For the reaction, `H _(2 (g)) + I _(2 (g)) hArr 2 HI _((g)) K = 47.6,` if the initial number of moles of each reactant and product is 1 mole, then at equilibrium:

Options

A. `[I_(2)] = [H_(2)], [I_(2)] gt [HI]`
B. `[I_(2)] lt [H_(2)] , [I_(2)] = [HI]`
C. `[I_(2)] = [H_(2)], [I_(2)] lt [HI]`
D. `[I_(2)] gt [H_(2)] , [I_(2)] = [HI]`

Answer

C

Explanation

`K_(c )= ([HI]^(2))/([H_(2)][I_(2)])`
`[H_(2)] = [I_(2)]` will be equilibrium, since it is same at initial state.
`K_(c )= 47.6`. i.e., concentration of products more than that of reactants.