For which of the following reactions will the reactant experience the largest degree of decomposition
upon reaching equilibrium at 500 k?
a) 2no2f(> 2no2(g) + f2(g); kp = 6.6 10-22
b) 2so3(> 2so2(g) + o2(g); kp = 1.3 10-5
c) 2nof(> 2no(g) + f2(g); kp = 1.2 10-26
d) 2nocl(> 2no(g) + cl2(g); kp = 1.7 10-2
e) 2no2(> 2no(g) + o2(g); kp = 5.9 10-5

D) 2 NOCl(g) ⇄ 2 NO(g) + Cl₂(g); Kp = 1.7 × 10⁻²

Explanation:

In order to compare the degree of decomposition of these reactions, we have to compare the equilibrium constant Kp. Kp is equal to the partial pressure of the products raised to their stoichiometric coefficients divided by the partial pressure of the reactants raised to their stoichiometric coefficients. The higher the Kp, the more products and fewer reactants at equilibrium. Among these reactions, D is the one that has the highest Kp, therefore the one experiencing the largest degree of decomposition.

i would say b

explanation:

but i think i would need more information than that