Question

Consider the following reversible reaction N2O4 + 2NO2(g) . How is the composition of the

equilibrium mixture affected by :

(1).A change in temperature (2). A change in pressure ( 3). A change in concentration of

N2O4 (4). The removal of NO2 from the reaction mixture.
​

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.

hope it helps...