• 072920 77839
  • info@smartachievers.in
Menu
Back
  • JEE ADVANCE
  • JEE MAIN
  • NEET
  • BITSAT
  • CBSE BOARD
  • UP BOARD
  • CUET
JEE ADVANCE
  • CLASS XI - XII
  • CRASH COURSE
CRASH COURSE
JEE MAIN
  • CLASS XI - XII
  • CRASH COURSE
CRASH COURSE
NEET
  • CLASS XI - XII
  • CRASH COURSE
BITSAT
  • CLASS XI - XII
CBSE BOARD
  • CLASS IX
  • CLASS X
  • CLASS XI
  • CLASS XII
  • CLASS VI
  • CLASS VII
  • CLASS VIII
UP BOARD
  • CLASS IX
  • CLASS X
  • CLASS XI
  • CLASS XII
CUET
  • CRASH COURSE
Courses


Solution


Q.

For the reaction in equilibrium

N2(g)+3H2(g)⇌2NH3(g),  ΔH=-Q

Reaction is favoured in the forward direction by                      [2024]
1 use of catalyst  
2 decreasing concentration of N2  
3 low pressure, high temperature and high concentration of ammonia  
4 high pressure, low temperature and higher concentration of H2  

Ans.

(4)

According to Le Chatelier’s principle:
(i) Raising the temperature shifts the equilibrium to the left and decreases the equilibrium concentration of ammonia. In other words, low temperature is favourable for high yield of ammonia, but practically very low temperatures slow down the reaction and thus a catalyst is used.
    
(ii) If H2 is added to the reaction mixture at equilibrium, then the equilibrium of the reaction is disturbed. In order to restore it, the reaction proceeds in a direction wherein H2 is consumed, i.e., more of H2 and N2 react to form NH3 and finally the equilibrium shifts in the right (forward) direction.
    
(iii) As the pressure increases, the equilibrium shifts in the forward direction, a direction in which the number of moles of the gas decreases.