Column I Column II A Dissociation of N 2 O 4( g ) N 2 O 4( g ) leftharpoons 2 NO 2( g ) Δ H=+57.0 kJ p Increases with temperature B Oxidation of NH 3( g ) 4 NH 3( g )+5 O 2( g ) leftharpoons 4 NO ( g )+6 H 2 O ( g ) Δ H=-900.0 kJ q Decreases with pressure C Oxidation of nitrogen N 2( g )+ O 2( g ) leftharpoons 2 NO ( g ) text ; Δ H=+180.0 kJ r Increases with addition of inert gas at constant pressure D Formation of NO 2( g ) NO 2+ O 3( g ) leftharpoons NO 2( g ) + O2(g) ; Δ H = -200 kJ s Decreases with temperature

Question

Column I Column II A Dissociation of N 2 O 4( g ) N 2 O 4( g ) leftharpoons 2 NO 2( g ) Δ H=+57.0 kJ p Increases with temperature B Oxidation of NH 3( g ) 4 NH 3( g )+5 O 2( g ) leftharpoons 4 NO ( g )+6 H 2 O ( g ) Δ H=-900.0 kJ q Decreases with pressure C Oxidation of nitrogen N 2( g )+ O 2( g ) leftharpoons 2 NO ( g ) text ; Δ H=+180.0 kJ r Increases with addition of inert gas at constant pressure D Formation of NO 2( g ) NO 2+ O 3( g ) leftharpoons NO 2( g ) + O2(g) ; Δ H = -200 kJ s Decreases with temperature (A) A - (p,r), B - (q,r,s), C - (p), D - (s) (B) A - (q,r,s), B - (p), C - (s), D - (p,r) (C) A - (s), B - (p,r), C - (p,r), D - (q,r,s) (D) A - (p), B - (s), C - (q,r,s), D - (p,r)

Tardigrade Admin · Accepted Answer

( a arrow p , r ) It is endothermic reaction hence on increasing temperature reaction proceed in forward direction. On addition of inert gas, at constant pressure also favour product side according to le-Chatelier principle ( b arrow q , r , s ) It is exothermic reaction hence on increasing temperature reaction proceed in backward direction ( c arrow p ) Endothermic reaction therefore on increasing temperature reaction proceed in product side ( d arrow s ) Exothermic reaction therefore on increasing temperature reaction proceed in backward side

Column I		Column II
A	Dissociation of $N_{2} O_{4} (g)$ $N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)$ $Δ H = + 57.0 k J$	p	Increases with temperature
B	Oxidation of $N H_{3} (g)$ $4 N H_{3} (g) + 5 O_{2} (g) ⇌$ $4 NO (g) + 6 H_{2} O (g) Δ H = - 900.0 k J$	q	Decreases with pressure
C	Oxidation of nitrogen $N_{2} (g) + O_{2} (g) ⇌ 2 NO (g); Δ H = + 180.0 k J$	r	Increases with addition of inert gas at constant pressure
D	Formation of $N O_{2} (g)$ $N O_{2} + O_{3} (g) ⇌ N O_{2} (g) + O_{2} (g); Δ H = - 200 k J$	s	Decreases with temperature