MCQ Questions Chapter 6 Thermodynamics Class 11 Chemistry

Please refer to MCQ Questions Chapter 6 Thermodynamics Class 11 Chemistry with answers provided below. These multiple-choice questions have been developed based on the latest NCERT book for class 11 Chemistry issued for the current academic year. We have provided MCQ Questions for Class 11 Chemistry for all chapters on our website. Students should learn the objective based questions for Chapter 6 Thermodynamics in Class 11 Chemistry provided below to get more marks in exams.

Chapter 6 Thermodynamics MCQ Questions

Please refer to the following Chapter 6 Thermodynamics MCQ Questions Class 11 Chemistry with solutions for all important topics in the chapter.

MCQ Questions Answers for Chapter 6 Thermodynamics Class 11 Chemistry

Question. For the reaction, C (graphite) + 1/2 O₂ (g) → CO(g) at 2 298 K and 1 atm, ΔH = – 26. 4 kcal. What is ΔE, if the molar volwne of graphite is 0.0053 L?
[R = 0. 002 kcal mol^-1 K^-1]
(a) – 26.7 kcal
(b) + 26.7 kcal
(c) – 52.4 kcal
(d) + 52.4 kcal       

Question. The value of ~E for combustion of 16 g of CH₄ is – 885389 J at 298 K. The ΔH combustion for CH₄ in J mol^-1 at this temperature will be
(Given that,R = 8. 314 JK^-1 mol^-1)
(a) – 55337
(b) – 880430
(c) – 885389
(d) – 890348      

Question. If the bond dissociation energies of XY, X ₂ and Y₂ (all diatomic molecules) are in the ratio of 1: 1: 0.5 and ΔH_f I for the formation of XY is -200 kJ mol^-1 . The bond dissociation energy of X₂ will be 
(a) 400 kJ mol^-1
(b) 300 kJ mol^-1
(c) 20 kJ mol^-1
(d) None of these      

Question. For the reaction (at 1240 Kand 1 atm.)
 CaCO₃(s) → CaO(s) + CO₂ (g) 
ΔH = 176 kJ/mol; ΔE will be
(a) 160 kJ
(b) 165.6 kJ
(c) 186.4 kJ
(d) 180 kJ     

Question. Which is correct for an endothermic reaction ? 
(a) ΔH is positive
(b) ΔH is negative
(c) ΔE isnegative
(d) ΔH = 0         

Question. In an isothermal process
(a) q = 0 and ΔE = 0
(b) q ≠ 0 and ΔE = 0
(c) q = 0 and ΔE ≠ 0
(d) q ≠ 0 and ΔE ≠ 0     

Question. Heat of neutralisation will be minimum for which of the following combination ? 
(a) NaOH + H₂SO₄
(b) NH₄OH + CH₃COOH
(c) NaOH + HCl
(d) NaOH + CH₃COOH     

Question. Which of the following indicates the heat ofreaction equal to heat of formation ? 
(a) C(graphite)  + O₂  (latm)  → CO₂ (latm)
(b) C(diamond) + O₂ (I atm) → CO₂ (2 atm)
(c) C(graphite)  + O₂  (latm) → CO₂ (2atm)
(d) C(diamond) + O₂ (l atrn) → CO₂ (1 atm)         

Question. For CaCO₃ (s) ⇔ CaO(s)+ CO₂(g) at 927° C ΔH = 176 kJ mol; then ΔE is 
(a) 180 kJ
(b) 186.4 kJ
(c) 166.0 kJ
(d) 160 kJ         

Question. The H—H bond energy is 430 kJ mol^-1 and Cl—Cl bond energy is 240 kJ mol^-1 , AH for HCI is – 90 kJ. The H—Cl bond energy is about 
(a) 180 kJ mol^-1
(b) 360kJ mol^-1
(c) 213 kJ mol^-1
(d) 425 kJ mol^-1       

Question. The ΔH°_f for CO₂ (g), CO(g) and H₂O(g) are – 393.5, – 110.5 and – 241.8 kJ/mol respectively. The standard enthalpy change (in kJ) for the reaction 
               CO₂(g)+H₂(g) → CO(g)+H₂O(g)is
(a) 524.1
(c) – 262.5
(b) 41.2
(d) – 4 1.2         

