Which of the following statements is true? A) This reaction will be spontaneous only at high temperatures. B) This reaction will be spontaneous at all temperatures. C) This reaction will be nonspontaneous at all temperatures. D) This reaction will be nonspontaneous only at high temperatures. E) It is not possible to determine without more information, 8. (2) Identify the compound with the standard free energy of formation equal to zero. A) KCI (S) B) HF (g) C) NO (g) D) Al (s) E) It is hard to determine.

D) This reaction will be nonspontaneous only at high temperatures.

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 ΔG, determines whether the reaction is Spontaneous or non Spontaneous or at equilibrium,

i. e.,

if

ΔG <0, the reaction is SpontaneousΔG> 0, the reaction is non Spontaneous ΔG = 0, the reaction is at equilibrium

The reaction has the value for ∆H = negative, and ∆S = negative,

Now,

∆G = ∆H - T∆S

= ( - ∆H) - T ( - ∆S)

= ( - ∆H) + T (∆S)

Now, for making the reaction Spontaneous ΔG = negative,

Hence,

The temperature is low, then the value for ΔG will be negative, i. e., Spontaneous reaction.

And, vice versa, at higher temperature, the reaction will have ΔG positive, and the reaction will be non - Spontaneous reaction.

The standard free energy of formation will be zero, only for the compounds that are in their pure form,

Hence, Al (s) will have ΔG = 0.