Question

What is the ∆G for the following reaction between O3 and O2?
3O2(g) 2O3(g)

Given:
O3: ∆H = 285.4 kJ ∆S = -137.14 J/K)
109.5 kJ
208.3 kJ
300.2 kJ
326.3 kJ

Answer 1

For Calculating the Value of the ΔG, we need to know about it.

ΔG is the Change in Gibbs Free Energy and is one of the famous Thermodynamic term.

Using the Formula,

ΔG = ΔH - TΔS

Now, It is given that,

ΔH =  = 285.4 kJ/mole.  = 285400 J/mole.  and ∆S = -137.14 J/Kmole.  

But for Change in Gibbs free Energy Temperature must be given. It is not there, then it can't be calcuated.

It must be there is the question, but you forget to write here.

Let me make the assumption about the temperature from the reaction.

Temperature is 27°C during this Reaction.

∴ T = 273 + 27 = 300 K.

∴ ΔG =  285400 - 300 × -137.14

∴ ΔG = 285400 - 41142

∴ ΔG = 326542 J/Kmole.

∴ ΔG= 326.542 kJ/Kmole.

Hence, Option (d). is the correct answer.

Hope it helps.