Chemistry - Thermodynamics - I Question with Solution | TestHub

ChemistryThermodynamics - IIsothermal Process/Isobaric/IsochoricMedium2 minQB

ChemistryMediumnumerical

Passage / Comprehension

Two mole of an ideal gas is expanded irreversiubly & isothermally at $2 7^{\circ} C$ untill its volume is doubled and 3.3 kJ heat is absorbed from surrounding. (R. ln $2 = 5.76 J / k mol$ )

Determine $Δ S_{system}$ (in $JK^{- 1}$ ).

Answer:

11.52

Solution:

For an ideal gas, entropy change depends only on the initial and final states.

$Δ S_{sys} = n R ln (\frac{V _{2}}{V _{1}}) = 2 \times 5.76 = 11.52 J K^{- 1}$

The given heat absorbed, $q = 3.3 k J$ , is not required for calculating $Δ S_{sys}$ because entropy is a state function.

$Δ S_{sys t e m} = 11.52 J K^{- 1}$

Answer: $11.52 J K^{- 1}$

Stream:JEESubject:ChemistryTopic:Thermodynamics - ISubtopic:Isothermal Process/Isobaric/Isochoric

⏱ 2mℹ️ Source: QB

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