The statement that said about a reaction with ΔH and ΔS is "It is never spontaneous."
The change in enthalpy (ΔH) is a measure of a system's energy. This is essentially the heat exchanged between a system and its environment under constant P. The change in entropy, indicated as ΔS, is a measurement of a system's irregularity or disorder.
A spontaneous reaction is a reaction that occurs naturally under defined conditions and promotes the creation of products.
A spontaneous reaction may result in a rise or drop in enthalpy, entropy, or both, but it will always result in a decrease in free energy, which is a negative ΔG.
The spontaneity equation is
ΔG = ΔH - TΔS
When ΔG is positive, the reaction proceeds in the other direction, with reactants creating products.
To put it another way, a spontaneous reaction is one that releases free energy, hence ΔG must have a negative sign.
As a result of the given reaction, because ΔH is positive and ΔS is negative, sign of ΔG will always remains to be positive, and the response will never be spontaneous. Both driving factors are working against product creation in this case.
Hence the correct option is D.
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