For a particular reaction delta G is more negative than delta H. This means that
a. delta S is zero.
b. deltaS is negative
c. delta S is positive
d. delta S is negative if delta H is positive.
e. delta S is negative if delta H is negative.
i thought it was c?
c should be right.
To determine the correct answer, we need to understand the relationship between ΔG (Gibbs free energy change), ΔH (enthalpy change), and ΔS (entropy change) for a reaction.
The relationship is given by the equation:
ΔG = ΔH - TΔS
where ΔG represents the change in Gibbs free energy, ΔH represents the change in enthalpy, ΔS represents the change in entropy, and T represents the temperature in Kelvin.
If ΔG is more negative than ΔH, it means that the term TΔS is positive and larger in magnitude than ΔH.
Now, considering the options:
a. ΔS is zero: This option cannot be correct because if ΔG is more negative than ΔH, it indicates that ΔS is not zero.
b. ΔS is negative: This option cannot be correct either because if ΔG is more negative than ΔH, it implies that TΔS is positive and larger in magnitude than ΔH, indicating that ΔS must be positive.
c. ΔS is positive: This option turns out to be the correct answer based on the previous explanation.
d. ΔS is negative if ΔH is positive: This statement is not valid because ΔG being more negative than ΔH does not necessarily mean that ΔS is negative.
e. ΔS is negative if ΔH is negative: This statement is also incorrect because ΔG being more negative than ΔH does not imply that ΔS is negative, but rather positive.
Therefore, the correct answer is option c. ΔS is positive.