Quiz: Chapter 7 - thermodynamics

1 Which of the following is a state function?

Heat (q) Work (w) Internal energy (U) Both heat and work

2 First law of thermodynamics is based on the law of:

Conservation of mass Conservation of energy Conservation of charge Thermodynamic equilibrium

3 The change in internal energy at constant volume is equal to:

qp w qv ΔH

4 Which of the following is NOT a thermodynamic state function?

Enthalpy Heat Entropy Internal energy

5 Enthalpy is defined as:

H = q + w H = U + PV H = qv H = TΔS

6 ΔH is equal to qp when the process occurs at:

Constant temperature Constant pressure Constant volume Constant entropy

7 Which process has ΔU = 0?

Adiabatic Isothermal Isobaric Isoboric

8 When a gas expands adiabatically, it:

Gains heat Loses heat Does no work Does work at constant temperature

9 Work done by the system is positive when:

Gas is compressed No volume change Gas expands Process is isochoric

10 A spontaneous process is one that:

Requires external energy Occurs with increase in entropy Occurs at constant pressure Decreases the total energy

11 In which of the following processes no heat is exchanged?

Isothermal Isochoric Adiabatic Isobaric

12 What does the first law of thermodynamics state?

Energy can be created Energy can be destroyed Energy is constant Work is energy

13 For an endothermic reaction, the sign of ΔH is:

Positive Negative Zero Not defined

14 The SI unit of entropy is:

J J/K J/mol J/mol-K

15 What is the heat capacity of a system?

Energy required to change pressure Energy to raise temp. of kg by 1°C Total internal energy None

16 What does the second law of thermodynamics state?

Energy is created in isolated systems Entropy always decreases Entropy increases in spontaneous processes Enthalpy is conserved

17 A process in which enthalpy remains constant is called:

Isochoric Isobaric Isoenthalpic Isothermal

18 Internal energy of an ideal gas depends on:

Pressure only Temperature only Volume only Enthalpy

19 If ΔH is negative and ΔS is positive, the reaction is:

Always spontaneous Never spontaneous Spontaneous at high temperature only Spontaneous at low temperature only

20 A thermodynamic process in which the temperature remains constant is:

Isochoric Isothermal Isobaric Adiabatic

21 Work done in an isochoric process is:

Maximum Positive Zero Negative

22 Which of the following defines Gibbs free energy?

G = H + TS G = H - TS G = U - TS G = PV - TS

23 If ΔG = 0, the system is:

At equilibrium Spontaneous Non-spontaneous Reversible

24 In an exothermic reaction:

ΔH is positive Heat is absorbed ΔH is negative ΔS is always positive

25 The value of ΔU for an isothermal process is:

Maximum Zero Minimum Infinite

26 The standard enthalpy of formation of elements in their natural state is:

Zero Positive Negative Depends on element

27 Which term represents heat change at constant pressure?

qv qp w ΔS

28 A process is non-spontaneous when ΔG is:

Zero Positive Negative Exothermic

29 Entropy of the universe:

Always decreases Always increases Remains constant Is unpredictable

30 In a cyclic process, the net change in internal energy is:

Zero One Infinite Negative

31 Heat and work are:

State functions Path functions Extensive properties Intensive properties

32 When ΔG < 0, the process is:

Non-spontaneous At equilibrium Spontaneous Endothermic

33 Which law states energy cannot be created or destroyed?

Zeroth First Second Third

34 What is the work done in free expansion of a gas?

Maximum Zero Positive Negative

35 Spontaneity of a reaction depends upon:

ΔH ΔS ΔG Temperature

36 The first law of thermodynamics relates:

Pressure and Volume Work and Temperature Internal energy, heat, and work Entropy and energy

37 During compression of a gas, work done is:

Positive Zero Negative None

38 An example of isobaric process is:

Heating water in an open container Filling a gas in sealed balloon Melting of ice at 0°C Compression in piston

39 The third law of thermodynamics deals with:

Absolute zero temperature Entropy of universe Enthalpy change Work done

40 Which of the following quantities is zero at absolute zero?

Enthalpy Temperature Entropy Internal energy

41 Which one is not a path function?

Heat Work Pressure Entropy

42 Which of these is not a spontaneous process?

Melting of ice Flow of water downhill Rusting of iron Water flowing uphill

43 A gas expands from V1 to V2 at constant pressure. The work done is:

P(V1 + V2) P(V2 – V1) P/V V2 – V1/P

44 The amount of energy needed to raise the temperature of 1 mole by 1°C is called:

Heat capacity Specific heat Molar heat capacity Thermal energy

45 An isothermal process has:

Constant energy Constant volume Constant temperature Constant pressure

46 Which of the following is extensive property?

Temperature Pressure Volume Density

47 In an adiabatic process, if a gas expands, it:

Heats up Cools down Remains same Reaches equilibrium

48 A reaction with ΔH > 0 and ΔS < 0 is:

Always spontaneous Sometimes spontaneous Always non-spontaneous Spontaneous at high temperature

49 When a system does work on the surroundings, the sign of w is:

Positive Negative Zero Undefined

50 Which of the following quantities increases in a spontaneous process?

Enthalpy Entropy Internal Energy Gibbs Energy

51 The force between two point charges is governed by:

Gauss’s Law Coulomb’s Law Faraday’s Law Ampere’s Law

52 The electric field inside a charged spherical conductor is:

Constant Zero Infinite Proportional to radius

53 Which of the following is a scalar quantity in electrostatics?

Electric field Electric force Electric potential Electric dipole moment

54 The work done in moving a charge in an equipotential surface is:

Positive Negative Zero Infinite

55 The SI unit of electric flux is:

N/C V/m Nm²/C C/N

56 A dielectric material placed between capacitor plates:

Decreases capacitance Increases capacitance Has no effect Increases resistance

57 The potential energy of a dipole in a uniform electric field is minimum when:

θ = 0° θ = 90° θ = 180° θ = 45°

58 Gauss’s Law is most useful for calculating electric fields with:

Arbitrary charge distributions Dipoles High symmetry Non-uniform fields

59 The electric field at the surface of a charged conductor is:

Zero Parallel to the surface Perpendicular to the surface Tangential

60 If the distance between two charges is doubled, the force becomes:

Half Double One-fourth Four times

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Chapter 7: thermodynamics