For the reaction N_(2(g)) + 3H_(2(g)) hArr 2NH_(3(g)), the standard equilibrium constant K_P is 5.8xx10^5 at 298 K temperature . If the concentration of gases indicate by mol L^(-1) then find the value of standard equilibrium constant from the following. (R=0.08314 L bar K^(-1) "mol"^(-1) )

For the reaction N_(2(g)) + 3H_(2(g)) hArr 2NH_(3(g)), the standard eq

1.	For the reaction N_(2(g)) + 3H_(2(g)) hArr 2NH_(3(g)), the standard equilibrium constant K_P is 5.8xx10^5 at 298 K temperature . If the concentration of gases indicate by mol L^(-1) then find the value of standard equilibrium constant from the following. (R=0.08314 L bar K^(-1) "mol"^(-1) )
Answer» `3.5xx10^6` `3.8xx10^7` `3.56xx10^(+8)` `3.99xx10^9` Solution :`{:(,N_2+,3H_2hArr, 2NH_3),("Mole",1,3,2),("Total of REACTANTS" ,,"4 mol", "2 mol products"):}` `Deltan_((G))` = mole of products 0 mole of reactants =(2-4)=-2 `K_p=K_c(RT)^(Deltan)` `therefore K_c=K_p/(RT)^(Deltan)` `=(5.8xx10^5)/(0.08314xx298)^(-2)` `=(5.8xx10^5)(0.08314xx298)^2` `=3.561xx10^8`