Nitric oxide reacts with Br_2 and gives nitrosyl bromide as per reaction given below: 2NO_((g)) + Br_(2(g)) hArr 2NOBr_((g)) When 0.087 mol of NO and 0.0437 mol of Br_2 are mixed in a closed container at constant temperature, 0.0518 mol of NOBr is obtained at equilibrium. Calculate equilibrium amount of NO and Br_2.

Nitric oxide reacts with Br_2 and gives nitrosyl bromide as per reacti

1.	Nitric oxide reacts with Br_2 and gives nitrosyl bromide as per reaction given below: 2NO_((g)) + Br_(2(g)) hArr 2NOBr_((g)) When 0.087 mol of NO and 0.0437 mol of Br_2 are mixed in a closed container at constant temperature, 0.0518 mol of NOBr is obtained at equilibrium. Calculate equilibrium amount of NO and Br_2.
Answer» Solution :According to stoichiometry of REACTION 2 MOL NO react with 1 mol `Br_2` and 2 mol NOBR formed. So, 2x mol NO react with X mol `Br_2` and from 2x mol NOBr. `{:("Reaction",2NO_((g))+ , Br_(2(g))HARR , 2NOBr_((g))),("Initial mol :",0.087 , 0.0437,Zero),("Reaction change :", "-2x mol","-x mol","+2x mol"),("Mol. at equilibrium :", (0.087-2x),0.0437-x , 2x=0.0518):}` `therefore x=0.0518/2`=0.0259 mol Thus, at equilibrium mol of NO = (0.087-2x) =0.087-0.0518 = 0.0352 mol mol of `Br_2`= (0.0437 -x) = 0.0437-0.0259 = 0.178