The following reaction was performed in a sealed vessel at 791 ∘C : H2(g)+I2(g)⇌2HI(g) Initially, only...
The following reaction was performed in a sealed vessel at 791 ∘C :
H2(g)+I2(g)⇌2HI(g)
Initially, only H2 and I2 were present at concentrations of [H2]=4.00M and [I2]=2.40M . The equilibrium concentration of I2 is 0.0500 M . What is the equilibrium constant, Kc, for the reaction at this temperature?
Express your answer numerically.
Homework Answers
ICE Table:
Given at equilibrium,
[HI] = 0.05
+2x = 0.05
x = 0.025
Equilibrium constant expression is
Kc = [HI]^2/[H2][I2]
Kc = (+2x)^2/(4.0-1x)(2.4-1x)
Kc = (+2*0.025)^2/(4.0-1*0.025)(2.4-1*0.025)
Kc = 2.65*10^-4
Answer: 2.65*10^-4
Add Answer to:
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