G and III rd Law of thermodynamics

7.1 For the reaction at 300 K A(g) + B(g)



^{C (g)}



^{E =} –3.0 kcal ;



^{S =} – 10.0 cal/K value of



^{G is}

(A) –600 cal (B) –6600 cal (C) –6000 cal (D) None

7.2* For isothermal expansion in case of an ideal gas :

(A) H = 0 (B) E = 0 (C) G = –T.S (D) T_final = T_initial

7.3 For the gas - phase decomposition, PCl₅ (g) PCl₃ (g) + Cl₂ (g) :

(A) H < 0, S < 0 (B) H > 0, S > 0 (C) H > 0, S < 0 (D) H < 0, S > 0

7.4 If



^Hvaporisation of substance X (l) (molar mass : 30 g/mol) is 300 J/g at it's boiling point 300 K, then molar entropy change for reversible condensation process is

(A) 30 J/mol.K (B) – 300 J/mol.K (C) –30 J/mol.K (D) None of these

7.5 What is the free energy change (G) when 1.0 mole of water at 100ºC and 1 atm pressure is converted into steam at 100ºC and 1 atm pressure ?

(A) 80 cal (B) 540 cal (C) 620 cal (D) Zero

7.6 What can be concluded about the values of



^{H and}



S from this graph?

(A)



^{H > 0,}



^{S > 0 (B)}



^{H > 0,}



^{S < 0}

(C)



^{H < 0,}



^{S > 0 (D)}



^{H < 0,}



^{S < 0}

7.7 The enthalpy change for a given reaction at 298 K is – x J mol^–1 (x being positive). If the reaction occurs spontaneously at 298 K, the entropy change at that temperature

(A) can be negative but numerically larger than x/298 (B) can be negative but numerically smaller than x/298 (C) cannot be negative

(D) cannot be positive

7.8 The change in entropy of 2 moles of an ideal gas upon isothermal expansion at 243.6 K from 20 litre until the pressure becomes 1 atm, is :

(A) 1.385 cal / K (B) –1.2 cal / K (C) 1.2 cal / K (D) 2.77 cal / K

7.9 A reaction has H = – 33 kJ and S = – 58 K

J. This reaction would be :

(A) spontaneous at all temperatures (B) non-spontaneous at all temperatures (C) spontaneous above a certain temperature (D) spontaneous below a certain temperature

Single Correct Answer Type :

1. A piece of zinc at a temperature of 20°C weighing 65.38 g is dropped into 180 g of boiling water (T = 100°C).

The specific heat of zinc is 0.4 J g^–1 C^–1 and that of water is 4.2 J g^–1°C^–1. What is the final common temperature reached by both the zinc and water ?

(A) 97.3 °C (B) 33.4 °C (C) 80.1 °C (D) 60.0°C

2. The heat capacity of liquid water is 75.6 J / mol.K, while the enthalpy of fusion of ice is 6.0 kJ/mol. What is the smallest number of ice cubes at 0°C, each containing 9.0 g of water, needed to cool 500 g of liquid water from 20°C to 0°C?

(A) 1 (B) 7 (C) 14 (D) None of these

3. A certain mass of gas is expanded from (1L, 10 atm) to (4L, 5 atm) against a constant external pressure of 1 atm. If initial temperature of gas is 300 K and the heat capacity of process is 50 J/°C. Then the enthalpy change during the process is (1L atm ~ 100 J)

(A) H = 15 kJ (B) H = 15.7 kJ (C) H = 14.4 kJ (D) H = 14.7 kJ

4. A heating coil is immersed in a 100 g sample of H₂O (l) at 1 atm and 100ºC in a closed vessel. In this heating process, 60% of the liquid is converted to the gaseous form at constant pressure of 1 atm. The densities of liquid and gaseous water under these conditions are 1000 kg/m³ and 0.60 kg/ m³ respectively. Magnitude of the work done for the process is :

(A) 4997 J (B) 4970 J (C) 9994 J (D) None of these

5. 10 litres of a monoatomic ideal gas at 0°C and 10 atm pressure is suddenly released to 1 atm pressure and the gas expands adiabatically against this constant pressure. The final temperature and volume of the gas respectively are.

