Thermodynamics Book Back Questions

11th Standard

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Chemistry

Time : 00:45:00 Hrs
Total Marks : 30
    5 x 1 = 5
  1. The amount of heat exchanged with surrounding at constant temperature pressure is given by the quantity

    (a)

    ΔE

    (b)

    ΔH

    (c)

    ΔS

    (d)

    ΔG

  2. In an adiabatic process, which of the following is true?

    (a)

    q = w

    (b)

    q = 0

    (c)

    ΔE = q

    (d)

    PΔV= 0

  3. An ideal gas expands from the volume of 1 x 10-3 m3 to 1 x 10-2 m3 at 300 K against a constant pressure at 1 x 105 Nm-2. The work done is

    (a)

    - 900 J

    (b)

    900 kJ

    (c)

    270 kJ

    (d)

    -900 kJ

  4. The heat of formation of CO and CO2 are - 26.4 kcal and - 94 kcal, respectively. Heat of combustion of carbon monoxide will be

    (a)

    + 26.4 kcal

    (b)

    - 67.6 kcal

    (c)

    - 120.6 kcal

    (d)

    + 52.8 kcal

  5. The enthalpies of formation of Al2O3 and Cr2Oare -1596 kJ and -1134 kJ, respectively. ΔH for the reaction 2AI + Cr2O3 ⟶ 2Cr + Al2O3 is

    (a)

    - 1365 kJ

    (b)

    2730 kJ

    (c)

    - 2730 kJ

    (d)

    - 462 kJ

  6. 3 x 2 = 6
  7. State the first law of thermodynamics.

  8. Define Gibb's free energy.

  9. What is lattice energy?

  10. 3 x 3 = 9
  11. 1 mole of an ideal gas, maintained at 4.1 atm and at a certain temperature, absorbs heat 3710 J and expands to 2 litres. Calculate the entropy change in expansion process.

  12. The standard enthalpies of formation of SO2 and SO3 are -297 kJ mol-1 and -396 kJ mol-1 respectively. Calculate the standard enthalpy of reaction for the reaction: SO2 + \(\frac{1}{2}\)O2⟶SO3

  13. For the reaction at 298 K: 2A +B ⟶ C.  ΔH = 400 J mol-1; ΔS = 0.2 JK-1 mol-1 Determine the temperature at which the reaction would be spontaneous.

  14. 2 x 5 = 10
  15. Explain how heat absorbed at constant volume is measured using bomb calorimeter with a neat diagram.

  16. List the characteristics of Gibbs free energy

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