MCQs For NCERT Class 11 Chemistry Chapter 6 Thermodynamics

MCQs Class 11

Please refer to the MCQ Questions for Class 11 Chemistry Chapter 6 Thermodynamics with Answers. The following Thermodynamics Class 11 Chemistry MCQ Questions have been designed based on the latest syllabus and examination pattern for Class 11. Our experts have designed MCQ Questions for Class 11 Chemistry with Answers for all chapters in your NCERT Class 11 Chemistry book.

Thermodynamics Class 11 MCQ Questions with Answers

See below Thermodynamics Class 11 Chemistry MCQ Questions, solve the questions and compare your answers with the solutions provided below.

Question. The densities of graphite and diamond at 298 K are 2.25 and 3.31 g cm–3, respectively. If the standard free energy difference (ΔG°) is equal to 1895 J mol–1, he pressure at which raphite will be transformed into diamond at 298 K is
(a) 9.92 × 108 Pa
(b) 9.92 × 107 Pa
(c) 9.92 × 106 Pa
(d) 9.92 × 105 Pa 

Answer

A

Question. Unit of entropy is
(a) J K–1 mol–1
(b) J mol–1
(c) J–1K–1 mol–1
(d) J K mol–1

Answer

A

Question. Cell reaction is spontaneous when
(a) ΔG° is negative
(b) ΔG° is positive
(c) ΔE°red is positive
(d) ΔE°red is negative.

Answer

A

Question. 2 moles 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

D

Question. PbO2 → PbO; ΔG298 < 0 SnO2 → SnO; ΔG298 > 0 Most probable oxidation state of Pb and Sn will be
(a) Pb4+, Sn4+
(b) Pb4+, Sn2+
(c) Pb2+, Sn2+
(d) Pb2+, Sn4+

Answer

D

Question. Following reaction occurring in an automobile 2C8H18(g) + 25O2(g) → 16CO2(g) + 18H2O(g) The sign of ΔH, ΔS and ΔG would be
(a) –, +, +
(b) +, +, –
(c) +, –, +
(d) –, +, –

Answer

D

Question. Thermodynamics is not concerned about____.
(a) energy changes involved in a chemical reaction.
(b) the extent to which a chemical reaction proceeds.
(c) the rate at which a reaction proceeds
(d) the feasibility of a chemical reaction.

Answer

C

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

C

Question. Which of the following statements 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.

Answer

C

Question. Which of the following is closed system ?
(a) Jet engine
(b) Tea placed in a steel kettle
(c) Pressure cooker
(d) Rocket engine during propulsion

Answer

C

Question. Heat of combustion of carbon monoxide at constant volume and at 17° C is -67710 cal. The heat of combustion at constant pressure is 
(a) – 68000 cal
(b) – 67800 cal
(c) – 67050 cal
(d) + 68500 cal     

Answer

A

Question. For N2 (g) + 3H2 (g) ⇔ 2NH3 (g ), AH is equal to
(a) ΔE + 2RT
(b) ΔE  – 2RT 
(c) ΔE  + RT
(d) ΔE  – RT     

Answer

B

Question. The standard molar heat of formation of ethane, CO2 and water (/) are – 21.1, – 94. land – 68.3 kcal, respectively. The standard molar heat of combustion of ethane will be
(a) – 372 kcal
(b) 162 kcal 
(c) – 240 kcal
(d) 183.5 kcal         

Answer

A

Question. A process is taking place at constant temperature and pressure. Then, 
(a) ΔH = ΔE
(b) ΔH = TΔS
(c) ΔH = 0
(d) ΔH = 0         

Answer

A

Question. For the gaseous reaction involving the complete combustion of iso-butane 
(a) ΔH = ΔE
(c) ΔH < ΔE
(b) ΔH > ΔE
(d) None of these     

Answer

B

Question. IfS + O2 → SO2; ΔH= – 298.2 kJ 
SO2 + 1/2 O2 → SO3; ΔH = – 98.7 kJ 
SO3 + H2O → H2SO4 ; ΔH = – 130.2 kJ 
H2 + 1/2 O2 → H2O; ΔH = – 287.3 kJ 
Then, the enthalpy of formation of H2SO4 at 298 K will be
(a) – 814.4 kJ
(b) + 320.5 kJ
(c) – 650.3 kJ
(d) – 933.7 kJ     

Answer

A

Question. The enthalpies of formation of Al2O3 and Cr2O3 are -1596 kJ and -1134 kJ respecti vet y. ΔH for the reaction, 2Al + Cr2O3 → 2Cr + Al2O3 is
(a) – 2730 kJ
(b) – 462 kJ
(c) – 1365 kJ
(d) + 2730 kJ       

