Question

Use the reaction l2(s) = 12(9), AH = 62.4 kJ/mol, AS = 0.145 kJ/(mol-K), for

this question
At what temperature is the reaction at equilibrium?
A. 157 K
B. 62 K
C. 0.002 K
D. 430 K

Answer 1

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

Answer 2

Answer: D. 430 K

Step-by-step explanation:

Using Gibbs Helmholtz equation:

`\Delta G=\Delta H-T\Delta S`

`\Delta G` = Gibbs free energy

`\Delta H` = enthalpy change = 62.4 kJ/mol

`\Delta S = entropy change  = 0.145 kJ/mol K</p><p>T = temperature in Kelvin</p><p>[tex]\Delta G` = +ve, reaction is non spontaneous

`\Delta G`= -ve, reaction is spontaneous

`\Delta G`= 0, reaction is in equilibrium

At equilibrium :
`T\Delta S=\Delta H`

`T=(\Delta H)/(\Delta S)`

`T=(62.4)/(0.145)`

`T=430K`

Thus at 430 K , the reaction is at equilibrium.