Calculate the pressures of no, cl2, and nocl in an equilibrium mixture produced by the reaction of a starting mixture with 7.0 atm no and 3.5 atm cl2. (hint: kp is relatively large; assume the reaction goes to completion then comes back to equilibrium.)
2 no(g) + cl2(g) --> 2 nocl(g)kp = 2.9 ✕ 103 at 149°c

 The pressures of , , and in an equilibrium mixture are 0.4 atm , 0.2 atm and 6.6 atm respectively.

Explanation:

Initial pressure of = 7.0 atm

Initial pressure of = 3.5 atm

The given balanced equilibrium reaction is,

Initial pressure    7.0 atm   3.5 atm      0 atm

At eqm. conc.    (7-2x)atm  (3.5-x)atm   (2x) Matm

The expression for equilibrium constant for this reaction will be,

we are given :

Now put all the given values in this expression, we get :

Pressure of at equilibrium = (7-2x) =

pressure of at equilibrium = (3.5-x) =

pressure of at equilibrium = (2x) =

a

explanation:

hloride, what is the mass of calcium in

explanation: