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

Explanation:

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:

where,

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)

more infor would

a lot