Respuesta :
Answer:
b. ΔS° > 0, ΔH° < 0
Explanation:
According the equation of Gibb's free energy -
∆°G = ∆°H -T∆°S
∆°G = is the change in gibb's free energy
∆°H = is the change in enthalpy
T = temperature
∆°S = is the change in entropy .
And , the sign of the Δ°G , determines whether the reaction is Spontaneous or non - Spontaneous or at equilibrium ,
i.e. ,
if
- Δ°G < 0 , the reaction is Spontaneous
- Δ°G > 0 , the reaction is non - Spontaneous
- Δ°G = 0 , the reaction is at equilibrium
The reaction has the value for ∆°H < 0 i.e. negative, and ∆°S > 0 i.e. , positive
Now ,
∆°G = ∆°H -T∆°S
= ( - ∆°H ) - T( + ∆°S )
= ( - ∆°H ) - T( ∆°S )
∆°G = negative
Hence ,
Δ°G < 0 , the reaction is Spontaneous .
When Gibb's free energy is negative then the reaction will be spontaneous, ΔS° > 0, ΔH° < 0 will give Δ°G < 0.
What is Gibb's free energy?
Gibb's free energy is used to determine the amount of work that can be done by a system.
(Gibb's free energy) ∆°G = ∆°H -T∆°S
∆°H = is the change in enthalpy
T = temperature
∆°S = is the change in entropy .
Gibb's free energy is given as Δ°G and it also be used to determine if a chemical reaction is spontaneous.
- Δ°G < 0 , the reaction is Spontaneous
- Δ°G > 0 , the reaction is non - Spontaneous
- Δ°G = 0 , the reaction is at equilibrium
Therefore, ΔS° > 0, ΔH° < 0 will give Δ°G < 0
∆°G = ∆°H -T∆°S
= ( - ∆°H ) - T( + ∆°S )
= ( - ∆°H ) - T( ∆°S )
∆°G = negative
Learn more on Gibb's free energy here,
https://brainly.com/question/10012881
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