The following reaction was performed in a sealed vessel at 774 ∘C : H2(g)+I2(g)⇌2HI(g) Initially, only H2 and I2 were present at concentrations of [H2]=3.30M and [I2]=2.15M. The equilibrium concentration of I2 is 0.0500 M . What is the equilibrium constant, Kc, for the reaction at this temperature?
H2(g) + I2(g) <---------------> 2HI(g)
3.30 M 2.15 M 0
3.30-x 2.15 - x 2x
equilibrium concentration I2 = 0.0500 M
2.15 - x = 0.0500
x = 2.10
[HI] = 2x = 4.20 M
[H2] = 1.20 M
Kc = [HI]^2 / [H2] [I2]
= (4.20)^2 / [1.20] [0.05]
Kc = 294
equilibrium constant, Kc = 294
The following reaction was performed in a sealed vessel at 774 ∘C : H2(g)+I2(g)⇌2HI(g) Initially, only...
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