The correct conclusion about the process is that "DeltaG" is negative and the product of temperature and "DeltaS" is greater than "DeltaH". That is option C
Spontaneous reaction are natural reactions that occurs without depending on energy from external sources.
A typical example of a spontaneous reaction is the rusting of iron.
To know if a reaction is spontaneous, second law of thermodynamics is used through Gibbs free energy.
At standard conditions ( constant temperature and pressure), Gibbs free energy(G) is equal to enthalpy change(ΔH) minus product of temperature(T) and the entropy change (ΔS) of the system.
That is, ΔG =ΔH −TΔS,
Entropy (S) is a measure of the degree of disorderliness of a system.
Enthalpy (H) is the heat of the reaction which is positive when heat is given out or negative when heat is absorbed.
From the formula, when ∆G is less than 0, the reaction is said to be spontaneous.
For ∆G to be less than 0, this means ∆H(DeltaH) is less than 0 and T∆ S( product of temperature and "DeltaS") is greater than 0 to achieve a negative value for ∆G(DeltaG)
Therefore, DeltaG" is negative and the product of temperature and "DeltaS" is greater than "DeltaH".
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