Question. For the following two reactions,
(i) CH₄ (g) + 2O₂ (g) → CO₂ (g) + 2H₂O
                                          ΔH = – 890.4 kJ
(ii) 2HgO(s) → 2Hg(/) + O₂ (g ); ΔH + 181.6 kJ
Which one of the following statements is correct ?
(a) Both of them are exothermic 
(b) Both of them are endothermic
(c) (i) is exothermic and (ii) is endothermic
(d) (i) is endothem1ic and (ii) is exothermic         

Question. The first law of thermodynan1ics is expressed as
(a) q – W = ΔE 
(b) ΔE = q – W
(c) q = M – W
(d) W = q + ΔE
(e) None of the above     

Question. Hess’s law is used to calculate 
(a) enthalpy ofreaction
(b) entropy of reaction
(c) work done in reaction
(d) All of these       

Question. The pair of isochoric processes among the transformation of states is 
(a) K to L and L to M
(b) L to M and N to K
(c) L to M and M to N
(d) M to N and N to K   

Question. The intensive property among these quantities is 
(a) enthalpy
(b) mass/volume
(c) mass
(d) volwne       

Question. A gas can expand from 100 mL to 250 mL under a constant pressure of 2 attn. The work done by the gas is 
(a) 30.48 J
(b) 25 J
(c) 5 kJ
(d) 16 J       

Question. Which one of the following is not a state function ?
(a) Enthalpy
(b) Entropy 
(c) Work
(d) Free energy       

Question. We believe in the laws of thermodynamics because they are
(a) theoretical
(b) derived based on mathematical analysis
(c) empirical and nobody disproved
(d) mere statements       

Question. The sublimation energy of I₂ (s) is 57 .3 kJ/mol and the enthalpy of fusion is 15.5 kJ/mol. The enthalpy of vaporisation of I₂ is
(a) 41.8 kJ/mol
(b) –41.8 k:J/ mol
(c) 72.8 kJ/mol
(d) –72.8 k:J/ mol     

Question. The temperature of the system decreases in an
(a) adiabatic compression
(b) isothermal compression
(c) isothermal expansion
(d) adiabatic expansion     

Question. On complete combustion, 0.246 g of an organic compound gave 0.198 g of CO₂ and 0.1014 g of H₂O. The ratio of carbon and hydrogen atoms in the compound is 
(a) 1 : 3
(b) 1 : 2
(c) 2: 5
(d) 2: 7     

Question. When ice melts into water, the entropy 
(a) becomes zero
(b) remains same
(c) decreases
(d) increases     

Question. Which one of the following is correct ? 
(a) – ΔG = ΔH – TΔS
(b) ΔH = [ΔG – TΔS] 
(c) ΔS = 1/T [ΔG – ΔH]
(d) ΔS = 1/T [ΔH – ΔG]       

Question. What is the relation between E° and K ?
(a) E° = 0.0591/n logK 
(b) E° = n/0.0591 logK
(c) E° = 2.303R/nF log K 
(d) E° = 2.303 RT/n log K   

Question. One mole of ice is converted into water at 273 K.. The entropies of H₂O(s) and H₂O(/) are 38.20 and 60.01 J mol^-1 K^-1 respectively. The enthalpy change for the conversion is
(a) 3 kJ mol^-1
(c) 5 kJ mol^-1
(b) 4 kJ mol^-1 
(d) 6 kJ mol^-1   

Question. Which of the following statements is true? 
(a) The total entropy of the universe is continuously decreasing
(b) The total energy of the universe is continuously decreasing
(c) The total energy of the universe remains constant
(d) The total entropy of the universe remains constant   

Question. For the reaction H₂O(/) ⇌ H₂O(g) at 373 K and I atm pressure
(a) ΔH = 0
(b) ΔE = 0
(c) ΔH = TΔS
(d) ΔH = ΔE     

Question. Given that dE = TdS – pdV and H = E + pV. Which one of the following relations is true?
(a) dH = TdS +Vdp
(b) dH = SdT + V dp
(c) dH = – SdT+Vdp
(d) dH = dE + pdV
(e) dH = dE – TdS     

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. The heat of neutralisation is highest for the reaction between 
(a) NH₄OH—CH₃COOH
(b) HNO3—NH₄OH
(c) NaOH—CH₃COOH
(d) HCI—NaOH       

