Students of class 11 Chemistry should refer to MCQ Questions Class 11 Chemistry Thermodynamics with answers provided here which is an important chapter in Class 11 Chemistry NCERT textbook. These MCQ for Class 11 Chemistry with Answers have been prepared based on the latest CBSE and NCERT syllabus and examination guidelines for Class 11 Chemistry. The following MCQs can help you to practice and get better marks in the upcoming class 11 Chemistry examination

Chapter 6 Thermodynamics MCQ with Answers Class 11 Chemistry

MCQ Questions Class 11 Chemistry Thermodynamics provided below have been prepared by expert teachers of grade 11. These objective questions with solutions are expected to come in the upcoming Standard 11 examinations. Learn the below provided MCQ questions to get better marks in examinations.

Question. For a particular reversible reaction at temperature T, ΔH and ΔS were found to be both positive. IfTe is the temperature at equilibrium, the reaction would be spontaneous when
(a) T_e > T
(b) T > T_e 
(c) T_e is 5 times T
(d) T = T_e 

Question. For the process,
        H₂O (l) (1 bar, 273 K)→H₂O(g) (1 bar, 373 K),
The correct set of thermodynamic parameters is
(a) ΔG = 0,ΔS = + ve
(b) ΔG = 0, ΔS = −ve
(c) ΔG = + ve,ΔS = 0
(d) ΔG = −ve,ΔS = + ve

Question.  Which of the following statement is correct?
(a) The presence of reacting species in a covered beaker is an example of open system
(b) There is an exchange of energy as well as matter between the system and the surroundings in a closed system
(c) The presence of reactants in a closed vessel made up of copper is an example of a closed system
(d) The presence of reactants in a thermos flask or any other closed insulated vessel is an example of a closed system

Question.  When 1 mole of a gas is heated at constant volume, temperature is raised from 298 K to 308 K. Heat supplied to the gas is 500 J. Then, which statement is correct?
(a) q = −W = 500 J, DE =0
(b) q =W = 500 J, DE =0
(c) q = DE = 500 J, W =0
(d) DE = 0, q =W = −500 J

Question. In an adiabatic process, no transfer of heat takes place between system and surroundings. Choose the correct option for free expansion of an ideal gas under adiabatic condition from the following.
(a) q = 0, DT ¹ 0,W = 0
(b) q ≠ 0, DT = 0,W = 0
(c) q = 0, DT = 0,W = 0
(d) q = 0, DT < 0,W ¹ 0

Question.  Heat required to raise the temperature of 1 mole of a substance by 1°C is called
(a) specific heat
(b) molar heat capacity
(c) water equivalent
(d) specific gravity

Question.  The molar heat capacity of water at constant pressure is 75 J K ⁻¹mol ⁻¹. When 1.0 kJ of heat is supplied to100 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) 6.8 K

Question. 1 mole of an ideal gas at 300 K is expanded isothermally from an initial volume of 1 L to 10 L. The DE for this process is (R = 2 cal K⁻¹ mol⁻¹ ) 
(a) 270 cal
(b) zero
(c) 10 L atm
(d) 181.7 cal

Question. ΔU is equal to
(a) isochoric work
(b) isobaric work
(c) adiabatic work
(d) isothermal work

Question. (ΔH − ΔE ) for the formation of carbon monoxide (CO) from its elements at 298 K is (R = 8.314 JK⁻¹ mol⁻¹ ) 
(a) −2477.57 J mol⁻¹
(b) 2477.57 Jmol ⁻¹
(c) –1238.78 Jmol ⁻¹
(d) 1238.78 Jmol ⁻¹

Question. The pressure-volume work for an ideal gas can be calculated by using the expression W = ∫^Vf_Vi pexdv. The work can also be calculated from the pV − plot by using the area under the curve within the specified limits. When an ideal gas is compressed (a) reversibly or (b) irreversibly from volumeVi toVt . Choose the correct option.
(a) W(reversible) = W _{(irreversible)} 
(b) W(reversible) < W_{(irreversible)}  
(c) W(reversible) >W_{(irreversible)}  
(d) W(reversible) = W_{(irreversible)}+p_ex V

