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,

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

"hydrogen bonding is the attraction of h atoms in the water molecule (slight + charge) to o atoms in a neighboring water molecule (slight - charge); it is a weak interatomic force. but it is still strong enough to the water molecules "stick" together."