28 gm n2 and 6 gm h2 are mixed in 1 lit container .Eqm mixture reacts completely with 500cc 1m h2so4 solution .Calculate kc
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initial number of mole of
H2 = 6/2 = 3 moles
N2 = 28/28 = 1 moles
initial number of moles: 1 3 0
N2 + 3H2 ⇔ 2NH3
at equilibrium number of moles: 1-x 3-3x 2x
at equilibrium number of mole of NH3 = 27.54/17 = 1.62
2x = 1.62
x = 0.81
at equilibrium number of mole of N2 = 1 - 0.81 = 0.19
at equilibrium number of mole of H2 = 3(1 - 0.81) = 0.57
equilibrium concentration of
N2 = 0.19/1 = 0.19M
H2 = 0.57/1 = 0.57M
NH3 = 1.62/1 = 1.62M
equilibrium constant Kc = [NH3]² / {[N2]*[H2]³}
Kc = 1.62² / (0.19*0.57³)
Kc = 2.6244 / 0.0352
Kc ≈ 74.6
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