Gaseous chemical equilibrium question?
I2 (g) + Br2 (g) <--> 2IBr (g)
A sealed 5.00 Liter container initially contains 0.0150 moles of each of iodine and bromine at 150 degrees Celcius. Calculate the equilibrium partial pressures of the gases if teh equilibrium constant for this system at 150 degrees Celcius is 1.20 x 10^2.
Can anyone help? I'm a little confused. Thanks
Answer:
I2 (g) + Br2 (g) <----> 2IBr
initial concentration
0.0150/5=
0.003. . . 0.003
at equilibrium
0.003-x 0.003-x . . . . .2x
1.20 x 10^2 =( 2x )^2/ ( 0.003-x)^2
square root =
10.95 = 2x / 0.003 -x
0.0328 - 10.95x = 2x
12.95 x = 0.0328
x = 0.00253 M
[ I2 ] = [ Br2] =0.003 - 0.00253 = 0.00047 M
[ IBr] = 2 x 0.00253 = 0.00506 M
pV = nRT
T = 150 + 273 = 423 K
p = nRT / V = n/V x RT ( n/V is the molar concentration )
p ( I2 ) = p ( Br2 ) = 0.00047 x 0.0821 x 423 = 0.0163 atm
p ( IBr ) = 0.00506 x 0.0821 x 423 = 0.176 atm
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