(A) T = 174.9 K, V = 64 L (B) T = 153 K, V = 57 L (C) T = 165.4 K, V = 78.8 L (D) T = 161.2 K, V = 68.3 L

6. Consider a classroom that is roughly 5 m × 10m × 3m. Initially t = 27°C and P = 1 atm. There are 50 people in an insulated class loosing energy to the room at the average rate of 150 watt per person. How long can they remain in class if the body temperature is 42°C and person feels uncomfortable above this temperature.

Heat capacity of air = (7/2) R.

(A) 4.34 minutes (B) 5.91 minutes (C) 6.86 minutes (D) 7.79 minutes

7. At 5 × 10⁵ bar pressure, density of diamond and graphite are 3 g/cc and 2 g/cc respectively, at certain temperature ‘T’. Find the value of U – H for the conversion of 1 mole of graphite to 1 mole of diamond at temperature ‘T’ :

(A) 100 kJ/mol (B) 50 kJ/mol (C) – 100 kJ/mol (D) None of these

8. A new flurocarbon of molar mass 102 g mol^1 was placed in an electrically heated vessel. When the pressure was 650 torr, the liquid boiled at 77⁰C. After the boiling point had been reached, it was found that a current of 0.25 A from a 12.0 volt supply passed for 600 sec vaporises 1.8g of the sample. The molar enthalpy & internal energy of vaporisation of new flourocarbon will be :

(A)H = 102 kJ/mol, E = 99.1 kJ/mol (B) H = 95 kJ/mol, E = 100.3 kJ/mol (C) H = 107 kJ/mol, E = 105.1 kJ/mol (D) H = 92.7 kJ/mol, E = 97.4 kJ/mol

9. Two rigid adiabatic vessels A and B which initially, contain two gases at different temperatures are connected

by pipe line with valve of negligible volume. The vessel 'A' contain 2 moles Ne gas





The volume of A & B vessel is 4 and 6 litre respectively.

The final total pressure (in atm) when valve is opened and 12 Kcal heat supplied through it to vessels.

[Use : R = 2 cal / mol. K and R = 0.08 L . atm / mol K as per desire]

Ne SO

₂

A B

(A) 3.5 atm (B) 7 atm (C) 35 atm (D) 70 atm

10. The maximum efficiency of a heat engine operating between 100°C and 25°C is

(A) 20.11% (B) 22.2% (C) 25.17% (D) None

11. A heat engine operating between 227°C and 27°C absorbs 2 Kcal of heat from the 227°C reservoir reversibly per cycle. The amount of work done in one cycle is

(A) 0.4 Kcal (B) 0.8 Kcal (C) 4 Kcal (D) 8 Kcal

12. A reversible heat engine A (based on carnot cycle) absorbs heat from a reservoir at 1000K and rejects heat to a reservoir at T₂. A second reversible engine B absorbs, the same amount of heat as rejected by the engine A, from the reservoir at T₂ and rejects energy to a reservoir at 360K.

If the efficiencies of engines A and B are the same then the temperature T₂ is

(A) 680 K (B) 640 K (C) 600 K (D) 550 K

13. Pressure of 10 moles of an ideal gas is changed from 2 atm to 1 atm against constant external pressure without change in temperature. If surrounding temperature (300 K) and pressure (1 atm) always remains constant then calculate total entropy change (



^S_system ⁺



^Ssurrounding) for given process.

[Given :



n2 = 0.70 and R = 8.0 J/mol/K]

(A) 56 J/K (B) 14 J/K (C) 16 J/K (D) None of these

14. For a perfectly crystalline solid C_p,m = aT³ + bT, where a and b constant. If C_p,m is 0.40 J/K mol at 10 K and 0.92 J/K mol at 20 K, then molar entropy at 20 K is :

(A) 0.92 J/K mol (B) 8.66 J/K mol (C) 0.813 J/K mol (D) None of these

15. When two equal sized pieces of the same metal at different temperatures T_h (hot piece) and T_c(cold piece) are brought into contact into thermal contact and isolated from it's surrounding. The total change in entropy of system is given by

(A) C ln

16. Reactions involving gold have been of particular interest to a chemist . Consider the following reactions, Au(OH)₃ + 4 HCl



^HAuCl₄ ^{+ 3 H}₂^{O ,}



^{H =}



^{28 kCal}

Au(OH)₃ + 4 HBr



^HAuBr₄ ^{+ 3 H}₂^{O ,}



^{H =}



^{36.8 kCal}

In an experiment there was an absorption of 0.44 kCal when one mole of HAuBr₄ was mixed with 4 moles of HCl . What is the percentage conversion of HAuBr₄ into HAuCl₄ ?

