Please refer to Chapter 6 Thermodynamics MCQ Class 11 Chemistry with answers below. These multiple-choice questions have been prepared based on the latest NCERT book for Class 11 Chemistry. Students should refer to MCQ Questions for Class 11 Chemistry with Answers to score more marks in Grade 11 Chemistry exams. Students should read the chapter Thermodynamics and then attempt the following objective questions.

MCQ Questions Class 11 Chemistry Chapter 6 Thermodynamics

The Thermodynamics MCQ Class 11 Chemistry provided below covers all important topics given in this chapter. These MCQs will help you to properly prepare for exams.

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

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, ΔE =0
(b) q = W = 500 J, ΔE =0
(c) q = ΔE = 500 J, W =0
(d) ΔE = 0, q =W = −500 J     

Question. The molar heat capacity of water at constant pressure is 75 J K⁻¹ mol⁻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. Which of the following statement is correct?1 Which of the following statement is correct?
(a) The presence of reacting species in a coveredbeaker is an example of open system
(b) There is an exchange of energy as well as matterbetween the system and the surroundings in a closedsystem
(c) The presence of reactants in a closed vessel madeup of copper is an example of a closed system
(d) The presence of reactants in a thermos flask or anyother closed insulated vessel is an example of aclosed system   

Question. The pressure-volume work for an ideal gas can becalculated by using the expression W = −∫^vf_vf p^exdv . Thework can also be calculated from the pV − plot by using thearea under the curve within the specified limits. When anideal gas is compressed (a) reversibly or (b) irreversiblyfrom volume V_i to V_t . 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 ΔV         

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

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 of heat. 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. (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. 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, ΔT ≠ 0,W = 0
(b) q ≠ 0, ΔT = 0,W = 0
(c) q = 0, ΔT = 0,W = 0
(d) q = 0, ΔT < 0,W ≠ 0       

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. What will be the change of entropy Δ_rS° at 298 K for the reaction, in which urea is formed from NH₃ 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. 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. For two moles of an ideal gas
(a) (C_p − C_V) = 2R   
(b) (C_p − C_V) = 0
(c) (C_p − C_V) = R 
(d) (C_p − C_V) = R/2     

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. 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⁻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. The combustion of benzene (l) gives CO₂(g) and H₂O(l). Given that heat of combustion of benzene 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⁻¹)  
(a) 4152.6
(b) −452.46
(c) 3260
(d) −3267 6 .     

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. The value of ΔH for cooling 2 mole of an ideal monoatomic gas from 225°C to 125°C at constant pressure will be(given C_P = 5/2 R)
(a) 250 R
(b) – 500 R
(c) 500 R
(d) – 250 R       

Question. Consider the following reactions at 1100° C
(I) 2C + O₂ → 2CO, ΔG° = – 460 kJ mol^-1
QuestionII) 2Zn + O₂ → 2Zno,ΔG° = – 360kJ mol^-1
Based on these, select correct alternate.
(a) Zinc can be oxidised by CO
(b) Zinc oxide can be reduced by carbon
(c) Both are correct
(d) None of the above is correct   

7. The enthalpy of vaporisation of a certain liquid at its boiling point of 35°C is 24.64 kJ  mol^-1 . The value of change in entropy for the process is 
(a) 704 JK^-1 mol^-1
(b) 80 JK^-1  mol^-1
(c) 24.64 JK^-1  mol^-11
(d) 7.04 JK^-1 mol^-1     

Question. The free energy change for the following reactions are given below₅
C₂H₂ (g) + 52 O₂ (g) → 2CO₂ (g)+ H₂O(/);
                                                  ΔG° = – 1234 kJ
C(s) + O₂ (g) → CO₂ (g ); ΔG° = -394 kJ
H₂ (g) + 1/2 O₂(g) → H₂O(/); ΔG° = -237 kJ 2
What is the standard free energy change for the reaction
               H₂ (g) + 2C(s) → C₂H₂ (g)? 
(a) – 209kJ
(b) – 2259kJ
(c) + 2259 kJ
(d) 209 kJ 

Question. The standard free energy change of a reaction is ti ΔG° = – 115 kJ at 298 K. Calculate the equilibrium constant K_P in log K_P [R = 8.314 JK^-1 mol^-1] 
(a) 20.16
(b) 2.303
(c) 2.016
(d) 13.83 

