For independent process at 300 K . Process Δ H / kJmol - 1 Δ S / JK - 1 A - 25 - 80 B - 22 40 C 25 - 50 D 22 20 The number of non-spontaneous process from the following is _____ .

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The relation between change in Gibbs free energy, change in enthalpy and change in entropy can be written as follows,

$ΔG = ΔH - TΔS$

If $∆ G$ is $+ ve$ , then the process is said to be non-spontaneous and if $∆ G$ is $- ve$ then the process is said to be spontaneous.

$A : ΔG ({Jmol}^{- 1}) = - 25 \times 10^{3} + 80 \times 300 : - ve$

$B : ΔG ({Jmol}^{- 1}) = - 22 \times 10^{3} - 40 \times 300 : - ve$

$C : ΔG ({Jmol}^{- 1}) = 25 \times 10^{3} + 300 \times 50; + ve$

$D : ΔG ({Jmol}^{- 1}) = 22 \times 10^{3} - 20 \times 300 : + ve$

Processes $C$ and $D$ are non-spontaneous.

Process	$Δ H / {kJmol}^{- 1}$	$Δ S / {JK}^{- 1}$
$A$	$- 25$	$- 80$
$B$	$- 22$	$40$
$C$	$25$	$- 50$
$D$	$22$	$20$

Chemistry - Thermodynamics - II Question with Solution | TestHub

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