(A)

0.5 %

^{(B) 0.6 % (C) 5 % (D) 50 %}

17. Ethanol can undergoes decomposition to form two sets of products

C₂H₅OH (g)



if the molar ratio of C₂H₄ to CH₃CHO is 8 : 1 in a set of product gases, then the enthalpy involved in the decomposition of 1 mole of ethanol is

(A) 65.98 kJ (B) 48.137 kJ (C) 48.46 kJ (D) 57.22 kJ

18. (i) Cis



²



^butene



^trans



²



^butene,



^H₁

(ii) Cis



²



^butene



¹



^butene,



^H₂

(iii) Trans



²



butene is more stable than cis



²



^butene.

(iv) Enthalpy of combustion of 1



^butene,



^{H =}



649.8 kCal/mol (v) 9



^H₁ ^{+ 5}



^H₂ ^{= 0}

(vi) Enthalpy of combustion of trans 2



butene,



H =



647.0 kCal/mol.

The value of



H₁ &



H₂ inKCal/mole are

(A)



^{1.0 , 1.8} (B) 1.8, -1.0 (C) –5, 9 (D) –2, 3.6

19. The enthalpy changes of the following reactions at 27°C are Na(s) +

2

1

Cl₂ (g)



^{NaCl (s)}



_rH = –411 kJ/mol

H₂(g) + S (s) + 2O₂ (g)



^H₂^SO₄ ^(l)



_r^{H =} –811 kJ/mol 2Na(s) + S(s) + 2O₂ (g)



^Na₂^SO₄ ^(s)



_rH = –1382 kJ/mol

2

1

H₂(g) +

2

1

Cl₂(g)



^{HCl (g)}



_r^{H =} –92 kJ/mol; R = 8.3 J/K-mol

from these data, the heat change of reaction at constant volume ( in kJ/mol) at 27°C for the process 2NaCl (s) + H₂SO₄ (l)



^Na₂^SO₄ (s) + 2HCl (g) is

(A) 67 (B) 62.02 (C) 71.98 (D) None

20. The standard enthalpy of formation of FeO & Fe₂O₃ is 65 kcal mol^1 and 197kcalmol^1 respectively.

A mixture of two oxides contains FeO & Fe₂O₃ in the mole ratio 2 : 1. If by oxidation, it is changed into a 1 : 2 mole ratio mixture, how much of thermal energy will be released per mole of the initial mixture ? (A) 13.4 kcal/mole (B) 14.6 kcal/mole (C) 15.7 kcal/mole (D) 16.8 kcal/mole

21. An athelete is given 100 g of glucose (C₆H₁₂O₆) of energy equivalent to 1560 kJ. He utilises 50 percent of this gained energy in the event. In order to avoid storage of energy in the body, the weight of water he would need to perspire is- (The enthalpy of evaporation of water is 44 kJ/mole.)

(A) 319 gm (B) 422 gm (C) 293 gm (D) 378 gm

22. The heat of formation of C₂H₅OH() is  66 kcal/mole. The heat of combustion of CH₃OCH₃ (g) is – 348 kcal/mole. H_f for H₂O and CO₂ are 68 kcal/mole and 94 kcal/mole respectively. Then, the H for the isomerisation reaction C₂H₅OH ()  CH₃OCH₃(g), and E for the same are

(A)H = 18 kcal/mole, E = 17.301 kcal/mole (B) H = 22 kcal/mole, E = 21.408 kcal/mole (C) H = 26 kcal/mole, E = 25.709 kcal/mole (D) H = 30 kcal/mole, E = 28.522 kcal/mole

23. AB, A₂ and B₂ are diatomic molecules. If the bond enthalpies of A₂, AB & B₂ are in the ratio 1 : 1 : 0.5 and enthalpy of formation of AB from A₂ and B₂ is – 100 kJ/mol^–1. What is the bond enthalpy of A₂. (A) 400 kJ/mol (B) 200 kJ/mol (C) 100 kJ/mol (D) 300 kJ/mol

24. Enthalpy of polymerisation of ethylene, as represented by the reaction, nCH₂=CH₂  CH₂CH₂)_n is

100 kJ per mole of ethylene. Given bond enthalpy of C=C bond is 600 kJ mol^1, enthalpy of CC bond (in kJ mol) will be :

