The following reaction was performed in a sealed vessel at 797 ∘C : H2(g)+I2(g)⇌2HI(g) Initially, only...
The following reaction was performed in a sealed vessel at 797 ∘C :
H2(g)+I2(g)⇌2HI(g)
Initially, only H2 and I2 were present at concentrations of [H2]=3.15M and [I2]=2.50M. The equilibrium concentration of I2 is 0.0900 M . What is the equilibrium constant, Kc, for the reaction at this temperature?
Homework Answers
Ans.
Initial concentration of H2 = 3.15M
Initial concentration of I2 = 2.50M
The given equilibrium is
The ICE table for the reaction is
| [H2] | [I2] | [HI] | |
| I | 3.15M | 2.50M | 0 |
| C | -x | -x | +2x |
| E | 3.15-x | 2.50-x | 2x |
The equilibrium concentration of I2 is 0.0900M
Therefore,
Since the value of 'x' is already known, you can also calculate the equilibrium concentration of H2 and HI
The expression for Kc is
Therefore, the equilibrium Kc at the given temperature is 349
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The following reaction was performed in a sealed vessel at 797
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