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What is the usual definition of entropy? - Chemistry

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प्रश्न

What is the usual definition of entropy?

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उत्तर

  1. Entropy is a thermodynamic state function that is a measure of the randomness or disorderliness of the system.
  2. For a reversible change taking place at a constant temperature (T). the change in entropy
  3. The system is equal to heat energy absorbed or evolved (q) by the system divided by the constant temperature (T).
    `Δ"S"_"sys" = "q"_"rev"/"T"`
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Various Statements of the Second Law of Thermodynamics
  क्या इस प्रश्न या उत्तर में कोई त्रुटि है?
अध्याय 7: Thermodynamics - Evaluation [पृष्ठ २२४]

APPEARS IN

सामाचीर कलवी Chemistry - Volume 1 and 2 [English] Class 11 TN Board
अध्याय 7 Thermodynamics
Evaluation | Q II. 5. a. | पृष्ठ २२४

संबंधित प्रश्न

The correct thermodynamic conditions for the spontaneous reaction at all temperature is


What is the unit of entropy?


Identify the state and path functions out of the following:

  1. Enthalpy
  2. Entropy
  3. Heat
  4. Temperature
  5. Work
  6. Free energy

State the various statements of the second law of thermodynamics.


Calculate the entropy change in the system, and surroundings, and the total entropy change in the universe during a process in which 245 J of heat flows out of the system at 77°C to the surrounding at 33°C.


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 the expansion process.


You are given normal boiling points and standard enthalpies of vapourisation. Calculate the entropy of vapourisation of liquids listed below.

Liquid Boiling points (°C) ΔH (kJ mol−1)
Ethanol 78.4 + 42.4

You are given normal boiling points and standard enthalpies of vapourisation. Calculate the entropy of vapourisation of liquids listed below.

Liquid Boiling points (°C) ΔH (kJ mol−1)
Toluene 110.6 + 35.2

Cyanamide (NH2CN) is completely burnt in excess oxygen in a bomb calorimeter, ΔU was found to be −742.4 kJ mol−1, calculate the enthalpy change of the reaction at 298 K.\[\ce{NH2CN_{(s)} + 3/2 O2_{(g)} -> N2_{(g)} + CO2_{(g)} + H2O_{(l)}}\] ΔH = ?


For the reaction at 298 K: \[\ce{2A + B -> C}\]

ΔH = 400 KJ mol−1; ΔS = 0.2 KJ K−1 mol−1 Determine the temperature at which the reaction would be spontaneous.


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