Calculating Equilibrium Constants The following reaction was performed in a sealed vessel at 752 âˆ˜C : H2(g)+I2(g)â‡Œ2HI(g) Initially, only...

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Chemistry

Calculating Equilibrium Constants
The following reaction was performed in a sealed vessel at 752âˆ˜C :
H2(g)+I2(g)â‡Œ2HI(g)
Initially, only H2 and I2 were present at concentrations of[H2]=3.75M and [I2]=3.00M. The equilibrium concentration of I2 is0.0900 M . What is the equilibrium constant, Kc, for the reactionat this temperature?

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3.7 Ratings (641 Votes)

Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â H2(g) +Â Â Â I2(g)Â Â â‡ŒÂ Â Â Â Â 2HI(g)

InitialÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â 3.75 MÂ Â Â 3.00 MÂ Â Â Â Â Â Â Â Â Â Â Â 0

at equilibriumÂ Â Â Â Â Â 3.75- xÂ Â Â Â 3-xÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â 2 x

So,

Â Â Â equilibrium concentration of I2 = 3-x

But given that equilibrium concentration of I2 = 0.0900 M

Â Â Â Then,

Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â 3-x = 0.09

Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â x = 2.91 M

Â Â Â Therefore, equilibrium concentrations are

Â Â [H2] = 3-75 -x = 3.75 - 2.91 = 0.84 M

[I2] = 0.09 M

[HI]= 2 x= 2 x 2.91 = 5.82 M

Â Â Â Â Â Â Â Â Kc = [HI]²/ [H2] [I2]

Â Â Â Â Â Â Â Â Â Â Â Â Â Â = (5.82)² / (0.84) (0.09)

Â Â Â Â Â Â Â Â Â Â Â Â Â = 448.05

Therefore, equilibrium constantÂ Â Kc = 448.05

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Calculating Equilibrium Constants The following reaction was performed in a sealed vessel at 752 âˆ˜C : H2(g)+I2(g)â‡Œ2HI(g) Initially, only...

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Chemistry

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