JEE MAIN - Chemistry (2020 - 5th September Morning Slot - No. 11)
Consider the following reaction:
N2O4(g) ⇌ 2NO2(g); $$\Delta $$Ho = +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 N2 at constant T.
N2O4(g) ⇌ 2NO2(g); $$\Delta $$Ho = +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 N2 at constant T.
(a) towards reactant, (b) towards product
(a) towards reactant, (b) no change
(a) towards product, (b) towards reactant
(a) towards product, (b) no change
Explanation
$$ \because $$ Given reaction is endothermic.
$$ \therefore $$ On decreasing temperature backward reaction will be favoured.
On adding N2, pressure is increased at constant T, and volume would also be constant so no change is observed.
$$ \therefore $$ On decreasing temperature backward reaction will be favoured.
On adding N2, pressure is increased at constant T, and volume would also be constant so no change is observed.
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