equilibrium constant and partial pressures?

Question

The reaction below was studied at a high temperature. At equilibrium, the partial pressures of the gases are as follows:
PCl5 = 1.4 x 10-4 atm, PCl3 = 2.4 x 10-2 atm, Cl2 = 3.0 x 10-1 atm.

What is the value of KP for the reaction?

PCl5(g) = PCl3(g) + Cl2(g)

Answer 1

Kp = P(PCl3) * P(Cl2) / P(PCl5) = 2.4 x 10^-2 * 0.3 / 1.4 x 10^-4
Kp = 51.4

Answer 2

you should redecorate all this equilibrium constants into equation H3PO4 -> H+ + H2PO4- K1 = 6.9 x 10-3 mol/L equation a million H+ + PO43- -> HPO42- K2 = 2.a million x 1012 mol/L equation 2 H2PO4- -> HPO42- + H+ K3 = 6.2 x 10-8 mol/L equation 3 and if i'm good, K1 = [H+][H2PO4-] / [H3PO4 ] , an analogous for the others then you truly truly definately may pick to rewrite the proper with the three first : H3PO4 + 3 H2O -> 3H3O+ + PO43- equation 4 eq. 4 = a million - 2 + 3 You write the perfect constants for this very very last equation, and then you seem with the a million, 2 and three. it isn't complicated, yet you should attentive with all this equations.