The Values Of $\Delta$ H°_rxn And $\Delta$ S°_rxn Are Shown for the Following Equilibrium Reaction

question 61

Multiple Choice

The values of $\Delta$ H°_rxn and $\Delta$ S°_rxn are shown for the following equilibrium reaction. What makes the equilibrium constant larger at low temperature?
2NO₂(g) $\leftrightarrows$ N₂O₄(g) $\Delta$ H $\degree$ = -58.02 kJ/mol, $\Delta$ S°=-176.5 J/mol .K

• A) The negative value of\(\Delta\)H \(\degree\)is dominant at all temperatures.
• B) The negative value of \(\Delta\)S° is dominant at all temperatures.
• C) The negative value of \(\Delta\)S° is combined with the small value of T.
• D) The negative value of \(\Delta\)0H \(\degree\) is combined with the small value of T.

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