Exam-Style Mock Test | Class 11 Chemistry: Thermodynamics

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Quiz: Thermodynamics – Certificate Challenge
Total questions: 495
Questions to attempt: 100 random
Time allotted: 100 minutes
Certificate pass score: 70%
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Certificate: Yes
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Thermodynamics – Progressive Test

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1 / 50

1. The distinction between heat and temperature is best represented by the statement

a) temperature is measured only in , while heat is measured only in

b) heat and temperature are always identical because both rise during warming

c) heat is a measure of hotness, while temperature is energy transfer

d) heat is energy transfer; temperature describes thermal state

2 / 50

2. A sample of gas is taken around a complete cycle and returns to its initial pressure, volume, temperature, and composition. The internal energy change for the cycle is

a) positive because a cycle has many steps

b) negative because the gas returns

c) zero because is a state function

d) equal to the total distance moved by the piston

3 / 50

3. At , a reaction has . Use and . The equilibrium constant is closest to

4 / 50

4. A spontaneous process is best described as a process that

a) must occur instantly

b) must always have

c) must always release heat

d) has a natural tendency to occur under given conditions

5 / 50

5. A reaction at has . The entropy change of the surroundings is

6 / 50

6. The standard enthalpy of formation of a compound is the enthalpy change when

a) forms from standard-state elements

b) the compound is separated into ions in the gas phase only

c) any amount of compound dissolves in water

d) of any compound is burned completely

7 / 50

7. In a rigid bomb calorimeter, the calorimeter absorbs of heat from a combustion reaction. For the reacting system, the internal energy change is

8 / 50

8. A reaction at has . Use and . The standard Gibbs energy change is closest to

9 / 50

9. Two gas containers have the same gas at the same initial conditions.
I. Container P has a rigid conducting wall.
II. Container Q has an insulated movable piston.
The better comparison is

a) both P and Q must allow matter exchange

b) P cannot exchange heat but can change volume; Q can exchange heat but cannot change volume

c) both P and Q must be isolated systems

d) P can exchange heat but cannot change volume; Q cannot exchange heat but can change volume

10 / 50

10. An ionic compound forms from and with lattice formation enthalpy . The hydration enthalpies are and . The enthalpy of solution of is closest to

11 / 50

11. In a Born-Haber cycle for , the step is

a) electron gain enthalpy of sodium

b) lattice enthalpy of sodium chloride

c) bond dissociation enthalpy of chlorine

d) first ionization enthalpy of sodium

12 / 50

12. A reaction has and . The equilibrium constant is expected to increase with temperature because

a) is independent of temperature for all endothermic reactions

b) becomes more negative as increases

c) becomes more positive as increases

d) has no role in

13 / 50

13. The expression is equivalent to the natural logarithm form because

b) changes volume from to

d) for all values of

14 / 50

14. A metal sample absorbs of heat, and its temperature rises by . The specific heat capacity of the metal is

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15. A final comparison of criteria is given below.

Criterion	Meaning under suitable conditions
P.	spontaneous process
Q. at constant	forward process favoured
R. at constant	equilibrium
S.	equilibrium composition

The correctly stated criteria are

a) P, Q, R, and S

b) Q and R only

c) P, Q, and R only

d) P and Q only

16 / 50

16. The statement that best separates internal energy from heat is

a) internal energy can be measured only in , while heat is measured only in

b) both heat and internal energy are path functions

c) heat is stored inside a body, while internal energy crosses the boundary only during cooling

d) internal energy is a state property; heat is energy transfer

17 / 50

17. A reaction in a calorimeter warms both the solution and the calorimeter. The solution absorbs , and the calorimeter absorbs . For the reacting system, the heat change is

18 / 50

18. A reaction has at a given temperature. The sign of is

a) zero for every

b) unrelated to

c) negative

d) positive

19 / 50

19. Standard thermodynamic data are reported for substances in their standard states. The statement that best avoids a common confusion is

a) standard state requires all substances to be gases

b) standard state means every enthalpy and entropy value is zero

c) standard state and always mean exactly the same condition

d) standard state is not the same as

20 / 50

20. A wall is described as permeable and diathermic. This means the wall allows

a) heat transfer but no matter transfer

b) matter transfer but no heat transfer

c) neither matter transfer nor heat transfer

d) matter transfer and heat transfer

21 / 50

21. A reaction has and . The temperature above which the reaction becomes non-spontaneous is

22 / 50

22. A graph is drawn with temperature rise on the vertical axis and heat supplied on the horizontal axis for equal masses of two substances. The steeper line represents the substance with

a) negative absolute temperature

b) larger heat capacity

c) zero heat capacity

d) smaller heat capacity

23 / 50

23. Two samples of the same metal are at the same initial temperature. Sample P has mass , and Sample Q has mass . If both are heated through the same , the heat required for Q is

a) half that for P

b) equal to that for P

c) four times that for P

d) twice that for P

24 / 50

24. In a non-standard reaction mixture, , but . This means the mixture is

a) at equilibrium for that mixture

b) impossible because and must be equal

c) strongly forward-spontaneous because

d) non-spontaneous in both directions

25 / 50

25. Two objects are at and . They are brought into thermal contact, and the cooler object is chosen as the system. The sign of heat for the cooler object during the initial contact is