Question. In a constant volume calorimeter, 3.5 g of a gas with molecular weight 28 was burnt in excess oxygen at 298.0 K. The temperature of the calorimeter was found to increase from 298.0 K to 298.45 K, due to the combustion process. Given, that the heat capacity of the calorimeter is 2.5 kJ K^-1 , the numerical value for the enthalpy of combustion of the gas in kJ mmol^-1 is 
(a) 7
(b) 9
(c) 0
(d) 8     

Question. For which of the following equations is the change in enthalpy at 25°C and 1 atm equal to ΔH°_f of CH₂O(/)
(a) C(g) + H₂ (g)+(V2) O₂ (g) → CH₂O(/)
(b) C(s) + H₂ (g) + (l/2)O₂ (g) → CH₂O(/)
(c) C(g)+ 2H₂ (g)+ O(g) → CH₂O(/)
(d) CO(g)+ H₂ (g) → CH₂O(/)     

Question. The standard enthalpies of formation of CO₂ (g ), H₂O(/) and glucose (s) at 25°C are – 400 kJ/ mol, –300 kJ/ mol and –1300 kJ/ mol, respectively. The standard enthalpy of combustion per gram of glucose at 25°C is
(a) + 2900 kJ
(b) –2900 kJ
(c) –16.11 kJ
(d) + 16.11 kJ         

Question. The standard enthalpy of formation (ΔH°_f ) at 298 K for methane, CH₄ (g), is – 78.4 kJ mol^-1. The additional information required to determine the average energy for C—H bond formation would be 
(a) the dissociation energy of H₂ and enthalpy of sublimation of carbon
(b) latent heat of vaporisation of methane
(c) the first four ionisation energies of carbon and electron gain enthalpy of hydrogen
(d) the dissociation energy of hydrogen molecule, H₂     

Question. The enthalpy changes for the following processes are listed below.
      Cl₂ (g) = 2Cl(g ), 242.3 kJ mol^-1
      I₂ (g)= 2I(g), 151.0 kJ mol^-1
      ICl (g)= I(g)+ Cl(g),211.3 kJ mol^-1
      I₂ (s) = I₂ (g), 62.76 kJ mol^-1
Given that the standard states for iodine and chlorine are I₂ (s) and Cl₂ (g), the standard enthalpy of formation of ICl (g) is
(a) – 14.6kJ mol^-1
(b) – 16.8kJ mol^-1
(c) + 16.8kJ mol^-1
(d) + 244.8kJ mol^-1     

Question. A monoatornic ideal gas undergoes a process in which the ratio of P to V 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
(d) O     

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

Question. If heat of neutralisation of HCN with NaOH is — 12.1 kJ and the heat of neutralisation of HCI by NaOH is —55.9 kJ/mol, then the energy of dissociation of HCN is
(a) 43.8 kJ
(b) – 43.8 kJ 
(c) – 68 kJ
(d) 68 kJ     

Question. ln an isochoric process, ΔH for a system is equal to
(a) p . ΔV
(b) pV 
(c) E + p.ΔV
(d) ΔE     

Question. For the reaction, A (g) + 2B(g) → 2C (g) + 3D (g) the change of enthalpy at 27° C is 19 kcal. The value of M is 
(a) 21.2 kcal
(b) 17.8 kcal
(c) 18.4 kcal
(d) 20.6 kcal           

Question. When 50cm³ of 0.2 N H₂SO₄ is mixed with 50cm³ of I N KOH, the heat liberated is 
(a) 11.46 kJ
(b) 157.3 kJ
(c) 573 kJ
(d) 573 J       

Question. The enthalpy of reaction, 
H₂(g) + 1/2 O₂(g) → H₂O(g) is ΔH₁ and that of  
H₂(g) + 1/2 O₂(g) → H2O(/) is ΔH₂.
Then
(a) ΔH₁ < ΔH₂
(b) ΔH₁ + ΔH₂ = 0
(c) ΔH₁ > ΔH₂
(d) ΔH₁ = ΔH₂         

Question. Identify the reaction for which ΔH ≠ ΔE
(a) S (rhombic) + O₂ (g) → SO₂ (g)
(b) N₂(g) + O₂(g) → 2NO(g)
(c) H₂(g) + Cl₂(g) → 2HCl(g)
(d) CO(g) + 1/2 O₂(g) → CO₂(g)     