(A) 116.7 (B) 350 (C) 700 (D) indeterminate

25. Substance A₂B(g) can undergoes decomposition to form two set of products :

If the molar ratio of A₂(g) to A(g) is 5 : 3 in a set of product gases, then the energy involved in the decomposition of 1 mole of A₂B₂ , is :

(A) 48.75 kJ/mol (B) 43.73 kJ/mol (C) 46.25 kJ/mol (D) None of these 26. For the hypothetical reaction

A₂(g) + B₂(g) 2AB(g)

If _rGº and _rSº are 20 kJ/mol and –20 JK^–1 mol^–1 respectively at 200 K.

_rC_p is 20 JK^–1 mol^–1 then _rHº at 400 K is :

(A) 20 kJ/mol (B) 7.98 kJ/mol (C) 28 kJ/mol (D) None of these

27. Enthalpy of neutralization of H₃PO₃ acid is – 106.68 kJ/mol using NaOH. If enthalpy of neutralization of HCl by NaOH is –55.84 kJ/mol. Calculate H_ionization of H₃PO₃ into its ions :

(A) 50.84 kJ/mol (B) 5 kJ/mol (C) 2.5 kJ/mol (D) None of these

28. The enthalpy of neutralisation of a weak acid in 1 M solution with a strong base is – 56.1 kJ mol^–1. If the enthalpy of ionization of the acid is 1.5 kJ mol^–1 and enthalpy of neutralization of the strong acid with a strong base is – 57.3 kJ equiv^–1 , what is the % ionization of the weak acid in molar solution (assume the acid to be monobasic)?

(A) 10 (B) 15 (C) 20 (D) 25

29. The heat of formation of HCl at 348 K from the following data, will be 0.5 H₂(g) + 0.5 Cl₂ (g)  HCl H°₂₉₈ = – 22060 cal The mean heat capacities over this temperature range are,

H₂(g), C_P = 6.82 cal mol^–1 K^–1 ; Cl₂ (g), C_p = 7.71 cal mol^–1 K^–1 ; HCl (g), C_P = 6.81 cal mol^–1 K^–1 (A) – 20095 cal (B) – 32758 cal (C) – 37725 cal (D) – 22083 cal

30. The average XeF bond energy is 34 kcal/mol, first I.E. of Xe is 279 kcal/mol, electron affinity of F is 85 kcal/mol & bond dissociation energy of F₂ is 38 kcal/mol. Then, the enthalpy change for the reaction

XeF₄  Xe⁺ + F^ + F₂ + F will be

(A) 367 kcal/mole (B) 425 kcal/mole (C) 292 kcal/mole (D) 392 kcal/mole

31. Combustion of sucrose is used by aerobic organisms for providing energy for the life sustaining processes.

If all the capturing of energy from the reaction is done through electrical process (non P–V work) then calculate maximum available energy which can be captured by combustion of 34.2 g of sucrose

Given : H_combustion (sucrose) = – 6000 kJ mol^–1

S_combustion = 180 J/K - mol and body temperature is 300 K

(A) 600 kJ (B) 594.6 kJ (C) 5.4 kJ (D) 605.4 kJ

32. The enthalpy of tetramerization of X in gas phase (4X(g)



^X₄^{(g)) is} – 100 kJ/mol at 300 K.

The enthalpy of vaporisation for liquid X and X₄ are respectively 30 kJ/mol and 72 kJ/mol respectively.



S for tetramerization of X in liquid phase is – 125 J / K mol at 300 K.

What is the



G at 300 K for tetramerization of X in liquid phase ?

(A) –52 kJ/mol (B) –89.5 kJ/mol (C) –14.5 kJ/mol (D) None of these One or More Than One Correct Answer Type :

33. The normal boiling point of a liquid 'A' is 350 K.H_vap at normal boiling point is 35 kJ/mole. Pick out the correct statement(s). (Assume DH_vap to be independent of pressure).

