Chemistry - Thermodynamics - II Question with Solution | TestHub

ChemistryThermodynamics - IIAdiabatic Process/PolytropicMedium2 minPYQ_2020

ChemistryMediumsingle choice

For a given reaction, $Δ H = 35 . 5 kJmo l^{- 1}$ and $Δ S = 83 . 6 J k^{- 1} mo l^{- 1}$ . The reaction is spontaneous at
(Assume that $Δ H$ and $Δ S$ do not vary with tempearature)

Options:

Answer:

Solution:

As Both $Δ H$ and $Δ S$ are positive so to keep $Δ G = - ve$ High Temp is favourable so that process become spontaneous.
$Δ G = Δ H - T . Δ S$
$T = \frac{Δ H}{Δ S} = \frac{35.5 \times 1000}{83.6} > 424.6 K$
$T > 425K$

Stream:NTA_ABHYASSubject:ChemistryTopic:Thermodynamics - IISubtopic:Adiabatic Process/Polytropic

⏱ 2mℹ️ Source: PYQ_2020

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