Answer

B

Question. The quantity of heat measured for a reaction in a bomb calorimeter is equal to 
(a) ΔG
(b) ΔH
(c) pΔV
(d) ΔE       

Answer

D

Question. The beat of neutralisation of any strong acid and a strong base is nearly equal to 
(a) – 75.3 kJ
(b) + 57.3 kJ
(c) – 57.3 kJ
(d) + 75.3 kJ       

Answer

C

Question. For the reaction, 2H2 + O2 → 2H2O
ΔH = -571. Bond energy of H—H = 435, O = O = 498, then calculate the average bond energy of O—H bond using the above data 
(a) 484
(b) – 484
(c) 271
(d) – 271       

Answer

A

Question. For hydrogen-oxygen fuel cell at I atrn and 298 K 
H2 (g) + 1/2 O2 (g) → H2O(/); ΔG° = – 240 kJ 
E° for the cell is approximately, (Given F = 96500 C)
(a) 2.48 V
(b) 1.24 V 
(c) 2.5 V
(d) 1.26 V     

Answer

B

Question. ΔG° vs T plot in the Ellingham’s diagram slopes upwards for the reactions 
(a) Mg + 1/2 O2 → MgO
(b) 2Ag + 1/2 O2 → Ag2O
(c) C + 1/2 O2 → CO
(d) CO + 1/2 O2 → CO

Answer

C

Question. For a reaction to be spontaneous at all temperatures
(a) ΔG and ΔH should be negative
(b) ΔG and ΔH should be positive
(c) ΔG = ΔS = 0
(d) ΔH < ΔG   

Answer

A

Question. Which one of the following is spontaneous at all temperatures ? 
(a) H2 (g) → 2H(atom); 
                  ΔH° = 436 kJ, ΔS° = 90.7 eu 
(b) 1/2 N2 (g)+ 1/2 O2 (g) → NO(g); 
                                  ΔH° = 90.3 kJ, ΔS° = 3.0eu
(c) 2NO2 (g) → N2O4 (g); 
                      ΔH° = – 56.0 kJ, ΔS° = -17.7eU 1
(d) H2O2 (g) → H2O(/)+ 1/2 O2 (g); 
                                      ΔH° = -98.3 kJ, ΔS° = 80.0 eu 

Answer

D

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 criterion for spontaneity 

Answer

A

Question. ΔH and ΔS for a reaction are+ 30.558 kJ mol-1 and 0.066 kJ K-1 mol-1 at l atm pressure. The temperature at which free energy change is equal to zero and the nature of the reaction below this temperature are 
(a) 483 K, spontaneous
(b) 443 K, non-spontaneous
(c) 443 K, spontaneous
(d) 463 K, non-spontaneous 

Answer

D

Question. The free energy for a reaction having ΔH= 31400 cal, ΔS = 32c al K-1 mol-1 at 1000° C is 
(a) – 9336 cal
(b) – 7386 cal
(c) – 1936 cal
(d) + 9336 cal   

Answer

A

Question. All naturally occurring process, proceed in a direction, which leads to 
(a) increase of enthalpy
(b) increase of free energy
(c) decrease of free energy
(d) decrease of entropy   

Answer

C

Question. In conversion of limestone to lime,
       CaCO3 (s) → CaO(s) + CO2 (g)
the values of ΔH° and ΔS° are+ 179.1 kJ mol-1 and 160.2 J/K respectively at 298 K and 1 bar. Assuming that ΔH° and ΔS° do not change with temperature, temperature above which conversion of limestone to lime will be spontaneous is 
(a) 1008K
(b) 1200K
(c) 845K
(d) 11 18K   

Answer

D

Question. Gibb’s free energy G, enthalpy H and entropy S are interrelated as in
(a) G = H + TS
(c) G – TS = H
(b) G = H – TS
(d) G = S = H 

Answer

B

Question. Which is a condition for spontaneous ? 
(a) ΔG < 0
(b) ΔG = 0
(c) ΔG > 0
(d) ΔG ≥ 0 

Answer

A

Question. If ΔH = – 25 kcal, T = 300 K and ΔS = 9 cal, then the reaction is 
(a) spontaneous
(c) equilibrium state
(b) non-spontaneous
(d) None of these   

Answer

A

Question. Molar heat of vaporisation of a liquid is 6 kJ mol-1 . If the entropy change is 16 J mol-1 K-1, the boiling point of the liquid is 
(a) 375° C
(b) 375 K
(c) 273 K
(d) 102° C   

Answer

B

Question. The free energy change ΔG= 0 when
(a) the reactants are completely consumed
(b) a catalyst is added
(c) the system is at equilibrium
(d) the reactants are initially mixed 

Answer

C

Question. What are the units of entropy ?
(a) cal K
(b) cal K-1
(c) cm K-1
(d) cm K   

Answer

B

Question. Which of the following statements is not true regarding the laws of thermodynamics ?
(a) It deal with energy changes of macroscopic systems.
(b) It deal with energy changes of microscopic systems.
(c) It does not depends on the rate at which these energy transformations are carried out.
(d) It depends on initial and final states of a system undergoing the change.

