1. Tardigrade
  2. Question
  3. Chemistry
  4. Consider the following reaction N 2 O 4( g ) leftharpoons 2 NO 2( g ) ; Δ H 0=+58 kJ For each of the following cases (a, b), the direction in which the equilibrium shifts is: (a) Temperature is decreased (b) Pressure is increased by adding N 2 at constant T

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Q. Consider the following reaction
$N _{2} O _{4}( g ) \rightleftharpoons 2 NO _{2}( g ) ; \Delta H ^{0}=+58 \,kJ$
For each of the following cases $(a, b),$ the direction in which the equilibrium shifts is:
(a) Temperature is decreased
(b) Pressure is increased by adding $N _{2}$ at constant $T$

JEE MainJEE Main 2020Equilibrium

Solution:

$\Delta H ^{\circ}>0 \quad T \downarrow$ equation shifts back ward.

$N _{2}$ is treated as inert gas in this case hence no effect on equilibrium