Consider the reaction: N2O4(g) 2NO2(g), H0 = +58\ kJ For each case, the direction in which equilibrium shifts is: (a)…
Chemical Equilibrium · Class 11 · JEE Main Previous Year Question
Consider the reaction: ,
For each case, the direction in which equilibrium shifts is: (a) Temperature is decreased. (b) Pressure is increased by adding at constant T.
- a
(a) towards product, (b) towards reactant
- b
(a) towards reactant, (b) towards product
- c✓
(a) towards reactant, (b) no change
- d
(a) towards product, (b) no change
(a) towards reactant, (b) no change
Step 1 — Case (a): Temperature decreased Reaction is endothermic ( kJ). By Le Chatelier's principle:
- Decreasing T removes heat equilibrium shifts in the direction that produces heat backward (toward , reactant)
Step 2 — Case (b): Pressure increased by adding at constant T
- is an inert gas added at constant temperature
- At constant T, adding inert gas at constant volume partial pressures of and unchanged
- no change in equilibrium position
Answer: Option (3) — (a) toward reactant, (b) no change
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