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Get Thermodynamics MCQs for NEET Chemistry
Question: In thermodynamics a process is called reversible when
- a) System and surrounding change into each other
- b) There is no boundary between system and surrounding
- c) The surroundings are always in equilibrium with the system
- d) The system changes into the surroundings spontaneously
Answer: The surroundings are always in equilibrium with the system
Question: The molar heat capacity of water at constant pressur e P is 75 J K–1 mol–1. When 1.0 kJ of heat is supplied to 1000 g of water, which is free to expand, the increase in temperature of water is
- a) 1.2 K
- b) 2.4 K
- c) 4.8 K
- d) 0.24 K
Answer: 0.24 K
Question: 16 kg oxygen gas expands at STP (1 atm) isobarically to occupy double of its original volume. The work done during the process is nearly
- a) 260 kcal
- b) 180 kcal
- c) 130 kcal
- d) 271 kcal
Answer: 271 kcal
Question: The enthalpy and entropy change for a chemical reaction are –2.5 × 103 cal and 7.4 cal K–1 respectively. Predict the nature of reaction at 298 K is
- a) Spontaneous
- b) Reversible
- c) Irreversible
- d) Non-spontaneous
Answer: Spontaneous
Question: The temperature at which the given reaction is at equilibrium
- a) 462.12 K
- b) 362.12 K
- c) 262.12 K
- d) 562.12 K
Answer: 462.12 K
Question: One mole of a non ideal gas undergoes a change of state (2.0 atm, 3.0 L, 95 K) → (4.0 atm, 5.0 L, 245 K) with a change in internal energy ΔU = 30.0 L atm. The change in enthalpy of the process in L atm is
- a) 40.0
- b) 42.3
- c) 44.0
- d) 56.0
Answer: 44.0
Question: In an insulated container water is stirred with a rod to increase the temperature. Which of the following is true?
- a) ΔU = W ≠0, q = 0
- b) ΔU = W = q ≠ 0
- c) ΔU = 0, W = q ≠ 0
- d) W = 0, ΔU = q ≠0
Answer: ΔU = W ≠0, q = 0
Question: Two atoms of hydrogen combine to form a molecule of hydrogen gas the energy of the H2 molecule is
- a) Greater than that of separate atoms
- b) Equal to that of separate atoms
- c) Lower than that of separate atoms
- d) Sometimes lower and sometimes higher
Answer: Lower than that of separate atoms
Question: The temperature of 15 ml of a strong acid increases by 2°C when 15 ml of a strong base is added to it. If 5 ml of each are mixed, temperature should increase by
- a) 0.6°C
- b) 0.3°C
- c) 2°C
- d) 6°C
Answer: 2°C
Question: The standard heat of formation of NO2(g) and N2O4(g) are 8.0 and 4.0 kcal mol–1 respectively. The heat of dimerisation of NO2 in kcal is
- a) –12 kcal
- b) 12 kcal
- c) 4 kcal
- d) 16 kcal
Answer: –12 kcal
Question: If 
Then heat change during reaction of metal X with one mole of O2 to form oxide to maximum extent is
- a) 360 kJ
- b) –360 kJ
- c) –180 kJ
- d) +180 kJ
Answer: –360 kJ
Question: For a gaseous reaction :
ΔE is 17 kcal at 27°C. Assuming R = 2 cal K–1 mol–1 the value of ΔH for the above reaction will be
- a) 15.8 kcal
- b) 16.4 kcal
- c) 18.2 kcal
- d) 20.0 kcal
Answer: 18.2 kcal
Question: A mixture of 2 mole of CO and 1 mol of O2 is ignited. Correct relationship is
- a) ΔH = ΔU
- b) ΔH > ΔU
- c) ΔH < ΔU
- d) The relationship depends upon the capacity of vessel
Answer: ΔH < ΔU
Question: Bond dissociation energy of XY, X2 and Y2(all diatomic molecules) are in the ratio of 1 : 1 : 0.5 and ΔHf of XY is –200 kJ mol–1. The bond dissociation energy of X2 will be
- a) 800 kJ mol–1
- b) 200 kJ mol–1
- c) 300 kJ mol–1
- d) 400 kJ mol–1
Answer: 800 kJ mol–1
Question: Vapour density of a gas is 8. Its molecular mass will be
- a) 8
- b) 16
- c) 32
- d) 64
Answer: 16
More Questions...........................................
