The equation represents the decomposition of a generic diatomic
element in its standard state.
1/2X₂(g)⟶X(g)
Assume that the standard molar Gibbs energy of formation of x(g) is 5.80kJ.mol⁻¹ at 2000 and −62.48 kJ.mol⁻¹ at 3 Determine the value of K (the thermodynamic equilibrium constant) at each temperature. K at 2000.K=
K at 3000.K=
Assuming that ΔH*ᵣₓₙ is independent of temperature, determine the value of ΔH*ᵣₓₙ
​from this data. ΔH*ᵣₓₙ= kJmol⁻1