Question

. Explain the effects of temperature and pressure on the following equilibrium.
2NO2(g) N2O4 (g) ∆H = -57.2 kJmol –1

Answer 1

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 NO

2

(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., N

2

O

4

(g) direction.

(iii) If we increase concentration of N

2

O

4

, then to keep equilibrium constant, more N

2

O

4

decomposes and greater amount of NO

2

is produced.

(iv) If we remove NO

2

from the reaction mixture then to keep equilibrium constant more N

2

O

4

decomposes to produce NO

2

to minimize that effect.