Question. An ideal gas expands in volume from1 ×10⁻³ m³ to 1 × 10⁻² m³ at 300 K against a constant  ressure of 1 × 10⁵ N/m². The work done is
(a) −900 J
(b) −900 kJ
(c) 270 kJ
(d) 900 kJ

Question. If ΔE is the h eat of reaction for
C₂H₅OH(l)+ 3O₂ (g) → 2CO₂ (g)+ 3H₂O(l)
at constant volume, then ΔH (heat of reaction at constant pressure), at constant temperature is 
(a) ΔH = ΔE + RT
(b) ΔH = ΔE -RT
(c) ΔH = ΔE -2RT
(d) ΔH = ΔE + 2RT     

Question. If one mole of ammonia and one mole of hydrogen chloride are mixed in a closed container to form ammonium chloride gas, then 
(a) ΔH > ΔU
(b) ΔH = ΔU
(c) ΔH < ΔU
(d) there is no relationship       

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 
(a) – 6 J
(b) – 6081
(c) + 304 J
(d) – 304 J       

Question. If the bond energies of H—H, Br—Br and H—Br are 433, 192 and 364 kJ mol^-1 respectively, then  ΔH°  for the reaction H₂ (g) + Br₂ (g) → 2HBr(g) is 
(a) – 261 kJ
(b) + 103 kJ
(c) + 261 kJ
(d) – 103 kJ       

Question. The bond energy is the energy required to 
(a) dissociate one mole of the substance
(b) dissociate bond in 1 kg of the substance
(c) break one mole of similar bonds
(d) break bonds in one mole of substance       

Question. For the reaction, 2H₂ (g) + O₂ (g) → 2H2 O(g);
                                                          ΔH = -573.2kJ
The heat of decomposition of water per mole is
(a) 286.6 kJ
(b) 573.2 kJ 
(c) -28.66 kJ
(d) zero       

Question. For an ideal gas, the heat of reaction at constant pressure and constant volume are related as 
(a) H + E = pV
(b) E = H + pΔV
(c) q_P = q_v + ΔnRT
(d) None of these         

Question. If at 298 K the bond energies of C—H, C—C, C = C and H—H bonds are respectively 414, 347, 615 and 435 kJ mol^-1, then value of enthalpy change for the reaction, H₂C= CH₂(g) + H₂(g) → H₃C—CH₃ (g) at 298 K will be 
(a) +250 kJ
(b) – 250 kJ
(c) + 125 kJ
(d) – 125 kJ       

Question. The relation between Wand AU is
(a) ΔH = ΔU+RT
(b) ΔH = ΔU – ΔnRT
(c) ΔH = ΔU + ΔnRT
(d) ΔU = ΔH + ΔnRT         

Question. Consider the reaction, N₂ + 3H₂ → 2NH₃ carried out at constant temperature and pressure. If Wand AU are the enthalpy and internal energy changes for the reaction, which of the following expressions is true ? 
(a) ΔH > ΔU
(b) ΔH < ΔU
(c) ΔH = ΔU
(d) ΔH = 0   

Question. The entropy change involved in the isothermal reversible expansion of 2 moles ofan ideal gas from a volume of 10 dm³ to a volume of 100 dm³ at 27°C is
(a) 38.3 J mol^-1 K^-1
(b) 35.8J mol^-1 K^-1
(c) 32.3 J mol^-1 K^-1
(d) 42.3 J mol^-1 K^-1       

Question. The entropy of a perfectly crystalline material is zero at 0°C. This is statement of 
(a) first law of thermodynamics
(b) second law of thermodynamics
(c) third law of thermodynamics
(d) law of conservation of energy     

Question. In view of the signs of Δ_rG° for the following reactions
            PbO₂ + Pb → 2PbO, Δ_rG° < 0,
           SnO₂ + Sn → 2SnO, Δ_rG° > 0,
Which oxidation states are more characteristic for lead and tin ? 
(a) For lead + 4, for tin + 2
(b) For lead + 2, for tin + 2
(c) For lead + 4, for tin + 4
(d) For lead + 2, for tin + 4     

