For the reaction , `H_2+I_2hArr2HI`, K=47.6. If the initial number of moles of each reactant and product is 1mol then at equilibrium

Options

A. `[I_2]=[H_2],[I_2]gt[HI]`
B. `[I_2]=[H_2],[I_2]lt[HI]`
C. `[I_2]=[H_2],[I_2]=[HI]`
D. `[I_2]gt[H_2],[I_2]=[HI]`

Explanation

For the given reaction, `K=([HI]^2)/([H_2][I_2])`
A 1mol of `H_2` reacts with 1 mole of `I_2`, even at equilibrium `[H_2]=[I_2]`
Hence, `K=([HI]^2)/([I_2]^2)` or `sqrtK=([HI])/([I_2])=sqrt(47.6)`
i.e, `[HI]>[I_2]`