In a reaction between `H_(2)` and `I_(2)` at a certain temperature, the amounts of `H_(2), I_(2)` and HI at equilibrium were found to be `0.45` mol, `0.39` mol, and `3.0` mol respectively. Calculate the equilibrium constant for the reaction at the given temperature.

In a reaction between `H_(2)` and `I_(2)` at a certain temperature, th

1.	In a reaction between `H_(2)` and `I_(2)` at a certain temperature, the amounts of `H_(2), I_(2)` and HI at equilibrium were found to be `0.45` mol, `0.39` mol, and `3.0` mol respectively. Calculate the equilibrium constant for the reaction at the given temperature.
Answer» Correct Answer - A::B::C The reaction between `H_(2)` and `I_(2)` may be represented as `H_(2)+I_(2) hArr 2HI` Amounts of `H_(2), I_(2)`, and `HI` at equilibrium are given to be `H_(2)=0.45 "mol", I_(2)=0.39 "mol"` and `HI=3.0 "mol"` Suppose the volume of the vessel (i.e., reaction mixture) `=V L` Then, the molar concentration at equilibrium will be `[H_(2)]=0.45/V, [I_(2)]=0.39/V`, and `[HI]=3.0/V "mol" L^(-1)` Applying the law of chemical equilibrium to the above reaction `K_(c)=([HI]^(2))/([H_(2)][I_(2)])=((3.0//V^(2)))/((0.45//V)(0.39//V))` `=((3.0)^(2))/(0.45xx0.39)=51.28`

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In a reaction between `H_(2)` and `I_(2)` at a certain temperature, the amounts of `H_(2), I_(2)` and HI at equilibrium were found to be `0.45` mol, `0.39` mol, and `3.0` mol respectively. Calculate the equilibrium constant for the reaction at the given temperature.

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