Consider the following reactions and their respective equilibrium constants: no(g)+12br2(g)⇌nobr(g)kp=5.3 2no(g)⇌n2(g)+o2(g)kp=2.1×1030 use these reactions and their equilibrium constants to predict the equilibrium constant for the following reaction: n2(g)+o2(g)+br2(g)⇌2nobr(g)

Answer :  The equilibrium constant for the given reaction is,

Explanation :

The given equilibrium reactions are,

(i) ;  

(ii) ;  

Now we have to determine the equilibrium constants for the following equilibrium reactions.

(iii) ;  

From the given reaction we conclude that, the reaction (iii) will takes place when reverse the reaction (ii) and reaction (i) is multiplied by 2 and then adding all the reaction.

Thus, the equilibrium constant will be:

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

Therefore, the equilibrium constant for the given reaction is,

the answer is 303.15 or 303

hey there!

mass = 6.75 g

volume =   9 cm³

therefore:

d = mass / volume

d   = 6.75 / 9

d = 0.7 g/cm³

answer b