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, > l ,+ve     

Question. The enthalpy change for the transition of liquid water to steam is 40.8 kJ per mol at 100° C. The entropy change for the process will be 
(a) 0.408 JK^-1 mol^-1
(b) 408 JK^-1 mol^-1
(c) 109.4 JK^-1 mol^-1
(d) 0.1094 JK^-1 mol^-1       

Question. When a solid melts reversibly
(a) H decreases
(b) G increases
(c) E decreases
(d) S increases 

Question. The value oflog Kc for a reaction
A ⇌ B is (Given, ΔH° 298K = – 54.07 kJ mol^-1, ΔS° 298 K = 10 JK^-1 rnol^-1 and
R = 8.314 JK^-1mol^-1
2303 X 8.314 X 298 = 5705)
(a) 5
(b) 10
(c) 95
(d) 100 

Question. For the process H₂O(/)(l bar, 273 K) ⇌ H₂O(g )(1 bar, 273 K) the correct set of themodynamic parameters is
(a) ΔG = 0, ΔS = + ve 
(b) ΔG = 0, ΔS = – ve
(c) ΔG =+ ve, ΔS =0
(d) ΔG = – ve, ΔS = + ve 

Question. If an endothermic reaction occurs spontaneously at constant temperature (T) and pressure (p), then which of the following is true ? 
(a) ΔG > 0
(b) ΔH < 0
(c) ΔS > 0
(d) ΔS < 0 

Question. A spontaneous process is one in which the system suffers
(a) no energy change
(b) a lowering of free energy
(c) a lowering of entropy
(d) an increase in internal energy 

Question. Condition for spontaneity in an isothermal process is
(a) ΔA + W < 0
(b) ΔG + U < 0 
(c) ΔA + U > 0
(d) ΔG – U < 0 

Question. Enthalpy is equal to
(a) T² [δ(G / T)/δ T]_p
(b) -T² [δ(G / T)/δ T]_p
(c) T² [δ(G / T)/δ T]_v
(d) -T² [δ(G / T)/δ T]_v 

Question. The decomposition of lin1estone
                  CaCO₃ (g) ⇌ CaO(s) + CO₂ (g)
is non-spontaneous at 298 K. The ΔH° and ΔS° values for the reaction are 76.0 kJ and 60 JK^-1 respectively. At what temperature the decomposition spontaneous?
(a) At 1000 K
(b) Below 500° C
(c) Between 500° C and 600° C
(d) Above 827° C becomes 

Question. Standard enthalpy and standard entropy changes for the oxidation of ammonia at 298 Kare – 382.64 kJ mol^-1 and – 145.6 JK^-1 mol^-1 , respectively. Standard Gibbs energy change for the same reaction at 298 K is 
(a) – 2221.1 kJ mol^-1
(b) – 339.3 kJ mol^-1
(c) – 439.3 kJ mol^-1
(d) – 523.2 kJ mol^-1      

Question. Given that C + O₂ → CO₂ ; ΔH° = – x kJ 2CO +O₂  → 2CO₂  ; ΔH° = – y kl The heat of formation of carbon monoxide will be 
(a) y – 2x
(b) y + 2x
(c) 2x – y
(d) 2x – y/2       

Question. A swimmer coming out from a pool is covered with a film of water weighing about 18 g. Calculate the internal energy of vaporisation at 100°C.
[Δ_vapH^Θ for water at 373 K = 40.66 kJ mol^-1] The correct option is
(a) 35.67kJ mol^-1
(c) 36.57 kJ mol^-1
(b) 37.56kJ mol^-1
(d) 38.75 kJ mol^-1       

Question. LVf for the reaction,
C(graphite) + 2H₂(g) → CH₄ (g)at 298 Kand l attn is – 17900 cal. The M for the above conversion would be
(a) – 17900cal
(b) 17900 cal 
(c) 17304 cal
(d) – 17304 cal       

Question. Assuming that water vapour is an ideal gas, the internal energy change (ΔU)when 1 mole of water is vaporised at 1 bar pressure and 100° C, (Given, molar enthalpy of vaporisation of water at 1 bar and 373 K = 41 kJ mol^-1 and R = 8.3 J mol^-1 K^-1 ) will be 
(a) 4.100 kJ mol^-1
(b) 3.7904 kJ mol^-1
(c) 37.904 kJ mol^-1
(d) 41.00 kJ mol^-1     

Question. The enthalpies of combustion of carbon and carbon monoxideare -393.5and- 283kJ mol^-1 respectively. The enthalpy of formation of carbon monoxide per mole is
(a) 110.5 kJ
(b) 676.5 kJ 
(c) – 676.5 kJ
(d) – 110.5 kJ   

