For most reactions,the value of $\Delta$U is very close to that for $\Delta$H

Question

Quizplus · Accepted Answer

This statement is generally true. For most reactions, the difference in enthalpy (ΔH) and entropy (ΔS) between the reactants and products is much larger than the difference in free energy (ΔG). Therefore, the value of ΔG is often dominated by ΔH - TΔS, where T is the temperature in Kelvin. Since the TΔS term is relatively small compared to ΔH, the value of ΔG is typically very similar to ΔH at most temperatures. Therefore, for most reactions, the value of ΔG for the reaction in standard conditions (ΔG°) is very close to ΔH.

For Most Reactions,the Value Of Δ\DeltaΔ U Is Very Close to That For

For Most Reactions,the Value Of $\Delta$ U Is Very Close to That For