(A) Svaporisation > 100 KJ/mole at 350 K and 0.5 atm (B) Svaporisation < 100 KJ/mole at 350 K and 0.5 atm (C) Svaporisation < 100 KJ/mole at 350 K and 2 atm

34. Which of the following statement(s) is/are false : (A)



_r^{S for}

2

1

N₂(g)



N(g) is positive

(B)



^G_system is always zero for a reversible process in a closed system (C)



G° for an ideal gas is a function of temperature and pressure (D) entropy of a closed system is always maximized at equilibrium 35. Which statement is / are correct:

(A) Final temperature in reversible adiabatic expansion is lesser than in irreversible adiabatic expansion.

(B) When heat is supplied to an ideal gas in an isothermal process, kinetic energy of gas will increase (C) When an ideal gas is subjected to adiabatic expansion it gets cooled

(D) Entropy increases in atomisation of dihydrogen 36. Which statement is / are correct:

(A) w_adiabatic > w_isothermal in an ideal gas compression from same initial state to same final state

(B) The value of

  





 









v p

C C

remains constant for diatomic gas at all temperature (C) Entropy increases when an ideal gas expanded isothermally.

(D)



_rH &



_rS both are + ve for the decomposition of MgCO₃(s) . 37. In isothermal ideal gas compression:

(A) w is +ve (B)



^{H is zero (C)}



^S_gas ^{is +ve (D)}



^{G is +ve}

38. Which of the following is true for reversible adiabatic process involving an ideal gas?

(A) Gas with higher



has high magnitude of slope in a P (y-axis) v/s T (x-axis) curve (B) Gas with higher



has high magnitude of slope in a V (y-axis) v/s T (x-axis) curve (C) Gas with higher



has high magnitude of slope in a P (y-axis) v/s V (x-axis) curve (D) Gas with higher



has low magnitude of slope in a P (y-axis) v/s T (x-axis) curve

39. One mole of an ideal diatomic gas (C_v = 5 cal) was transformed from initial 25°C and 1 L to the state when temperature is 100°C and volume 10 L. Then for this process(R = 2 calories/mol/K) (take calories as unit of energy and kelvin for temp)

(A) H = 525 (B) S = 5 ln 298

373 + 2 ln 10 (C) E = 525 (D) G of the process can not be calculated using given information.

40. Consider the reactions

(i) S (rhombic) + 3/2 O₂(g)  SO₃(g), H₁ (ii) S (monoclinic) + 3/2O₂(g)  SO₃(g), H₂ (iii) S (rhombic) + O₃(g)  SO₃(g), H₃ (iv) S (monoclinic) + O₃(g)  SO₃(g), H₄ (A) H₁ < H₂ < H₄ (magnitude only) (B) H₁ < H₃ < H₄ (magnitude only)

(C) H₁ < H₂ = _H₄ (magnitude only) (D) H₁ + H₄ = _H₃

41. The normal boiling point of a liquid `X` is 400 K. Which of the following statement is true about the process X (l)  X(g)?

(A) at 400 K and 1 atm pressure G = 0 (B) at 400 K and 2 atm pressure G = + ve (C) at 400 K and 0.1 atm presure G = – ve (D) at 410 K and 1 atm pressure G = + ve

42. 100 ml 0.5 N H₂SO₄ (strong acid) is neutralised with 200 ml 0.2M NH₄OH in a constant pressure Calorimeter which results in tem perature rise of 1.4 °C. If heat c apac ity of Calor im eter c ontent is 1.5 kJ/°C. Which statement is/are correct

Given : HCl + NaOH



^{NaCl + H}₂^{O + 57 kJ}

CH₃COOH + NH₄OH



CH₃COONH₄ + H₂O + 48.1 kJ (A) Enthalpy of neutralisation of HCl v/s NH₄OH is – 52.5 kJ/mol

(B) Enthalpy of dissociation (ionization) of NH₄OH is 4.5 kJ/mol (C) Enthalpy of dissociation of CH₃COOH is 4.6 kJ/mol

(D)



^{H for 2H}₂^O(l)



^2H+ (aq.) + 2OH¯(aq.) is 114 kJ

43. From the following data at 25°C

Reaction



_r^H° kJ/mol

2

1

H₂(g) +

2

1

O₂(g)



^{OH (g) 42}

H₂(g) +

2

1

O₂(g)



^H₂^O(g) –242

H₂(g)



2H(g) 436

O₂(g)



^{2O(g) 495}

Which of the following statement(s) is/are correct:

(A)



_rH° for the reaction H₂O (g)



2H(g) + O(g) is 925.5 kJ/mol (B)



_rH° for the reaction OH(g)



H(g) + O(g) is 502 kJ/mol (C) Enthalpy of formation of H(g) is –218 kJ/mol

(D) Enthalpy of formation of OH(g) is 42 kJ/mol 44. Which of the following is true ?