Question: If x mole of ideal gas at 27°C expands isothermally and reversibly from a volume of y to 10y, then the work done is
- a) w = x R 300 ln y
- b)
- c) w = – 300x R ln 10
- d)
Answer: w = – 300x R ln 10
Question: Enthalpy of formation of NH3 is – X kJ and ΔHH–H, ΔHN–H are respectively Y kJ mol–1 and ΔZ kJ mol–1. The value of ΔHN ≡ N is
- a)
- b) – 3Y + 6Z – 2X
- c) 3Y + 6Z + X
- d) Y + 6X + Z
Answer: – 3Y + 6Z – 2X
Question: A system X undergoes following changes
The overall process may be called as
- a) Reversible process
- b) Cyclic process
- c) Cyclic reversible process
- d) Isochoric process
Answer: Cyclic process
Question: The heat of neutralisation for strong acid and strong base forming 2 moles of water is
- a) – 2 × 57.1 kJ
- b) – 57.1 kJ
- c)
- d) Strong acid and strong base will not undergo neutralisation
Answer: – 2 × 57.1 kJ
Question: The value of ΔH° in kJ for the reaction will be
- a) x + 4y – z – 2r
- b) r + z + 4y – x
- c) 2r + z + 4y + x
- d) x + 4y + z – 2r
Answer: x + 4y + z – 2r
Question: The heat liberated on complete combustion of 1 mole of CH4 gas to CO2 (g) and H2O(l) is 890 kJ. Calculate the heat evolved by 2.4 L of CH4 on complete combustion.
- a) 95.3 kJ
- b) 8900 kJ
- c) 890 kJ
- d) 8.9 kJ
Answer: 95.3 kJ
Question: The work done in an open vessel at 300 K, when 112 g iron reacts with dil HCl to give FeCl2 , is nearly
- a) 1.1 kcal
- b) 0.6 kcal
- c) 0.3 kcal
- d) 0.2 kcal
Answer: 1.1 kcal
Question: Which statement is correct?
- a)
- b)
- c)
- d) All of these
Answer:
Question: A schematic representation of enthalpy changes for the 
reaction, is given below.
The missing value is
- a) + 10.5 kJ
- b) – 11.05 kJ
- c) – 110.5 kJ
- d) – 10.5 J
Answer: – 110.5 kJ
Question: Which of the following equations represent standard heat of formation of CH4?
- a) C(diamond)+ 2H2(g) → CH4(g)
- b) C(graphite)+ 2H2(g) → CH4(g)
- c) C(diamond)+ 4H(g) → CH4(g)
- d) C(graphite)+ 4H(g) → CH4(g)
Answer: C(graphite)+ 2H2(g) → CH4(g)
Question: Different types of systems are given below
The A and B systems respectively are
- a) Open system, Closed system
- b) Isolated system, Closed system
- c) Adiabatic system, Isolated system
- d) Closed system, Isolated system
Answer: Closed system, Isolated system
Question: Set of intensive properties is shown by
- a) Mole fraction, standard electrode potential, heat capacity
- b) Viscosity, refractive index, specific heat
- c) Density, Gibbs free energy, internal energy
- d) Number of moles, molarity, electrode potential
Answer: Viscosity, refractive index, specific heat
Question: For the expansion occurring from initial to final stage in finite time, which is incorrect?
- a) Equilibrium exist in initial and final stage
- b) Work obtained is maximum
- c) Driving force is much greater than the opposing force
- d) Both (1) & (2)
Answer: Work obtained is maximum
Question: The enthalpy of fusion of water is 1.435 kcal/mol. The molar entropy change for the melting of ice at 0°C is
- a) 5.260 cal/(mol K)
- b) 0.526 cal/(mol K)
- c) 10.52 cal/(mol K)
- d) 21.04 cal/(mol K)
Answer: 5.260 cal/(mol K)
Question: Three moles of an ideal gas expanded spontaneously into vacuum. The work done will be
- a) Infinite
- b) 3 Joules
- c) 9 Joules
- d) Zero
Answer: Zero
Question: Which of the following are not state functions ? (I) q + w (II) q (III) w (IV) H-TS
- a) (II) and (III)
- b) (I) and (IV)
- c) (II), (III) and (IV)
- d) (I), (II) and (III)
Answer: (II) and (III)
Question: Given that bond energies of H–H and Cl – Cl are 430 kJ/mol and 240 kJ/mol respectively and ΔfH of HCl is –90kJ/mol. Bond enthalpy of HCl is
- a) 245 kJ mol–1
- b) 2909 kJ mol–1
- c) 380 kJ mol–1
- d) 425 kJ mol–1
Answer: 425 kJ mol–1
Question: Which of the following pairs of a chemical reaction is certain to result in a spontaneous reaction ?
