First slide

Fundamentals of thermodynamics

Question

For which of the processes is $∆ S$ negative

Moderate

A

$H_{2} (g) \to 2 H (g)$
B

$N_{2} (g) 1 atm \to N_{2} (g) 8 atm$
C

$2 {SO}_{3} (g) \to 2 {SO}_{2} (g) + O_{2} (g)$
D

$C_{(dicmend)} \to C_{(qraphite)}$

Solution

The thermodynamic quantity of the system, the decrease in whose value during a process is equal to useful work done by the system $i, e ., ΔG = ΔH - TΔS,$ $H =$ enthalpy $S =$ entropy and $T =$ absolute temperature.
If an endothermic reaction occurs spontaneously i.e $ΔH = + ve$ then for reaction to be spontaneous $∆ G$ should be negative that is only possible when $ΔS > 0$ at constant temperature and pressure.

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