Question. For the reversible reaction, A(s) + B(g) → C(g) + D(g); ΔG° =- 350kJ, which one of the following statements is true ? 
(a) The reaction is thermodynamically non-feasible
(b) The entropy change is negative
(c) Equilibrium constant is greater than one
(d) The reaction should be instantaneous     

Question. In any chemical reaction, a quantity that decrease to a minimum is 
(a) free energy
(b) entropy
(c) temperature
(d) enthalpy     

Question. Carbon cannot reduce Fe₂O₃ to Feat a temperature below 983 K because 
(a) free energy change for the formation of CO is more negative than that of Fe₂O₃
(b) CO is thermodynamically more stable than Fe₂O₃
(c) carbon has higher affinity towards oxygen than iron
(d) iron has higher affinity towards oxygen than carbon     

Question. In evaporation of water ΔH and ΔS are
(a) + ,+
(b) +, –
(c) – , –
(d) – , + 

Question. ΔG for the reaction Ag₂O ➔ 2Ag + 1/2 O₂ at a certain 2 temperature is found to be -10.0kJ moI^{– 1} , which one of the following statements is correct at this temperature ?
(a) Silver oxide decomposes to give silver and oxygen
(b) Silver and oxygen combine to form silver oxide
(c) The reaction is in equilibrium
(d) The reaction can neither occur in the forward direction nor in the backward direction       

Question. For the reaction at 298 K. A (g) + B(g) → C(g) ΔE = -5 cal and ΔS = -10 cal K^-1 
(a) ΔG = + 2612cal
(b) ΔG = – 2612cal
(c) ΔG = + 261.2 cal
(d) None of these     

Question. Which of the following is correct for the reaction ΔH= + ve and ΔS = + ve?
(a) Spontaneous at high temperature
(b) Spontaneous at low temperature
(c) Non-spontaneous at high temperature
(d) Non-spontaneous at all temperatures   

Question. For the reaction CO(g) + 1/2 O₂ (g) → CO₂ (g ), CO₂ and ΔS are – 283 kJ, – 87 JK^-1 , respectively. It was intended to carry out this reaction at 1000, 1500, 3000 and 3500 K. At which of these temperatures would this reaction be thermodynamically spontaneous? 
(a) 1500 and 3500 K
(b) 3000 and 3500 K
(c) 1000, 1500 and 3000 K
(d) 1500, 3000 and 3500 K   

Question. The direct conversion of A to B is difficult, hence it is canied out by the following shown path
               C → D
               ↑      ↓
               A     B
Given; ΔS (A ➔ C) = 50 eu
          ΔS (C ➔ D) = 30eu
          ΔS (B ➔ D) = 20eu
where eu is entropy unit, then ΔS _{(A ➔ B)} is 
(a) + lO0eu
(b) + 60eu
(c) – l00eu
(d) – 60eu   

Question. The enthalpy of vaporisation of benzene is + 35. 3 kJ/mol at its boiling point of 80°C. The entropy change in the transition of vapour to liquid at its boiling point is …. [in J mol^-1 K^-1].
(a) – 100
(b) +1 00
(c) +342
(d) – 342       

Question. What will be the value of ΔG for ice at 8°C temperature ?
(a) One
(b) Negative
(c) Positive
(d) Zero   

Question. If ΔG= 46.06 kcal / mol, K_P at 300 K is
(a) 10^-33.33
(b) 10^-23.03
(c) 10^-50.12
(d) 10^+33.33   

Question. Consider the reaction, N₂ + 3H² → 2NH₃ carried out at constant temperature and pressure. If ΔH and ΔE are the enthalpy and internal energy changes for the reaction, which of the following  expressions is true?
(a) ΔH > ΔE
(b) ΔH < ΔE
(c) ΔH =ΔE
(d) ΔH = 0

