Question

Use the reaction I2(s) I2(g), H = 62.4 kJ/mol, S = 0.145 kJ/(molK)

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

Answer 1

430 K

Step-by-step explanation:

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Answer 2

Answer: B. 430 K

Step-by-step explanation:

According to Gibb's 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/molK

T = temperature in Kelvin

`\Delta G` = +ve, reaction is non spontaneous

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

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

`\Delta H-T\Delta S=0` for reaction to be spontaneous

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

`T=(62.4kJ/mol)/(0.145kJ/molK)=430K`

Thus the Reaction is spontaneous when temperature is 430 K.