**Q1. Which of the following statements is correct about the process of evaporation of water from an open beaker?**

- It is a spontaneous and endothermic process.
- It is a spontaneous and exothermic process.
- It is a non-spontaneous and endothermic process.
- It is a non-spontaneous and exothermic process.

**Answer :- (1)**

**Q2. The absolute entropy of a perfectly crystalline substance is zero at 0 K. The given statement is known as**

- Second law of Thermodynamics
- Third law of Thermodynamics
- Law of chemical equilibrium
- Law of calorimetery

**Answer :- (2)**

**Q3. Which of the following process does NOT occur during a chemical reaction?**

- Rearrangement of atoms
- Collision between molecules
- Formation of new atoms
- Formation of new products from the elements that are not present in the reactants

**Answer :- (4)**

**Q4. For the reaction Hg (l) ———> Hg (g) , the entropy change will have the sign:**

- Negative
- Positive
- Both positive and negative
- None of the above

**Answer :- (2)**

**Q5. Which of the following is NOT a state function?**

- PV
- q + w
- q
_{rev}/T - q

**Answer :- (4)**

**Q6. The enthalpies of all elements in their standard states are**

- infinite
- zero
- negative
- positive

**Answer :- (2)**

**Q7. The solubility of fluorides is much less as compared to corresponding chlorides**

- because of high ionization energy.
- because of high lattice enthalpy.
- because of low ionization energy.
- because of low lattice enthalpy.

**Answer :- (2)**

**Q8. On which of the following factors the enthalpy change of a reaction is NOT dependent?**

- State of reactants and products
- Nature of reactants and products
- Enthalpy of reactants and products
- Various intermediate reactions

**Answer :- (4)**

**Q9. Which of the following is true about a spontaneous process?**

- Gibbs energy change is 0.
- Gibbs energy change is less than 0.
- Gibbs energy change is greater than 0.
- Spontaneity does not depend on Gibbs energy.

**Answer :- (2)**

**Q10. Which of the following process is NOT included in phase transformation?**

- Vaporization
- Fusion
- Ionisation
- Sublimation

**Answer :- (3)**

**Q11. Which of the following relations is correct for an adiabatic process?**

- ∆U = q
- P∆V = 0
- ∆q = 0
- q = + w

**Answer :- (3)**

**Q12. Which of the following property is NOT an intensive property?**

- Temperature
- Viscosity
- Pressure
- Volume

**Answer :- (4)**

**Q13. The difference between Cp and Cv is equal to**

- 2 kcal mol
^{-1} - 1.99 cal
- 8.314 JK
^{-1}mol^{-1} - 8.314 ergs K
^{-1}mol^{-1}

**Answer :- ()**

**Q14. Born-Haber cycle is used to calculate:**

- Lattice enthalpy
- Enthalpy of formation
- Enthalpy of sublimation
- Enthalpy of fusion

**Answer :- (1)**

**Q15. What is the value of the enthalpy of neutralization for all strong acids and bases?**

- -57.1 kJ
- 57.1 kJ
- 1 kJ
- -1 kJ

**Answer :- (1)**

**Q16. What is the change in the entropy of water, When ice melts into water?**

- Entropy of water decreases.
- Entropy of water increases.
- Entropy of water becomes zero.
- Entropy of water remains same.

**Answer :- (2)**

**Q17. Which of the following is a state function?**

- Heat
- Volume
- Pressure
- Internal energy

**Answer :- (4)**

**Q18. On increasing the temperature the entropy of the system**

- Increases
- Decreases
- Become zero
- None of these

**Answer :- (1)**

**Q19. A system absorbs 500 kJ heat and performs 250 kJ work on the surroundings. The increase in internal energy of the system is:**

- 750 kJ
- 250 kJ
- 500 kJ
- 1000 kJ

**Answer :- (2)**

**Q20. What is the enthalpy called when one mole of compound is formed under standard conditions from one mole of its constituent elements in their standard state?**

- Enthalpy of formation
- Enthalpy of combustion
- Enthalpy of bond dissociation
- Enthalpy of phase change

**Answer :- ()**

**Q21. What happens to the ions, when an ionic compound dissolves in a solvent?**

- They leave their ordered position in the crystal lattice and gets hydrated.
- They leave their ordered position in the crystal lattice and doesn’t hydrate.
- They doesn’t leave their ordered position in the crystal lattice and gets hydrated.
- None of the above.

