To study the decomposition of hydrogen iodide, a student fills an evacuated 3 litre flask with0.3 mole of HI gas and allows the reaction to proceed at 500^@C. At equilibrium he found the concentratin of HI which is equal to 0.05 M. Calculate K_C and K_P for this reaction.

To study the decomposition of hydrogen iodide, a student fills an evac

1.	To study the decomposition of hydrogen iodide, a student fills an evacuated 3 litre flask with0.3 mole of HI gas and allows the reaction to proceed at 500^@C. At equilibrium he found the concentratin of HI which is equal to 0.05 M. Calculate K_C and K_P for this reaction.
Answer» Solution :`V = 3L` `[HI]_("initial") = (0.3 mol)/(3L) = 0.1 M` `[HI]_(EQ)= 0.05 M` `2HI (g) hArr H_2(g) + I_2(g)` `K_C = ([H_2][I_2])/([HI]^2) = (0.025 xx 0.025)/(0.05 xx 0.05)` `K_C = 0.25` `K_P = K_C (RT)^(Deltan_g)` `DELTA n_g = 2-2=0` `K_P = 0.25 (RT)^0` `K_P = 0.25`