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) =

answer: e.   sour taste

explanation: acids are those substances which dissociates in water to give ions. as they dissociate to give ions, they act as electrolytes and thus are electrically conductive. acids are sour in taste. example: hcl

bases are those substances which dissociates in water to give ions or accepts ions. as they dissociate to give ions, they act as electrolytes and thus are electrically conductive. bases are bitter in taste. bases are slippery in nature.

it would be b. 6co2 + 6h2o --> c6h12o6 + 6o2