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
dG = dH-TdS
Substitute and solve for dG
Post your work if you get stuck.
To find the ∆G (change in Gibbs free energy) for the given reaction, you can use the equation:
∆G = ∆H - T∆S
where ∆H is the change in enthalpy, ∆S is the change in entropy, and T is the temperature in Kelvin.
In this case, you are given the values for ∆H and ∆S for the reaction. The enthalpy change (∆H) is 285.4 kJ, and the entropy change (∆S) is -137.14 J/K.
To use these values in the equation, you need to convert the entropy change to the same units as the enthalpy change. Since the enthalpy change is given in kJ and the entropy change is given in J/K, you need to divide the entropy change by 1000 to convert it to kJ:
∆S = -137.14 J/K ÷ 1000 = -0.13714 kJ/K
Now, you can substitute the values into the equation:
∆G = ∆H - T∆S
∆G = 285.4 kJ - T(-0.13714 kJ/K)
At this point, we don't have the temperature (T) provided in the given information, so it's not possible to calculate the precise value of ∆G.
However, if you were given the temperature, you could substitute it into the equation and calculate the ∆G. The resulting value of ∆G would determine the spontaneity of the reaction. If ∆G is negative, the reaction is spontaneous; if ∆G is positive, the reaction is non-spontaneous; and if ∆G is zero, the reaction is at equilibrium.
Since the temperature is not provided, we cannot determine the exact value of ∆G.