- a) Exothermic and decreasing disorder
- b) Endothermic and increasing disorder
- c) Exothermic and increasing disorder
- d) Endothermic and decreasing disorder
Answer: Exothermic and increasing disorder
Question: Identify the correct statement regarding entropy
- a) At absolute zero of temperature, the entropy of all crystalline substances is taken to be zero
- b) At absolute zero of temperature, the entropy of a perfectly crystalline substance is +ve
- c) At absolute zero of temperature, entropy of a perfectly crystalline substance is taken to be zero
- d) At 0°C, the entropy of a perfectly crystalline substance is taken to be zero
Answer: At absolute zero of temperature, entropy of a perfectly crystalline substance is taken to be zero
Question: One mole of an ideal gas at 300 K is expanded isothermally from an initial volume of 1 litre to 10 litres. The ΔE for this process is (R = 2 cal. Mol–1K–1)
- a) 1381.1 cal
- b) Zero
- c) 163.7 cal
- d) 9 L atm
Answer: Zero
Question: At 27°C latent heat of fusion of a compound is 2930 J/mol. Entropy change is
- a) 9.77 J/mol·K
- b) 10.77 J/mol·K
- c) 9.07 J/mol·K
- d) 0.977 J/mol·K
Answer: 9.77 J/mol·K
Question: When 1 mol of gas is heated at constant volume temperature is raised from 298 to 308 K. Heat supplied to the gas is 500 J. Then which statement is correct?
- a) q = ΔU = –500 J, w = 0
- b) q = ΔU = 500 J, w = 0
- c) q = w = 500 J, ΔU = 0
- d) ΔU = 0, q = w = –500 J
Answer: q = ΔU = 500 J, w = 0
Question: Enthalpy of 
is negative. If enthalpy of combustion of CH4 and CH3OH are x and y respectively. Then which relation is correct?
- a) x > y
- b) x < y
- c) x = y
- d) x ≥ y
Answer: x > y
Question: Unit of entropy is
- a) JK–1 mol–1
- b) J mol–1
- c) J–1 K–1 mol–1
- d) JK mol–1
Answer: JK–1 mol–1
Question: In a closed insulated container a liquid is stirred with a paddle to increase the temperature which of the following is true?
- a) ΔE = W ≠ 0, q = 0
- b) ΔE = W = q ≠ 0
- c) ΔE = 0, W = q ≠0
- d) W = 0, ΔE = q ≠0
Answer: ΔE = W ≠ 0, q = 0
Question: 2 mole of ideal gas at 27°C temperature is expanded reversibly from 2 lit. to 20 lit. Find entropy change (R =2 cal/mol K)
- a) 92.1
- b) 0
- c) 4
- d) 9.2
Answer: 9.2
Question: What is the entropy change (in JK–1 mol–1) when one mole of ice is converted into water at 0°C? (The enthalpy change for the conversion of ice to liquid water is 6.0 kJ mol–1 at 0°C)
- a) 20.13
- b) 2.013
- c) 2.198
- d) 21.98
Answer: 21.98
Question: The molar heat capacity of water at constant pressure, C, is 75 J K–1 mol–1. When 1.0 kJ of heat is supplied to 100 g of water which is free to expand, the increase in temperature of water is
- a) 1.2 K
- b) 2.4 K
- c) 4.8 K
- d) 6.6 K
Answer: 2.4 K
Question: The work done during the expansion of a gas from a volume of 4 dm3 to 6 dm3 against a constant external pressure of 3 atm is (1 L atm = 101.32 J)
- a) –6 J
- b) –608 J
- c) +304 J
- d) –304 J
Answer: –608 J
Question: Three moles of an ideal gas expanded spontaneously into vacuum. The work done will be
- a) Infinite
- b) 3 Joules
- c) 9 Joules
- d) Zero
Answer: Zero
Question: The enthalpy of fusion of water is 1.435 kcal/mol. The molar entropy change for the melting of ice at 0°C is
- a) 5.260 cal/(mol K)
- b) 0.526 cal/(mol K)
- c) 10.52 cal/(mol K)
- d) 21.04 cal/(mol K)
Answer: 5.260 cal/(mol K)
