Consider the conversion of C to D via a one-step reaction. The activation energy of this reaction is 3 kcal/mol. The energy difference between D and the transition state of the reaction is 7 kcal/mol. What is the $\Delta H ^ { \circ }$ or the reaction?

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The Answer of Consider the conversion of C to D via a one-step reaction. The activation energy of this reaction is 3 kcal/mol. The energy difference between D and the transition state of the reaction is 7 kcal/mol. What is the $\Delta H ^ { \circ }$ or the reaction?

Consider the Conversion of C to D Via a One-Step ΔH∘\Delta H ^ { \circ }ΔH∘

Consider the Conversion of C to D Via a One-Step $\Delta H ^ { \circ }$