Answer to Question #281278 in General Chemistry for Metro

Question

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

Answer 1

(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