Question: The enthalpy of hydrogenation of cyclohexene is –119.5 kJ mol–1. If resonance energy of benzene is –150.4 kJ mol–1, its enthalpy of hydrogenation would be
- a) –358.5 kJ mol–1
- b) –508.9 kJ mol–1
- c) –208.1 kJ mol–1
- d) –269.9 kJ mol–1
Answer: –208.1 kJ mol–1
Question: The work done during the expansion of a gas from a volume of 4 dm3 to 6 dm3 against a constant external pressure of 3 atm is (1 L atm = 101.32 J)
- a) –6 J
- b) –608 J
- c) +304 J
- d) –304 J
Answer: –608 J
Question: The molar heat capacity of water at constant pressure, C, is 75 J K–1 mol–1. When 1.0 kJ of heat is supplied to 100 g of water which is free to expand, the increase in temperature of water is
- a) 1.2 K
- b) 2.4 K
- c) 4.8 K
- d) 6.6 K
Answer: 2.4 K
Question: What is the entropy change (in JK–1 mol–1) when one mole of ice is converted into water at 0°C? (The enthalpy change for the conversion of ice to liquid water is 6.0 kJ mol–1 at 0°C)
- a) 20.13
- b) 2.013
- c) 2.198
- d) 21.98
Answer: 21.98
Question: Heat of combustion for C(s), H2(g) and CH4(g) are –94, –68 and –213 kcal/mol, then ΔH forC(s) + 2H2(g) → CH4(g) is
- a) –17 kcal
- b) –111 kcal
- c) –170 kcal
- d) –85 kcal
Answer: –17 kcal
Question: 2 mole of ideal gas at 27°C temperature is expanded reversibly from 2 lit. to 20 lit. Find entropy change (R =2 cal/mol K)
- a) 92.1
- b) 0
- c) 4
- d) 9.2
Answer: 9.2
Question: For the reaction
,which one is true?
- a) ΔH = ΔE – RT
- b) ΔH = ΔE + RT
- c) ΔH = ΔE + 2RT
- d) ΔH = ΔE – 2RT
Answer: ΔH = ΔE – RT
Question: In the reaction : S + 3/2 O2→ SO3+ 2x kcal and SO2+ 1/2 O2→SO3+ y kcal, the heat of formation of SO2 is
- a) (2x + y)
- b) (x – y)
- c) (x + y)
- d) (y – 2x)
Answer: (y – 2x)
Question:
What is heat of formation of CO?
- a)
- b) 2x – y
- c) y – 2x
- d)
Answer:
Question: For a reaction to occur spontaneously
- a) ΔH must be negative
- b) ΔS must be negative
- c) (ΔH – TΔS) must be negative
- d) (ΔH + TΔS) must be negative
Answer: (ΔH – TΔS) must be negative
Question: Which reaction, with the following values of ΔH, ΔS, at 400 K is spontaneous and endothermic?
- a) ΔH = –48 kJ; ΔS = + 135 J/K
- b) ΔH = –48 kJ; ΔS = – 135 J/K
- c) ΔH = +48 kJ; ΔS = + 135 J/K
- d) ΔH = +48 kJ; ΔS = – 135 J/K
Answer: ΔH = +48 kJ; ΔS = + 135 J/K
Question: Which of the following pairs of a chemical reaction is certain to result in a spontaneous reaction ?
- a) Exothermic and decreasing disorder
- b) Endothermic and increasing disorder
- c) Exothermic and increasing disorder
- d) Endothermic and decreasing disorder
Answer: Exothermic and increasing disorder
Question: Three moles of an ideal gas expanded spontaneously into vacuum. The work done will be
- a) Infinite
- b) 3 Joules
- c) 9 Joules
- d) Zero
Answer: Zero
Question: For the gas phase reaction,
which of the following conditions is correct ?
- a) ΔH > 0 and ΔS < 0
- b) ΔH = 0 and ΔS < 0
- c) ΔH > 0 and ΔS > 0
- d) ΔH < 0 and ΔS < 0
Answer: ΔH > 0 and ΔS > 0
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FAQs
You can get most exhaustive NEET Chemistry Thermodynamics MCQs Set 02 for free on StudiesToday.com. These MCQs for NEET Chemistry are updated for the 2026-27 academic session as per NEET examination standards.
Yes, our NEET Chemistry Thermodynamics MCQs Set 02 include the latest type of questions, such as Assertion-Reasoning and Case-based MCQs. 50% of the NEET paper is now competency-based.
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