Answer: D. 430 K
Explanation:
Using Gibbs Helmholtz equation:
[tex]\Delta G=\Delta H-T\Delta S[/tex]
[tex]\Delta G[/tex] = Gibbs free energy
[tex]\Delta H[/tex] = enthalpy change = 62.4 kJ/mol
[tex]\Delta S = entropy change = 0.145 kJ/mol K
T = temperature in Kelvin
[tex]\Delta G[/tex] = +ve, reaction is non spontaneous
[tex]\Delta G[/tex]= -ve, reaction is spontaneous
[tex]\Delta G[/tex]= 0, reaction is in equilibrium
At equilibrium : [tex]T\Delta S=\Delta H[/tex]
[tex]T=\frac{\Delta H}{\Delta S}[/tex]
[tex]T=\frac{62.4}{0.145}[/tex]
[tex]T=430K[/tex]
Thus at 430 K , the reaction is at equilibrium.
Use the reaction I2(s) ⇌ l2(g), ΔH = 62.4 kJ/mol, ΔS+ 0.145 kJ/(mol⋅K), for this question. At what temperature is the reaction at equilibrium?
430 K
