The Equilibrium Constants for the Chemical Reaction N₂(g)+ O₂(g) $\Delta$ Hº < 0
B)The Partial Pressure of NO(g)is Less at 2,200 K

The equilibrium constants for the chemical reaction N₂(g) + O₂(g) 2NO(g) are K_P = 1.1 * 10^-3 and 3.6 *10^-3 at 2,200 K and 2,500 K, respectively. Which one of these statements is true?

A) The reaction is exothermic, $\Delta$ Hº < 0.
B) The partial pressure of NO(g) is less at 2,200 K than at 2,500 K.
C) K_P is less than K_c by a factor of (RT) .
D) The total pressure at 2,200 K is the same as at 2,500 K.
E) Higher total pressure shifts the equilibrium to the left.