Question

Phosphorous pentafluoride (PF5) gas decomposes into phosphorous (P4) gas and fluorine (F2) gas at a certain temperature. Determine the equilibrium constant for this reaction at this temperature if the measured equilibrium concentrations ([ ](eq)) are: [PF5](eq) = 0.0198 M, [P4](eg) = 0.317 M, [F2](eq) = 0.744 M. Hint: You should write a balanced chemical equation for the reaction described. 11.9 1.07 x 105 8.41 x 10-2 1.85 x 10-7 2.37 x 107

Answer 1

PESCg) decomposes into Pe and Fz at Certain temprature, We have to determine Kalequilibrium Constant) for this Reaction. We have equilibrium concentrations are given PeJey = = 0.312 m = 0.01g8M [PF5Den [1] eq=0 4PF5 (8) -0.744m Pa CO2 + 10F268) Now we see how to write kcceruilibrium constant) att bb cct do Kc = [c]*[n]d [A]a[B]b Now for given reaction, 4PF5 (6) Paco) + 10F268) Kc = [Puder [F] [PEDRO Kc (-317) X (0:744) 1-07X165 0.019814 Kc=10x15 - Equilibrium constant option Correct 2 -