log [M■■]
B. E = E° – (0.059/n) log [M■■]
C. E = E° + (0.059/n) log 1/[M■■]
D. E = E° – 0.059 log [M■■]
✓ Correct Answer: A
Why this is correct: E = E° – (0.059/n) log (1/[M■■]) which rearranges to E = E° + (0.059/n) log [M■■].
✗ Why the other options are wrong:
• B has the wrong sign.
• C is the same as A but written differently; the conventional form is A.
• D omits n.
Q4. In an electrolytic cell, the electrode at which oxidation occurs is called:
A. Cathode
B. Anode
C. Both
D. Neither
✓ Correct Answer: B
Why this is correct: Oxidation always occurs at the anode (whether the cell is galvanic or electrolytic).
✗ Why the other options are wrong:
• A is the site of reduction.
NEET 2027 | High-Weightage Chemistry | Part 2 Page 3
, • C and D are incorrect.
Q5. Faraday’s first law of electrolysis states that the mass of a substance deposited is proportional to:
A. Time only
B. Current only
C. Quantity of electricity passed
D. Resistance of the solution
✓ Correct Answer: C
Why this is correct: m ∝ Q (charge), where Q = I × t. Hence mass is proportional to the total quantity of electricity passed.
✗ Why the other options are wrong:
• A and B are incomplete.
• D does not appear in Faraday’s law.
Q6. The amount of electricity required to deposit 1 mol of Al from Al³■ is:
A. 1 F
B. 2 F
C. 3 F
D. 0.5 F
✓ Correct Answer: C
Why this is correct: Al³■ + 3e■ → Al. Three moles of electrons (3 F) are required to deposit 1 mol of Al.
✗ Why the other options are wrong:
• A and B are insufficient charge.
• D is far too little.
Q7. Molar conductivity of a strong electrolyte:
A. Increases sharply with dilution
B. Decreases with dilution
C. Increases slowly with dilution and approaches a limiting value
D. Remains constant
✓ Correct Answer: C
Why this is correct: For strong electrolytes Λ■ increases slowly on dilution because of decrease in inter-ionic attraction and
approaches Λ■° at infinite dilution.
✗ Why the other options are wrong:
• A describes weak electrolytes.
• B is opposite of the observed trend.
• D is incorrect.
Q8. Kohlrausch’s law is used to determine Λ■° of:
A. Only strong electrolytes
B. Only weak electrolytes
C. Both strong and weak electrolytes
D. Only solids
✓ Correct Answer: C
Why this is correct: Kohlrausch’s law of independent migration of ions allows calculation of Λ■° for both strong and weak
electrolytes from ionic conductivities.
✗ Why the other options are wrong:
• A and B are incomplete.
• D is irrelevant.
Q9. The SI unit of conductivity (κ) is:
A. S m■¹
B. S m² mol■¹
C. S cm² mol■¹
NEET 2027 | High-Weightage Chemistry | Part 2 Page 4
