Question

1 mole of a gas 'AB' dissociates to an extent of 10% at 127°C according to AB = A + B.
Occupies a volume of 4 x 10^4 ml. find total pressure at this temp, assuming ideal gas behaviour.​

Answer 1

Answer:

1.084 N/m.

Explanation:

Since, the chemical equation is a dissociation reaction hence, the van't hoff factor for the given dissociation reaction in the question will be i=1+d(n-1) for the reaction the value of n will be 2 and d=0.1. So, i=1+0.1(2-1) which will be   i=1.1.

So, the ideal gas equation is PV=inRT, in which P is the total pressure, v is the volume, i is the van't hoff factor , t is the temperature and R is the Rydberg constant. So, on substituting the values we will get that P*40=1.1*2*0.082*400 which on solving we will get the P = 1.084 N/m.