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The Values of and Are Shown for the Following

Question 132

Multiple Choice

The values of $The values of and are shown for the following equilibrium reaction.What makes the equilibrium constant larger at low temperature? 2 NO2(g) \leftrightarrows N2O4(g) \Delta H \circ = -58.02 kJ/mol, \Delta S \circ =-176.5 J/mol . K A) The negative value of \Delta H \circ is dominant at all temperatures. B) The negative value of \Delta S \circ is dominant at all temperatures. C) The negative value of \Delta S \circ is combined with the small value of T. D) The negative value of \Delta H \circ is combined with the small value of T.$ and $The values of and are shown for the following equilibrium reaction.What makes the equilibrium constant larger at low temperature? 2 NO2(g) \leftrightarrows N2O4(g) \Delta H \circ = -58.02 kJ/mol, \Delta S \circ =-176.5 J/mol . K A) The negative value of \Delta H \circ is dominant at all temperatures. B) The negative value of \Delta S \circ is dominant at all temperatures. C) The negative value of \Delta S \circ is combined with the small value of T. D) The negative value of \Delta H \circ is combined with the small value of T.$ are shown for the following equilibrium reaction.What makes the equilibrium constant larger at low temperature? 2 NO₂(g) $\leftrightarrows$ N₂O₄(g) $\Delta$ H^$\circ$= -58.02 kJ/mol, $\Delta$ S^$\circ$ =-176.5 J/mol . K

A) The negative value of $\Delta$ H^$\circ$ is dominant at all temperatures.
B) The negative value of $\Delta$ S^$\circ$ is dominant at all temperatures.
C) The negative value of $\Delta$ S^$\circ$ is combined with the small value of T.
D) The negative value of $\Delta$ H^$\circ$ is combined with the small value of T.