Answer

B

Question. A……………… in thermodynamics refers to that part of universe in which observations are made and remaining universe constitutes the………………
(a) surroundings, system
(b) system, surroundings
(c) system, surroundings
(d) system, boundary

Answer

B

Question. The universe refers to
(a) only system
(b) only surroundings
(c) both system and surroundings
(d) None of these

Answer

C

Question. An isolated system is that system in which
(a) There is no exchange of energy with the surroundings
(b) There is exchange of mass and energy with the surroundings
(c) There is no exchange of mass or energy with the surroundings
(d) There is exchange of mass with the surroundings

Answer

C

Question. The state of a thermodynamic system is described by its measurable or macroscopic (bulk) properties. These are
(a) Pressure and volume
(b) Pressure, volume, temperature and amount
(c) Volume, temperature and amount
(d) Pressure and temperature

Answer

B

Question. Which of the following are not state functions ?
(I) q + w (II) q
(III) w (IV) H – TS
(a) (I) and (IV)
(b) (II), (III) and (IV)
(c) (I), (II) and (III)
(d) (II) and (III)

Answer

D

Question. ………………. is a quantity which represents the total energy of the system
(a) Internal energy
(b) Chemical energy
(c) Electrical energy
(d) Mechanical energy

Answer

A

Question. Which of the following factors affect the internal energy of the system ?
(a) Heat passes into or out of the system.
(b) Work is done on or by the system.
(c) Matter enters or leaves the system.
(d) All of the above

Answer

D

Question. Among the following the state function(s) is (are) (i) Internal energy
(ii) Irreversible expansion work
(iii) Reversible expansion work
(iv) Molar enthalpy
(a) (ii) and (iii)
(b) (i), (ii) and (iii)
(c) (i) and (iv)
(d) (i) only

Answer

C

Question. Enthalpy change (ΔH) of a system depends upon its
(a) Initial state
(b) Final state
(c) Both on initial and final state
(d) None of these

Answer

C

Question. The system that would not allow exchange of heat between the system and surroundings through its boundary is considered as
(a) isothermal
(b) adiabatic
(c) isobaric
(d) isochoric

Answer

B

Question. The enthalpy change of a reaction does not depend on
(a) The state of reactants and products
(b) Nature of reactants and products
(c) Different intermediate reactions
(d) Initial and final enthalpy change of a reaction.

Answer

C

Question. The q is ……………. when heat is transferred from the surroundings to the system and q is……………………….. When heat is transferred from system to the surroundings.
(a) positive , negative
(b) negative , positive
(c) high, low
(d) low, high

Answer

A

Question. Adiabatic expansions of an ideal gas is accompanied by
(a) decrease in ΔE
(b) increase in temperature
(c) decrease in ΔS
(d) no change in any one of the above properties

Answer

A

Question. Which of the following statements is incorrect?
(a) q is a path dependent function.
(b) H is a state function.
(c) Both H and q are state functions.
(d) Both (a) and (b)

Answer

D

Question. When 1 mol of a gas is heated at constant volume, temperature is raised from 298 to 308 K. If heat supplied to the gas is 500 J, then which statement is correct ?
(a) q = w = 500 J, ΔU = 0
(b) q = ΔU = 500 J, w = 0
(c) q = –w = 500 J, ΔU = 0
(d) ΔU = 0, q = w = –500 J

Answer

B

Question. During isothermal expansion of an ideal gas, its
(a) internal energy increases
(b) enthalpy decreases
(c) enthalpy remains unaffected
(d) enthalpy reduces to zero.

Answer

C

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

B

Question. An ideal gas expands in volume from 1×10–3 to 1 × 10–2 m3 at 300 K against a constant pressure of 1×105 Nm–2. The work done is
(a) 270 kJ
(b) – 900 kJ
(c) – 900 J
(d) 900 kJ

Answer

C

Question. The difference between ΔH and ΔU is usually significant for systems consisting of
(a) only solids
(b) only liquids
(c) both solids and liquids
(d) only gases

Answer

D

Question. If a reaction involves only solids and liquids which of the following is true ?
(a) ΔH < ΔE
(b) ΔH = ΔE
(c) ΔH > ΔE
(d) ΔH = ΔH ΔE + RTΔn

Answer

B

Question. Assume each reaction is carried out in an open container. For which reaction will ΔH = ΔE ?
(a) C(s) + 2H2O (g) → 2H2 (g) + CO2 (g)
(b) PCl5 (g) → PCl3 (g) + Cl2 (g)
(c) 2CO (g) + O2 (g) → 2CO2 (g)
(d) H2 (g) + Br2 (g) → 2 HBr (g)