**Answer :- (1)**

**Q22. Evaporation of water is:**

- A process in which no heat changes occur.
- A process accompanied by chemical reaction.
- An exothermic change.
- An endothermic change.

**Answer :- (4)**

**Q23. The process in which no exchange of heat takes place between system and surrounding is known as**

- Isobaric process
- Adiabatic process
- Isothermal process
- Isochoric process

**Answer :- (2)**

**Q24. Enthalpy of hydration of CuSO _{4}.5H_{2}O is:**

- positive
- negative
- zero
- not measurable

**Answer :- (2)**

**Q25. For the reaction,**

A (g) +2B (g) → 2C (g) +3D(g)

the change of enthalpy at 27^{o}C is 19 kCal. The Value of ΔE is

- 21.2 kcal
- 17.8 kcal
- 18.4 kcal
- 20.6 kcal

**Answer :- (2)**

**Q26. What are the units of molar heat capacity?**

- J K
^{-1}mol^{-1} - J K
- J K
^{-1} - J

**Answer :- (1)**

**Q27. Enthalpy change for a cyclic process is**

- zero
- positive
- negative
- not measurable

**Answer :- (1)**

**Q28. The enthalpies of fusion for all reactions are**

- Positive
- Negative
- Zero
- Depends on the type of substance

**Answer :- (1)**

**Q29. The sum of internal energy and pressure-volume work is defined as**

- Enthalpy
- Entropy
- Heat capacity
- Free energy

**Answer :- (1)**

**Q30. Spontaneous processes proceed:**

- Till equilibrium is achieved.
- Till conditions are favorable.
- Till heat is supplied.
- Till reactant is supplied.

**Answer :- (1)**

**Q31. In the evaporation of water, the entropy**

- decreases
- increases
- does not change
- first increases and then decreases

**Answer :- (2)**

**Q32. What does term specific heat implies?**

- Heat capacity of 1 g of sample
- Heat capacity of 1 mole of sample
- Heat capacity of 1Kg of sample
- Heat capacity of 1000 g of sample

**Answer :- (1)**

**Q33. For a spontaneous chemical process, the free energy change is**

- positive
- negative
- zero
- not measurable

**Answer :- (2)**

**Q34. The increasing order of enthalpy of vaporization of NH _{3}, PH_{3}, and AsH_{3} is**

- NH
_{3}, PH_{3}, AsH_{3} - AsH
_{3}, PH_{3}, NH_{3} - NH
_{3}, AsH_{3}, PH_{3} - PH
_{3}, AsH_{3}, NH_{3}

**Answer :- (4)**

**Q35. The internal energy of a system is**

- Kinetic energy only
- Potential energy only
- Kinetic as well as potential energy
- Unpredictable

**Answer :- (3)**

**Q36. In Born-Haber cycle, the sum of the enthalpy changes around a cycle is**

- Zero
- Constant
- Negative integer
- Positive integer

**Answer :- (1)**

**Q37. When there will be increase in the internal energy of a system?**

- If the system gains heat and performs work.
- If the system gains heat and work performed on the system both are positive.
- If the system loses heat and performs work.
- If the system loses heat and work performed on the system both are negative.

**Answer :- (2)**

**Q38. Standard enthalpy of vapourisation ∆ _{vap} H^{o} for water at 100^{o}C is 40.66 kJ mol^{-1}. The internal energy of vaporization of water at 100^{o}C (in kJmol-1) is:**

- +37.56
- -43.76
- +43.76
- +40.66

**Answer :- (1)**

**Q39. What is the enthalpy called when one mole of compound reacts completely with excess oxygen under standard conditions?**

- Enthalpy of solution
- Enthalpy of atomization
- Lattice enthalpy
- Enthalpy of combustion

**Answer :- (4)**

**Q40. Heat change of a process in which volume remains constant is given by:**

- ∆H
- ∆n
- ∆G
- ∆U

**Answer :- (4)**