(A) For the reaction CaCO₃(calcite)



^CaCO₃ (aragonite)

given :



_f

G

^o₂₉₈(calcite) = –1128.8 kJ/mol,



_f

G

^o₂₉₈(aragonite) = – 1127.75 kJ/mol, then calcite form is thermodynamically more stable at standard conditions.

(B) For the reaction,

(a) C(diamond) + 2H₂ (g)



CH₄(g)



H₁ (b) C(g) + 4H(g)



^CH₄^(g)



^H₂

then more heat is evolved in reaction (b).

(C)



_f^{H° (I}₂^{, g) =}



_sub^{H [I}₂, s] at 25°C.

(D) For the exothermic reaction 2Ag(s) + 1/2 O₂(g)



2Ag₂O(s) at 298 K.



H <



U 45. Which of the following do(es) not represent



H formation of the product.

(A)

2

1

H₂(g) + (aq)



^{H+(aq) (B)}

3

2

O₃(g)



^O₂^{(g) + e¯}

(C)

NH

^₄(g) + Cl^–(g)



^NH₄^{Cl(s) (D) P}₄(black) + 5O₂ (g)



^P₄^O₁₀^(s)

46. Which of the following statement(s) is/are true?

(A) When (



^G_system⁾_T,P < 0; the reaction must be exothermic (B)



_f H° (S, monoclinic)



⁰

(C) If dissociation enthalpy of CH₄(g) is 1656 kJ/mole and C₂H₆ (g) is 2812 kJ/mole, then value of C–C bond enthalpy will be 328 kJ/mole

(D) If H⁺(aq) + OH^–(aq)



^H₂^O(l)



_rH° = –56 kJ/mol



_f ^H°(H₂O, g) = –242 kJ/mole; Enthalpy of vaporization of liquid water = 44 kJ/mol then,



_f ^H°(OH^–, aq) will be –142 kJ/mole

47. Select the option in which heat evolved is maximum.

Given :



_fH° (CO₂,g) = – 75 kCal/mol ;



_fH° (CO,g) = – 25 kCal/mol

The product will be CO if excess amount of carbon is present and CO₂ if excess O₂ is present (A) 10 moles of carbon and 4.5 moles of O₂

(B) 24 gm of carbon and 64 gm of O₂ (C) 4 moles of carbon and 3.5 moles of O₂ (D) 30 gm of carbon and 80 gm of O₂

1. MATCH THE COLUMN

1.1 Columm-I Columm-II

(A) Reversible isothermal expansion of an ideal gas (p) w = –2.303 nRT log _^











1 2

V V

(B) Reversible adiabatic compression of an ideal gas (q) PV^ = constant (C) Irreversible adiabatic expansion of an ideal gas (r) w = ₍^nR₁₎



 (T₂ – T₁) (D) Irreversible isothermal compression of an ideal gas (s) H = 0

1.2 Columm - I Columm - II

(A) C (s, graphite) + O₂(g)  CO₂(g) (p) Hº_combustion

(B) C(s, graphite)  C(g) (q) Hº_formation

(C) CO(g) + 2

1O₂(g)  CO₂(g) (r) Hºatomization

(D) CH₄(g)  C(g) + 4H(g) (s) Hºsublimation

1.3 Column-I, may have more than one matching options in column-II

Column-I Column-II

(A) Reversible condensation of vapour (p)



^S_system ^{> 0}

(B) Irreversible adiabatic compression of an ideal gas (q)



^S_system ^{< 0}

(C) Isothermal free expansion of an ideal gas in vacuum (r)



^S_surounding ^{< 0}

(D) Reversible adiabatic expansion of an ideal gas (s)



^S_surounding ^{= 0}

1.4 Column–I Column–II

(Related to process) (Related to system)

(A) Fusion at melting point (p)



^{G = 0}

(B) Vapourisation at boiling point (q)



^{G < 0}

(C) Condensation at triple point (r)



^{S > 0}

(D) Melting at normal boiling point (s)

 H  ~  U

1.5 Column I Column II

(A) For the process (p) – ve, + ve

In document Thermodynamics (Page 39-46)