The decomposition of a generic diatomic element in its standard state is represented by the equation 12x2(g)⟶x(g) assume that the standard molar gibbs energy of formation of x(g) is 4.84 kj·mol−1 at 2000 . k and −61.53 kj·mol−1 at 3000 . k. determine the value of the thermodynamic equilibrium constant, k , at each temperature. at 2000 . k, δ=4.84 kj·mol−1 . what is k at that temperature?
At 2000 K. K: 0.747
At 3000 K. K: 11.79
Let's consider the decomposition of a generic diatomic element in its standard state.
1/2 X₂(g) ⟶ X(g)
The relation between the equilibrium constant (K) and the standard Gibbs energy (ΔG°) is:
R is the ideal gas constant (8.314 × 10⁻³ kJ/mol.K)
T is the absolute temperature
At 2000 K (ΔG° = 4.84 kJ·mol⁻¹)
At 3000 K (ΔG° = −61.53 kJ·mol⁻¹)