In: Chemistry
Given the following equilibrium:
Br2 (g) + F2 (g) <----> 2 BrF (g)
Kc = 54.7 at 300 K
An evacuated flask is charged with 2.2 atm of Br2 and 2.2 atm of F2 at 300 K. Calculate the partial pressure of BrF at equilibrium at this temperature.
Br2 (g) + F2 (g) 2 BrF (g)
initial pressure 2.2 2.2 0
change -p -p +2p
Equb pressure 2.2-p 2.2-p 2p
Equilibrium constant , Kc = p2BrF(g) / ( pBr2(g) x p F2(g) )
54.7 = (2p)2 / [(2.2-p)(2.2-p)]
2p / (2.2-p) = 7.39
2p = 16.3 - 7.39p
9.39 p = 16.3
p = 1.73 atm
Therefore the equilibrium partial pressure of BrF = 2p = 2x1.73 = 3.46 atm