Answer

D

Question. For a reaction in which all reactants and products are liquids, which one of the following equations is most applicable ?
(a) ΔH < ΔE
(b) ΔH = ΔS
(c ΔH = ΔE
(d) ΔH = ΔG

Answer

C

Question. The relationship between enthalpy change and internal energy change is
(a) ΔH = ΔE + P ΔV
(b) ΔH = ( ΔE + V ΔP)
(c) ΔH = ΔE – P ΔV
(d) ΔH = PΔV – ΔE

Answer

A

Question. For the reaction C3H8 (g) → 5O2 (g)→3CO2 (g) → 4H2O(l) at constant temperature, ΔH – ΔE is
(a) – RT
(b) + RT
(c) – 3 RT
(d) + 3 RT

Answer

C

Question. Consider the reaction : N→ 3H2 → 2NH3 carried out atconstant temperature and pressure. If ΔH and ΔU 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

Answer

B

Question. Among the following, the intensive properties are
(i) molar conductivity
(ii) electromotive force
(iii) resistance (iv) heat capacity
(a) (ii) and (iii)
(b) (i), (ii) and (iii)
(c) (i) and (iv)
(d) (i) only

Answer

A

Question. Which is an extensive property of the system ?
(a) Volume
(b) Viscosity
(c) Temperature
(d) Refractive index

Answer

A

Question. Which of the following is an example of extensive property?
(a) Temperature
(b) Density
(c) Mass
(d) Pressure

Answer

C

Question. Which of the following factors do not affect heat capacity?
(a) Size of system
(b) Composition of system
(c) Nature of system
(d) Temperature of the system

Answer

D

Question. The heat required to raise the temperature of body by 1 C° is called
(a) specific heat
(b) thermal capacity
(c) water equivalent
(d) None of these.

Answer

B

Question. Which of the following is not true regarding thermo-chemical equations?
(a) The coefficients in a balanced thermo-chemical equation refer to the number of moles of reactants and products involved in the reaction
(b) The coefficients in a balanced thermo-chemical equation refer to the number of molecules of reactants and products involved in the reaction
(c) The numerical value of ΔrH refers to the number of moles of substances specified by an equation.
(d) Standard enthalpy change ΔrHΘ will have units as kJ mol-1.

Answer

B

Question. The enthalpies of elements in their standard states are taken as zero. The enthalpy of formation of a compound
(a) is always negative
(b) is always positive
(c) may be positive or negative
(d) is never negative

Answer

C

Question. Equal volumes of two monoatomic gases, A and B, at same temperature and pressure are mixed. The ratio of specific heats (Cp/Cv) of the mixture will be :
(a) 0.83
(b) 1.50
(c) 3.3
(d) 1.67

Answer

D

Question. The molar heat capacity of water at constant pressure is 75 JK–1 mol–1. When 1kJ of heat is supplied to 100 g of water, which is free to expand, the increase in temperature of ter is   
(a) 6.6 K
(b) 1.2 K
(c) 2.4 K
(d) 4.8 K

Answer

C

Question. Calorie is equivalent to :
(a) 0.4184 Joule
(b) 4.184 Joule
(c) 41.84 Joule
(d) 418.4 Joule

Answer

B

Question. If enthalpies of formation of C2H4 (g) , CO2(g) and H2O(l) at 25°C and 1atm pressure are 52, – 394 and – 286 kJ/mol respectively, the change in ethalpy is equal to
(a) – 141.2 kJ/mol
(b) – 1412 kJ/mol
(c) + 14.2 kJ/mol
(d) + 1412 kJ/mol

Answer

B

Question. The enthalpy change for a reaction does not depend upon
(a) use of different reactants for the same product
(b) the nature of intermediate reaction steps
(c) the differences in initial or final temperatures of involved substances
(d) the physical states of reactants and products

Answer

B

Question. Given that bond energies of H – H and Cl – Cl are 430 kJ mol– 1 and 240 kJ mol–1 respectively and ΔHf for HCl is – 90 kJ mol– 1, bond enthalpy of HCl is
(a) 380 kJ mol–1
(b) 425 kJ mol–1
(c) 245 kJ mol–1
(d) 290 kJ mol–1

Answer

B

Question. Bond dissociation enthalpy of H2, Cl2 and HCl are 434 , 242 and 431 kJ mol–1 respectively. Enthalpy of formation of HCl is:
(a) 93 kJ mol–1
(b) – 245 kJmol–1
(c) – 93 kJmol–1
(d) 245 kJmol–1

Answer

C

Thermodynamics Class 11 Chemistry MCQ Questions