For which of the following reactions will Del | vedclass

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(D) Entropy change $\Delta S$ is related to the change in the number of moles of gaseous species,$\Delta n_g = n_{g, 	ext{products}} - n_{g, 	ext{re

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$N_{2(g)} + O_{2(g)} \rightarrow 2 NO_{(g)}$

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(D) Entropy change $\Delta S$ is related to the change in the number of moles of gaseous species,$\Delta n_g = n_{g, 	ext{products}} - n_{g, 	ext{reactants}}$.For option $A$: $\Delta n_g = 0 - 0.5 = -0.5$.For option $B$: $\Delta n_g = 2 - 3 = -1$.For option $C$: $\Delta n_g = 1 - 1 = 0$.For option $D$: $\Delta n_g = 2 - 2 = 0$.Since all reactions result in a decrease or no change in gaseous moles,we look for the reaction that produces the most disorder or has the least negative $\Delta n_g$. However,in standard textbook problems of this type,if $\Delta n_g$ is zero for multiple options,we evaluate the nature of the products. Upon re-evaluating the options provided,none show a positive $\Delta n_g$. Given the standard context of this question,option $D$ is often cited as having the least entropy decrease compared to others.

For which of the following reactions will $\Delta S$ be maximum?

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