Thermodynamics Exam For 12th Grade! Quiz

30 Questions | Total Attempts: 66

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Thermodynamics Exam For 12th Grade! Quiz

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Questions and Answers
  • 1. 
    A well stoppered Thermo flask containing some ice cubes is an example of
    • A. 

      Closed system

    • B. 

      Open system

    • C. 

      Isolated system

    • D. 

      Non thermodynamic system

  • 2. 
    Identify the intensive quantity from the following.
    • A. 

      Enthalpy and temperature

    • B. 

      Volume and temperature

    • C. 

      Enthalpy and volume

    • D. 

      Temperature and refractive index

  • 3. 
    For an adiabatic process, which of the following is correct?
    • A. 

      Q = 0

    • B. 

      P∆V = 0

    • C. 

      ∆E = 0

    • D. 

      Q = + W

  • 4. 
    In which of the following, work behaves as a state function?
    • A. 

      Isothermal

    • B. 

      Adiabatic

    • C. 

      Isobaric

    • D. 

      Isochoric

  • 5. 
    When a gas is compressed adiabatically and reversibly the final temperature is:
    • A. 

      Higher than the initial temperature

    • B. 

      Lower than the initial temperature

    • C. 

      The same as initial temperature

    • D. 

      Dependent upon the rate of compression

  • 6. 
    Q = -w is not true for
    • A. 

      Isothermal

    • B. 

      Adiabatic

    • C. 

      Cyclic process

    • D. 

      Both 1 & 3

  • 7. 
    The temperature of an ideal gas increases in an:
    • A. 

      Adiabatic expansion

    • B. 

      Isothermal expansion

    • C. 

      Adiabatic compression

    • D. 

      Isothermal compression

  • 8. 
    Which one is a state function:-
    • A. 

      Heat supplied at constant pressure

    • B. 

      Heat supplied at constant volume

    • C. 

      Enthalpy

    • D. 

      All of the above

  • 9. 
    The work is done by a weightless piston in causing an expansion ΔV (at constant temperature), when the opposing pressure P is variable. What will be the final expression of the work?
    • A. 

      W = - ∫ P∆V

    • B. 

      W= - PΔV

    • C. 

      W = 0

    • D. 

      None of these

  • 10. 
    The work done by 100 calorie of heat in isothermal expansion of ideal gas is:
    • A. 

      418.4 J

    • B. 

      4.184 J

    • C. 

      41.84 J

    • D. 

      None

  • 11. 
    Temperature and heat are not:
    • A. 

      Extensive properties

    • B. 

      Intensive properties

    • C. 

      Intensive and extensive properties respectively

    • D. 

      Extensive and intensive properties respectively

  • 12. 
    One mole of gas absorbs 200 J of heat at constant volume. Its temperature rises from 298 K to 308 K. The change in internal energy is:
    • A. 

      -200 J

    • B. 

      400 J

    • C. 

      200 J

    • D. 

      - 400 j

  • 13. 
    Which statement is true for the reversible process:-
    • A. 

      It takes place in single step

    • B. 

      Driving force is much greater than opposing force

    • C. 

      Work obtain is minimum

    • D. 

      None

  • 14. 
    Both q & w are __________ function & q + w is a ___________ function.
    • A. 

      State, State

    • B. 

      State, path

    • C. 

      Path, state

    • D. 

      Path, path

  • 15. 
    The work done by a system is 8J when 40 J  heat is supplied to it. Calculate the increases in internal energy of the system.
    • A. 

      32 J

    • B. 

      42 J

    • C. 

      48 J

    • D. 

      - 32 J

  • 16. 
    Under which of the following conditions is the relation ΔH=ΔE+PΔV valid for a closed system?
    • A. 

      Constant pressure

    • B. 

      Constant temperature

    • C. 

      Constant temperature and pressure

    • D. 

      Constant temperature pressure and composition

  • 17. 
    ΔvapH for water at 100°C is 40.66 kJ mol-1  The internal energy of vaporization of water at 100°C (in KJ) 
    • A. 

      37.53

    • B. 

      39.08

    • C. 

      42.19

    • D. 

      43.73

  • 18. 
    The difference between heats of reaction at constant pressure and constant volume for the reaction, 2C6H6 (l)+15 O2 (g) → 12CO2(g)+ 6H2O(l) at 25°C in kJ is:
    • A. 

      7.43

    • B. 

      -7.43

    • C. 

      3.72

    • D. 

      -3.72

  • 19. 
    For a gaseous reaction, A(g) + 3B(g) → 3C(g) + 3D(g) ∆E is 17 kCal at 27°C assuming R = 2 Cal /Kmol, the value of ∆H for the above reaction is: 
    • A. 

      15.8 Kcal

    • B. 

      18.2 Kcal

    • C. 

      20.0 Kcal

    • D. 

      16.4 Kcal

  • 20. 
    For CaCO3​(s)→CaO(s)+CO2​(g ) at 977°C, ΔH=174 kJ/mol; then ΔE is:
    • A. 

      160 KJ

    • B. 

      163.6 KJ

    • C. 

      186.4 KJ

    • D. 

      180 KJ

  • 21. 
    The difference in ΔH and ΔU for combustion of methane for the combustion of methane at 250C would be:
    • A. 

      Zero

    • B. 

      2 x 298 x -2 cals

    • C. 

      2 x 298 x -3 cals

    • D. 

      2 x 25 x -3 cals

  • 22. 
    For the system S(s) + O2(g) → SO2(g) 
    • A. 

      ΔH = ΔE

    • B. 

      ΔH > ΔE

    • C. 

      ΔE > ΔH

    • D. 

      ΔH = 0 

  • 23. 
    ΔS for the reaction :  MgCO3(s) → MgO(s) + CO2(g) will be:
    • A. 

      0

    • B. 

      -ve

    • C. 

      +ve

    • D. 

      Infinity

  • 24. 
    In which of the following cases, entropy will decrease:
    • A. 

      Solid changing to liquid

    • B. 

      Expansion of gas

    • C. 

      Crystal dissolve

    • D. 

      Polymerization

  • 25. 
    For the reaction Ag2O(s) → 2Ag(s) + 1/2 O2(g), the value of ΔH=30.56 KJ/mol and ΔS=66 J/Kmol. The temperature at which the free energy change for the reaction will be zero is:
    • A. 

      373 K

    • B. 

      413 K

    • C. 

      463 K

    • D. 

      493 K

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