Question. EnthalpyofformationofHFandHCl are -16l kJ and -92 kJ respectively. Which of the following statements is incorrect ? 
(a) HCl is more stable than HF
(b) HF and HCl are exothermic compounds
(c) The affinity of fluorine to hydrogen is greater than the affinity of chlorine to hydrogen
(d) HF is more stable than HCl           

Question. A mixture of two moles of carbon monoxide and one mole of oxygen, in a closed vessel is ignited to convert the carbon monoxide to carbon dioxide. If ΔH is the enthalpy change and ΔE is the change in internal energy, then
(a) ΔH > ΔE
(b) ΔH < ΔE
(c) ΔH = ΔE
(d) the relationship depends on the capacity of the vessel         

Question. The cooling in refrigerator is due to 
(a) reaction of the refrigerator gas
(b) expansion of ice
(c) the expansion of the gas in the refrigerator
(d) the work of the compressor     

Question. What would be the heat released when an aqueous solution containing 0.5 mole of HNO₃ is mixed with 0.3 mole of OH^– (enthalpy ofneutralisation is -57.1 kJ)?
(a) 28.5 kJ
(b) 17.1 kJ
(c) 45.7 kJ 
(d) 1.7 kJ       

Question. ΔE° of combustion of iso-butylene is – X kJ mol^-1 . The value of ΔH°  is 
(a) = ΔE°
(b) > MΔE°
(c) = 0
(d) < ΔE°   

Question. Calculate ΔH (in Joules) for, C (graphite) → C ( diamond), from the following data
C (graphite) + O₂ (g) → CO₂ (g ); ΔH = – 393.5 kJ
C (diamond) + O₂ (g) → CO₂ (g ); ΔH= – 395.4 kJ
(a) 1900
(b) – 788.9x 10³
(c) 190000
(d) + 788.9x 10³           

Question. In which of the following reactions, the heat liberated is known as “heat of combustion” ? 
(a) H⁺ (aq) + OH^– (aq)➔ H₂O(l)+ heat
(b) C (graphite) + 1/2 O₂ (g) ➔ CO(g) + heat 
(c) CH₄ (g)+2O₂ (g) ➔ CO₂(g)+2H₂O(/)+heat
(d) H₂SO₄ (aq)+ H₂O (l)➔ H₂SO₄ (aq)+ heat         

Question. Heat of formation of SO₂ is -298 kJ. What is the heat of combustion of 4 g of S ? 
(a) + 37 kJ
(b) – 37.25 kJ
(c) + 298kJ
(d) 18.6 kJ     

Question. Among the following which is true forl mole of liquid ?
(a) C_p ≈ C_v
(b) C_{p –} C_v = R 
(c) C_p – C_v > R
(d) C_p < C_v         

Question. The heats of combustion of carbon monoxide at constant pressw-e and at constant volume at 27° C will differ from one another by 
(a) 27 cal
(b) 54 cal
(c) 300 cal
(d) 600 cal     

Question. Minimum work is obtained when 1 kg of…gas expanded under 500 kPa to 200 kPa pressure at 0°C. 
(a) chlorine
(b) oxygen
(c) nitrogen
(d) methane         

Question. Which of the following is not correct? 
(a) Dissolution of NH₄Cl in excess of water is an endothermic process
(b) Neutralisation process is always exothermic
(c) The absolute value of enthalpy (H) can be determined experimentally
(d) The heat ofreaction at constant volume is denoted by ΔE   

Question. Heat liberated with 100 mL of l N NaOH is neutralised by 300 mL of IN HCI 
(a) 11.56kJ
(b) 5.73kJ
(c) 22.92kJ
(d) 17.19kJ     

Question. Given, 2Fe + 3/2 O₂ → Fe₂O₃; ΔH =- 193.4 kJ;
Mg+ 1/2 O₂ → MgO; ΔH= – 140.2kJ;
What is the t’1H of the reaction ?
3Mg + Fe₂O₃ → 3MgO + 2Fe 
(a) – 227.2 kJ
(b) – 272.3 kJ
(c) 227.2 kJ
(d) 272.2 kJ     

We hope you liked the above provided MCQ Questions Chapter 6 Thermodynamics Class 11 Chemistry with solutions. If you have any questions please ask us in the comments box below.