Question. Calculate enthalpy for formation of ethylene from the following data 
I. C(graphite)+ O₂(g) → CO₂(g);ΔH = 393.5kJ
II. H₂(g)+ 1/2 O₂(g) → H2O(/);ΔH = -286.2 kJ
III. C₂H₄ (g)+ 3O₂(g) → 2CO₂(g)+2H₂O(/);
                                           ΔH = -1410.8kJ
(a) 54.1 kJ
(b) 44.8 kJ
(c) 51.4 kJ  
(d) 48.4 kJ     

Question. The decreasing order of bond dissociation energies of C—C, C—H and H—H bonds is 
(a) H—H>—C—H>—C—C—
(b) —C—C—>—C—H>H—H
(c) —C—H>—C—C—> H—H
(d) —C—C—>H—H>—C—H—     

Question. When 1.8 g of steam at the normal boiling point of water is converted into water, at the same temperature, enthalpy and entropy changes respectively will be [Given, ΔH_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. . The enthalpy of vaporisation of liquid diethyl ether (C_{2 H5} )₂O, is 26.0 kJmol⁻¹ at its boiling point (35°C). What will be the ΔS for conversion of liquid to vapour and vapour to liquid respectively?
(a) + 84.41and − 84.41 JK⁻¹ mol⁻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. For a particular reversible reaction at temperature T, ΔH and ΔS were found to be both positive. If T_e 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. The value of log₁₀ K_C for a reaction A=B is [Given, Δ_rH°₂₉₈ = − 54.07 °  kJ 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. 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. 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     

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. The incorrect expression among the following is 
(a) ΔG_system / ΔS_stotal= −T
(b) In isothermal process,W_reversible = − nRT ln V V_f/v_i
(c) lnK =  ΔH° − TΔS°/ RT
(d) K = e ^−ΔG°/RT       

Question. For a reaction, M₂O(s) → 2M(s) + 1/2 O₂(g) ΔH = 30 kJ mol⁻¹ and DS = 0.07 kJ K⁻¹ mol⁻¹ at 1 atm. The temperature upto which the reaction would not be spontaneous is
(a) T < 400.08 K
(b) T < 273.15 K
(c) T < 428.57 K
(d) T < 473.50K       

Question. For the process, H₂O(l ) → H₂O(g)atT=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. In a fuel cell, methanol is used as fuel and oxygen gas is used as an oxidiser. The reaction is
         CH₃OH(l) + 3/2 O₂(g) → CO₂(g) + 2H₂O(l)
At 298 K standard Gibb’s energies of formation for CH₃OH(l)  ,H₂O(l ) and CO₂ (g) are –166.2, –237.2 and −394.4 kJ mol⁻¹, respectively. If standard enthalpy of combustion  f methanol is –726 kJmol⁻¹, efficiency of the fuel cell will be 
(a) 80%
(b) 87%
(c) 90%
(d) 97%             

Question. An ideal gas is allowed to expand both reversibly and irreversibly in an isolated system. If T_i is the initial
temperature and T_f is the final temperature, which of the following statement is correct?
(a) (T_f)_irrev > (T_f)_rev
(b) T_f > T_t  for reversible process, but T_f = T_i  for irreversible process
(c) (T_f)_rev > (T_f)_irrev
(d) T_f =  T_i for both reversible and irreversible processes     

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         

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

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.  CaCO₃ 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. In view of the signs of Δr G° for the following reactions
       PbO₂ + Pb → 2PbO, Δ_rG° 0 < 0
       SnO₂ + Sn → 2SnO, Δ_rG° 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. 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 ofn100 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. 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. 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. 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. In an irreversible process taking place at constantT and p and in which only pressure volume work is being done, the change in Gibbs free energy (ΔG) and change in entropy (ΔS), satisfy the criteria
(a) (ΔS)_V.E < 0, (ΔG)_T,p < 0
(b) (ΔS)_V.E > 0, (ΔG)_T,p < 0
(c) (ΔS)_V.E = 0, (ΔG)_T,p = 0
(d) (ΔS)_V.E = 0, (ΔG)_T,p > 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. ΔU and ΔH will be respectively.
(a) 10 J, 10 J
(b) 10 J, 0
(c) 0, 10 J
(d) 5 J, 10 J       

Question.  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.  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. 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. 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       

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