Can $\Delta$ S = 0 ?

Given are the Gibbs-Helmholtz equation: $\Delta G = \Delta H - T \cdot \Delta S$ and any possible chemical reactions you come up with.

$\Delta S = S(Product) - S(Educt)$

$0 = S(Product) - S(Educt)$

$S(Educt) = S(Product)$

Remember, we are in Chemistry, which means that there must be a chemical reaction with this property or it must be in fact impossible for $\Delta S$ to equal 0.

I think it is impossible, because the educt must be the same as the product in order to get the same entropy and this wouldn't be considered a chemical reaction anymore.

It would be nice if you could prove me or disprove me. Anyway looking forward to see your comments on this.

#Chemistry

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Comments

It's not always about reactions when you think on a big scale. Think about thermodynamics. If an ideal gas is expanded reversibly and adiabatically or if it undergoes a cyclic process then $\Delta S = 0$ for the isolated system.

Tapas Mazumdar - 3 years, 1 month ago

However, perfectly isolated systems cannot be found in nature, they are a mathematical model. Entropy always increases in general - if it does decrease somewhere, then it is only because somewhere else it has increased.

Alexandra Sidorovich - 1 year, 11 months ago

Math	Appears as
Remember to wrap math in `\(` ... `\)` or `\[` ... `\]` to ensure proper formatting.
`2 \times 3`	$2 \times 3$
`2^{34}`	$2^{34}$
`a_{i-1}`	$a_{i-1}$
`\frac{2}{3}`	$\frac{2}{3}$
`\sqrt{2}`	$\sqrt{2}$
`\sum_{i=1}^3`	$\sum_{i=1}^3$
`\sin \theta`	$\sin \theta$
`\boxed{123}`	$\boxed{123}$

Can Δ\DeltaΔS = 0 ?

Comments

Can $\Delta$ S = 0 ?