In a vessel containing N2.H2 and NH3 at equilibrium,some helium gas is introduced so that pressure increases while temperature and volume remain constant.According to Le Chatelier’s principle, the dissociation of NH3
[A]increases
[B]decreases
[C]Remains unaltered
[D]Changes unpredictably
I think ans should be decreases as no of moles on right side are 4 while on Left side are 2..But ans is [C]..Can anyone tell how??
13As far as i've read.... adding an Inert gas at const. volume ,increases the Pressure but does not affect the Equilibrium...
Tht concept of moles is 2b used when the inert gas is added keeping "the Pressure" const. so tht only the volume changes...
1ya, true.
addition of inert gas ( here He ) to a system at constant volume has no effect on equillibrium condition.
addition of an inert gas at constant pressure has some effect on the equilibrium condition , as does by decreasing the system pressure i.e.
i) If np - nr > 0 , equilibrium shifts towards right.
ii) If np - nr < 0 , equilibrium shifts towards left.
iii) If np - nr = 0 , no effect on equilibrium.
as , here , its given at constant pressure , thus no effect on equilibrium
1357Here think in terms of Kc
As the concentration of all the substances remains same, there will be no shift