a) zero, because both objects have temperature in

b) undefined, because heat cannot flow between solids

c) negative, because heat leaves the cooler object

d) positive, because heat enters the cooler object

26 / 50

26. For a reaction at a fixed temperature, the current mixture has . The forward direction is favoured because

b) necessarily

27 / 50

27. For the reaction , the reaction quotient in terms of partial pressures is

28 / 50

28. A rigid sealed vessel contains a gas. The gas is heated, but the wall does not move. The work associated with volume change is

a) zero because volume does not change

b) positive because heat is supplied

c) negative because temperature rises

d) equal to the pressure of the gas

29 / 50

29. A Born-Haber cycle for is summarized as:

If all terms except are known, the lattice enthalpy is obtained by

b) for every ionic solid

30 / 50

30. For a reaction with and , the temperature at which is

31 / 50

31. The table gives bond-count information for a reaction.

Step	Bond event	Energy effect using positive bond enthalpies
P	bonds in reactants broken	energy absorbed
Q	bonds in products formed	energy released
R	bonds formed counted as positive addition to	always correct
S	bonds broken counted in	correct

The row with the incorrect interpretation is

a) Q

b) S

c) R

d) P

32 / 50

32. One mole of an ideal gas expands reversibly and isothermally at from to . Use and . For the gas, the values of , , and are closest to

a) , ,

b) , ,

c) , ,

d) , ,

33 / 50

33. During a process, a system releases of heat and does of work on the surroundings. The value of is

34 / 50

34. A gas in a sealed vessel is heated, and its temperature rises. At the molecular level, this most directly suggests a change in

a) only the label on the vessel

b) atomic numbers of all atoms

c) gravitational energy of the laboratory building

d) internal energy of the gas

35 / 50

35. A student writes, “Because , a larger always makes more positive.” The correction is that

a) is negative, so the sign changes

b) increase makes more negative

c) has no logarithm in the relation

d) is positive for every value of

36 / 50

36. Average bond enthalpy values are often approximate for polyatomic molecules because

a) the values are measured only for liquids at zero pressure

b) bond breaking never requires energy

c) bond enthalpy depends on molecular surroundings

d) bond enthalpy is independent of molecular environment in every case

37 / 50

37. Use bond enthalpies , , , and . For , one bond and one bond are broken, while one bond and one bond are formed. The approximate is

38 / 50

38. Use the graph description below.

An energy profile is drawn with enthalpy on the vertical axis and progress of reaction on the horizontal axis. The products are at a lower enthalpy level than the reactants.

The reaction represented by the graph is

a) exothermic with

b) endothermic with

c) isothermal with

d) impossible because products cannot have lower enthalpy

39 / 50

39. The thermochemical equation has . The enthalpy change for formation of of from the same elements is

40 / 50

40. Study the table and identify the inconsistent row for ideal-gas heat capacities.

Row	Statement	Comment
P		constant-volume heating
Q		constant-pressure heating
R		ideal gas relation
S		extra heat is needed at constant pressure

a) S

b) Q

c) P

d) R

41 / 50

41. Study the table and choose the row that misinterprets the - work graph.

Row	Graph feature	Interpretation
P	Area under - curve	magnitude of -work
Q	Expansion from lower to higher	negative for the system
R	Compression from higher to lower	positive for the system
S	Zero slope horizontal line	zero work for every process

a) S

b) Q

c) R

d) P

42 / 50

42. A sample absorbs the same heat in two trials. In Trial P, its temperature rise is . In Trial Q, its temperature rise is . The heat capacity in Trial P compared with Trial Q is

a) four times as large

b) half as large

c) twice as large

d) the same only if

43 / 50

43. A gas expands by against external pressure and absorbs of heat. Use . The value of is

44 / 50

44. A system changes from state I to state II. State I is described by , , and , while state II is described by , , and . This description mainly represents

a) a boundary that must be imaginary

b) a change of state

c) a system without measurable properties

d) a proof that no energy transfer occurred

45 / 50

45. A reversible isothermal work calculation uses and . The safest way to form the volume ratio is

a) , keeping the written numbers exactly as given

b) , because logarithms use differences

c) , because initial volume must be subtracted from final volume

d) use the same unit in numerator and denominator

46 / 50

46. A straight-line plot of against cuts the axis at . The reaction has . The value of is

47 / 50

47. A system absorbs of heat and has of work done on it. The change in internal energy is

48 / 50

48. The following signs are reported for four reactions.

Reaction			Temperature favourability
P			all
Q			high
R			low
S			all

The row with the wrong temperature favourability is

a) P

b) R

c) Q

d) S

49 / 50

49. Process P has , and Process Q has . If they are coupled in the same overall direction, the combined process has

a) , non-spontaneous

b) , equilibrium

c) , spontaneous

d) , spontaneous

50 / 50

50. A reaction has and . At , the reaction mixture has . Use and . The actual Gibbs energy change is closest to

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Thermodynamics Mock Test – Class 11 Chemistry

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