Question. The combustion of benzene (l ) gives CO₂(g) and H₂O(l ). Given that heat of combustion of enzene at constant volume is −3263 9 . kJ mol⁻¹ at 25° C; heat of combustion (in kJ mol⁻¹) of benzene at constant pressure will be (R = 8.314 JK⁻¹ mol)
(a) 4152.6
(b) −452.46
(c) 3260
(d) −3267.6

Question.  A piston filled with 0.04 mole of an ideal gas expands reversibly from 50.0 mL to 375 mL at a constant temperature of 37.0°C. As it does so, it absorbs 208 J ofnheat. The values of q and W for the process will be [R = 8.314 J/mol K) (ln 7.5 = 2.01)
(a) q = − 208 J,W = − 208 J
(b) q = − 208 J,W = + 208 J
(c) q = + 208 J,W = + 208 J
(d) q = + 208 J,W = − 208 J

Question. Latent heat of vaporisation of a liquid at 500 K and 1 atm pressure is 10.0 kcal/mol. What will be the change in internal energy (ΔE ) of 3 moles of liquid at same temperature?
(a) 30 kcal
(b) –54 kcal
(c) 27.0 kcal
(d) 50 kcal

Question. For two moles of an ideal gas
(a) (Cp CV ) = 2R
(b) (Cp CV ) = 0
(c) (Cp CV ) = R 
(d) (Cp CV ) = R/2

Question. The heat of sublimation of iodine is 24 cal g ⁻¹ at 50°C. If specific heat of solid iodine and its vapours are 0.055 and 0.031 cal g −1 respectively, the heat of sublimation of iodine at 100°C is
(a) 22.8 cal g ⁻¹
(b) 25.2 cal g ⁻¹
(c) –22.8 cal g ⁻¹
(d) –25.2 cal g ⁻

Question. For an isolated system, ΔE = 0, then
(a) ΔS = 0
(b) ΔS < 0
(c) ΔS > 0
(d) the value ofΔS cannot be predicted

Question. When 1.8 g of steam at the normal boiling point of water is converted into water, at the same  emperature, enthalpy and entropy changes respectively will be [Given, DH_vap for water = 40 8 . kJmol ⁻¹]
(a) −8.12 kJ, 11.89 JK⁻¹
(b) 10.25 kJ, 12.95 JK ⁻¹
(c) −4.08 kJ, − 10.93 JK⁻¹
(d) 10.93 kJ, − 4.08 JK ⁻¹

Question. In view of the signs of Dr G° for the following reactions
          PbO₂ + Pb → 2PbO, Δ,G° < 0 
          SnO₂ + Sn → 2SnO, Δ,G° > 0
(a) For lead + 4, for tin + 2
(b) For lead + 2 , for tin + 2
(c) For lead + 4, for tin + 4
(d) For lead + 2, for tin + 4

Question. When the heat of a reaction at constant pressure is − 2.5 × 10³ cal and entropy change for the reaction is 7.4 cal deg⁻¹, it is predicted that the reaction at 25°C is
(a) reversible
(b) spontaneous
(c) non-spontaneous
(d) irreversible

Question. For an isomerisation reaction A ⇔B, the temperature dependence of equilibrium constant is given by
      log_e K T = 4.0 − 2000/T
The value of ΔS° at 300 K is therefore,
(a) 4R
(b) 5 R
(c) 400R
(d) 2000R

Question.  Which of the following does not have zero entropy even at absolute zero?
           CO, CO₂, NaCl, NO
(a) CO, CO₂
(b) CO, NO
(c) CO₂, NaCl
(d) NaCl

Question. What will be the change of entropy DrS° at 298 K for the reaction, in which urea is formed fromNH₃ and CO₂?
2NH₃(g) + CO₂(g) → NH₂CONH₂(aq) + H₂O(l )
[Given, the standard entropy of NH₂CONH₂(aq),
CO₂(g),NH₃(g) and H₂O(l ) are 174.0, 213.7, 192.3 and 69.9 JK mol⁻¹ respectively]
(a) 200 JK⁻¹ mol⁻¹
(b) –35.44 JK⁻¹ mol⁻¹
(c) –354.4 JK⁻¹ mol⁻¹
(d) 425.2 JK⁻¹ mol⁻¹

