Question

Read the given passage and answer the questions 1 to 5 that follow :
One of the principal goals of chemical synthesis is to maximise the conversion ofthe reactants to products
while minimizing the expenditure of energy. This implies maximum yield of products at mild temperature and
pressure conditions. If it does not happen, then the experimental conditions need to be adjusted. For
example, in Haber's process for the synthesis of ammonia from N
H2
773 K
N2 + 3H2(e) 773 K2NH3)
A. Hº = - 46.1 kJ mol-1
K = 1.06 x 103
the choice of experimental conditions is of real economic importance. Annual world production of ammonia
is about hundred million tones, primarily for use as fertilizers.
1. Write an expression of K for the Haber's process.
What is the value of K for the reverse reaction of Haber's process?
Indicate the direction in which equilibrium ofabove reaction will shift when temperature is increased ?
4. What would be the effect of increase in pressure in the formation of ammonia ?
5. In which direction above reaction will proceed if value of Q = 2.04 x 103?​

Answer 1

Answer:

Don't know

Mark me as brainliest

Answer 2

(1). Expression of K for the Haber's process is ,

                 K =$[NH_{3}]^{2}$ / [N$_{2}$] $[H_{2}]^{3}$

(2). The value of K for the reverse reaction of Haber's process is 9.43 * $10^{-4}$

(3). When temperature is increased , the equilibrium of the  reaction of Haber's process shifted in backward direction .

(4). More ammonia is formed if the pressure is increased in Haber's process.

(5). When Q > K , reaction proceed in reverse direction .