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.

samuel de champlain. in 1608, king henry iv sponsored pierre dugua, sieur de mons and samuel de champlain as founders of the city of quebec with 28 men. this was the second permanent french settlement in the colony of canada.

m=9

step-by-step explanation: