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Thermodynamics Model Question Paper

11th Standard

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Chemistry

Time : 01:00:00 Hrs
Total Marks : 50
    10 x 1 = 10
  1. All the naturally occurring processes proceed spontaneously in a direction which leads to _______________

    (a)

    decrease in entropy

    (b)

    increase in enthalpy

    (c)

    increase in free energy

    (d)

    decrease in free energy

  2. Heat of combustion is always ____________

    (a)

    positive

    (b)

    negative

    (c)

    zero

    (d)

    either positive or negative

  3. Change in internal energy, when 4 kJ of work is done on the system and 1 kJ of heat is given out by the system is ______________

    (a)

    +1 kJ

    (b)

    - 5 kJ

    (c)

    +3 kJ

    (d)

    - 3 kJ

  4. The bond dissociation energy of methane and ethane are 360 kJ mol-1 and 620 kJ mol-1 respectively. Then, the bond dissociation energy of C-C bond is ______________.

    (a)

    170 kJ mol-1

    (b)

    50 kJ mol-1

    (c)

    80 kJ mol-1

    (d)

    220 kJ mol-1

  5. Which among the following is not an extensive property?

    (a)

    Volume

    (b)

    internal energy

    (c)

    Mass

    (d)

    temperature

  6. Which among the following is not a state function?

    (a)

    Pressure

    (b)

    Volume

    (c)

    Temperature

    (d)

    Work

  7. Which among the following is a state function?

    (a)

    Pressure

    (b)

    Enthalpy

    (c)

    Heat

    (d)

    Both (a) and (b)

  8. In a compression process, Pext is ___________

    (a)

    (Pint+ dP)

    (b)

    (Pint- dP)

    (c)

    (dP-Pint)

    (d)

    (-Pint+dP)

  9. ΔHo of H2O(1) is KJ/mol.

    (a)

    -74.85

    (b)

    -242

    (c)

    +242

    (d)

    +74.85

  10. Heat absorbed at constant volume is measured in ____________ calorimeter.

    (a)

    Coffee cup

    (b)

    Differential scanning

    (c)

    Bomb

    (d)

    Adiabatic

  11. 5 x 2 = 10
  12. State the first law of thermodynamics.

  13. Define Gibb's free energy.

  14. Identify the state and path function out of the following:
    a) Enthalpy
    b) Entropy
    c) Heat
    d) Temperature
    e) Work
    f) Free energy.

  15. Give examples for extensive and intensive properties.

  16. Explain Zeroth law of thermodynamics.

  17. 5 x 3 = 15
  18. What are state and path functions? Give two examples

  19. In a constant volume calorimeter:3.5g of a gas with molecular weight 28 was burnt in excess oxygen at 298 K. The temperature of the calorimeter was found to increase from 298 K to 298.45 K due to the combustion process. Given that the calorimeter constant is 2.5 kJ K-1. Calculate the enthalpy of combustion of the gas in kJ mol-1

  20. For a reaction, 2Cl(g) ⟶ Cl2, What are the signs of ΔH and ΔS?

  21. In the equation N2(g)+ 3H2(g) ⇌2NH3(g) What would be the sign of work done?

  22. Which law of thermodynamics deals with equivalence of different forms of energies?

  23. 2 x 5 = 10
  24. List the characteristics of internal energy.

  25. For the equilibrium \({ PCl }_{ 5 }\rightleftharpoons { PCl }_{ 3(g) }+{ Cl }_{ 2(g) }\) at 298 K, K is 1.8 x 10-7. What is the ΔG0 for the reaction?

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