1. Tardigrade
  2. Question
  3. Chemistry
  4. 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

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Q.
Column I Column II
A Dissociation of $N _2 O _4( g )$ $N _2 O _4( g ) \rightleftharpoons 2 NO _2( g )$ $\Delta H=+57.0\, kJ$ p Increases with temperature
B Oxidation of $NH _3( g )$ $4 NH _3( g )+5 O _2( g ) \rightleftharpoons$ $4 NO ( g )+6 H _2 O ( g ) \Delta H=-900.0 \,kJ $ q Decreases with pressure
C Oxidation of nitrogen $ N _2( g )+ O _2( g ) \rightleftharpoons 2 NO ( g ) \text {; } \Delta 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 ) \rightleftharpoons NO _2( g ) + O_2(g) ; \Delta H = -200\,kJ$ s Decreases with temperature

Equilibrium

Solution:

$( a \rightarrow p , r )$ 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
$( b \rightarrow q , r , s )$ It is exothermic reaction hence on increasing temperature reaction proceed in backward direction $( c \rightarrow p )$ Endothermic reaction therefore on increasing temperature reaction proceed in product side $( d \rightarrow s )$ Exothermic reaction therefore on increasing temperature reaction proceed in backward side