A mixture containing an initial concentration of 0.1614 M for H2 and 0.1440 M for I2 is allowed to come to equilibrium (see reaction below). What must be the equilibrium concentration of HI?
H2(g) + I2(g) ↔ 2HI(g) Kc = 48.7000 |
H2(g) + I2(g) 2HI (g)
initial concentration 0.1614 0.1440 0
equillibrium concentration 0.1614 - x 0.1440 -x 2x
Kc = [ 2HI ]2 / [ H2] [I2]
48.7 = [2x]2 / [ 0.1614 - x ] [0.1440 -x ] = 4x2 / 0.02324 - 0.1614x - 0.1440x - x2
48.7 = 4x2 / 0.02324 -0.3054 -x2
48.7 ( 0.02324 -0.3054 -x2 ) = 4x2
1.1317 - 14.87x - 48.7x2 = 4x2
52.7x2 + 14.87x - 1.1317 = 0 ( using the quadratic equation we solve it )
x = -b +_ ( b2 - 4*a*c) /2a
= - 14.87 +_ ( 14.872 - 4*52.7*-1.1317) / 2 * 52.7
= - 14.87 +_ ( 221.12 + 238.56 ) / 105.4
= - 14.87 +_ 459.68 / 105.4
= - 14.87 + 21.44 /105.4
= 6.57 / 105.4 = 0.062 = x
[HI] = 2x = 0.062 * 2 = 0.124 at equillibrium
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