Question. 2 moles of an ideal gas at 27°C are expanded reversibly from 2 L to 20 L. Find entropy change (in cal/mol K).
(R = 2 cal/mol K)
(a) 0
(b) 4
(c) 9.2
(d) 92. 0

Question. A Carnot engine operates between temperatureT and 400 K (T > 400 K). If efficiency of engine is 25%, the temperatureT is
(a) 666.0 K
(b) 498.5 K
(c) 533.3 K
(d) 500.0 K

Question. C_aCO₃ exists in two forms calcite and aragonite. The conversion of 1 mole of calcite to aragonite is
accompanied by internal energy change equal to + 0.21kJ. Given that the densities of calcite and aragonite are 2.71 cm⁻³ and 2.73 g cm⁻³ respectively. The enthalpy change at the pressure of 1.0 bar will be
(a) 200.72 J mol⁻¹
(b) 309.72 J mol⁻¹
(c) 209.72 J mol⁻¹
(d) 315.00 J mol⁻¹

Question. At 1 atmpressure, ΔS = 75 J K⁻¹ mol⁻¹ ; ΔH = 30 kJ mol⁻¹. The temperature of the reaction at equilibrium is
(a) 400K
(b) 330K
(c) 200K
(d) 110K

Question. The enthalpy of vaporisation of liquid diethyl ether (C₂ H₅ )₂O, is 26.0 kJmol⁻¹ at its boiling point (35°C). What will be the DS for conversion of liquid to vapour and vapour to liquid respectively?
(a) + 84.41and − 84.41 JK⁻¹ mo^l−1 
(b) + 80.90 and − 68.83 JK⁻¹ mol⁻¹ 
(c) − 84.41and + 90.63 JK⁻¹ mol⁻¹ 
(d) + 68.83 and − 84.41 JK⁻¹ mol⁻¹ 

Question. Identify the correct statement regarding a spontaneous process.
(a) For a spontaneous process in an isolated system, the change in entropy is positive
(b) Endothermic processes are never spontaneous
(c) Exothermic processes are always spontaneous
(d) Lowering of energy in the reaction process is the only criteria for spontaneity

Question. 1 kg block of ice at 0°C is placed into a perfectly insulated, sealed container that has 2 kg of water also at 0°C. The water and ice completely fill the container is flexible. After sometime one can except that
(a) the water will freeze so that the mass of the ice will increase
(b) the ice will melt so that the mass of ice will decrease
(c) both the amount of water and the amount of ice will remain constant
(d) both the amount of water and the amount of ice will decrease

Question. For the process, H₂O(l )→ H₂O (g)aT=100 °Cand 1 atmosphere pressure, the correct choice is 
(a) ΔS_system > 0 and ΔS_Surrounding > 0
(b) ΔS_system > 0 and ΔS_Surrounding < 0
(c) ΔS_system < 0 and ΔS_Surrounding > 0
(d) ΔS_system < 0 and ΔS_Surrounding < 0

Question. A reaction is non-spontaneous at the freezing point of water but is spontaneous at the boiling point of water, then
      ΔH        ΔS
(a) + ve     + ve
(b) − ve     − ve
(c) − ve     + ve
(d) + ve     − ve

Question. One mole of a liquid (1 bar, 100 mL) is taken in an adiabatic container and the pressure increases steeply to 100 bar. Then at constant pressure of 100 bar, volume decreases by 1 mL. DU and DH will be respectively.
(a) 10 J, 10 J
(b) 10 J, 0
(c) 0, 10 J
(d) 5 J, 10 J

Question. The value of log₁₀ K_C for a reaction A=B is [Given, Δ/H°_298K = −54.07kJ mol⁻¹
Δ,rS°_298K = 10 JK⁻¹ mol⁻¹ and R = 8.314 JK⁻¹ mol⁻¹ and 2.303 × 8.314 × 298 = 5705]
(a) 5
(b) 10
(c) 95
(d) 100

