Question #281278
Consider this reaction: 2NOCI(g)⇌NO2(G)+CI2(g) ∆ H=77.16 KJ/mol
Predict the direction of shifting (to the left/right) if the following stresses are applied
1) [NOCI] is increased
2) Temperature is decreased
3)pressure is increased
4) [CI2] is increased
Expert's answer
(i) With increase in temperature, the equilibrium will shift to right according to Le Chatelier's principle. Thus, with an increase in temperature, more NO2
(g) is produced and vice-versa.
(ii) Forward reaction is accompanied by increase in mole number. According to Le Chateliers principle with increase in pressure the equilibrium will shift in that direction where number of mole decreases. i.e., N2
O4
(g) direction.
(iii) If we increase concentration of N2
O4
, then to keep equilibrium constant, more N2
O4
decomposes and greater amount of NO2
is produced.
(iv) If we remove NO2
from the reaction mixture then to keep equilibrium constant more N2
O4
decomposes to produce NO2
to minimize that effect