Question. When one mole of monoatomic ideal gas atT K undergoes adiabatic change under a constant external pressure of 1 atm, changes volume from1L to 2 L.The final temperature in Kelvin would be
(a) T/2^2/3 Z
(b) T +2/3× 0.0821
(c) T
(d) T − 2/3× 0.0821

uestion.  Water is brought to boil under a pressure of 1.0 atm. When an electric current of 0.50 A from a 12 V supply is passed for 300 s through a resistance in thermal contact with it, it is found that 0.798 g of water is vaporised. Calculate the molar internal energy change at boiling point (373.15 K).
(a) 37.5 kJ mol⁻¹
(b) 3.75 kJ mol⁻¹
(c) 42.6 kJ mol⁻¹
(d) 4.26 kJ mol⁻¹

Question. For a spontaneous reaction, the ΔG, equilibrium constant (K) and E °cell will be respectively
(a) − ve, > 1, − ve
(b) − ve, < 1, − ve
(c) + ve, > 1, − ve
(d) − ve, > 1, + ve

Question.  An ideal gas is allowed to expand both reversibly and irreversibly in an isolated system. IfTi is the initial temperature andTf is the final temperature, which of the following statement is correct?
(a) (T_f ) irrev > (T_f) rev 
(b)T_f> T_ff i > for reversible process, but T_f = T_f for irreversible process
(c) (T_f )rev > (T_f)irrev
(d) T_f = T_f  for both reversible and irreversible processes

Question. 1 mole of CO₂ gas at 300 K is expanded under adiabatic conditions such that its volume becomes 27 times. What is work done? (ϒ = 1.33 and C_V = 6 cal mol⁻¹ for CO₂)
(a) 900 cal
(b) 1000 cal
(c) 1200 cal
(d) 1400 cal

Question. A monoatomic ideal gas undergoes a process in which the ratio of p toV at any instant is constant and equals to 1. What is the molar heat capacity of the gas?
(a) 4R / 2
(b) 3R / 2
(c) 5R / 2
(d) Zero

Question.  A gas present in a cylinder, fitted with a frictionless piston, expands against a constant pressure of 1 atm from a volume of 2 litre to a volume of 6 litre. In doing so, it absorbs 800 J heat from surroundings. The increase in internal energy of process is
(a) 305.85 J
(b) 394.95 J
(c) 405.83 J
(d) –463.28 J

Question. Standard entropy of X2,Y2 and XY3 are 60, 40 and 50 JK −1mol −1 respectively. For the reaction,
      1/2_X2 +3/2_Y2 →XY₃, ΔH = − 30 kJ
to be at equilibrium, the temperature will be
(a) 750 K
(b) 1000 K
(c) 1250 K
(d) 500 K

Question. The entropy change involved in the isothermal reversible expansion of 2 moles of an ideal gas from a volume of 10 dm³ to a volume of100 dm³ at 27°C is
(a) 38.3 J mol⁻¹ K⁻¹
(b) 35.8 J mol⁻¹ K⁻¹
(c) 32.3 J mol⁻¹ K⁻¹
(d) 42.3 J mol⁻¹ K⁻¹

Question. Considering entropy (S) as a thermodynamic parameter, the criterion for the spontaneity of any process is
(a) ΔS_system + ΔS_surrounding be +ve
(b) ΔS_system be zero
(c) ΔS_system − ΔS_surrounding be + ve
(d) ΔS_surrounding be zero

We hope the above multiple choice questions for Class 11 Chemistry for Chapter 6 Thermodynamics provided above with answers based on the latest syllabus and examination guidelines issued by CBSE, NCERT and KVS are really useful for you. Thermodynamics is an important chapter in Class 11 as it provides very strong understanding about this topic. Students should go through the answers provided for the MCQs after they have themselves solved the questions. All MCQs have been provided with four options for the students to solve. These questions are really useful for the benefits of class 11 students. Please go through these and let us know if you have any feedback in the comments section.