For the equilibrium 2 NO 2 g - N 2 O 4 g - heat 14-6 kcal the increase intemperature wouldA- Not alter the equilibriumB- Stop the reactionC- Favour the formation of N 2 O 4D- Favour the decomposition of N 2 O 4

The correct option is D Favour the decomposition of N2O4 The reaction is endothermic in reverse direction and hence increase in temperature will favour rever ...

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Standard XII

Chemistry

Characteristics of Equilibrium Constant

For the equil...

Question

For the equilibrium $2 N O_{2} (g) ⇌ N_{2} O_{4} (g) + h e a t (14.6 k c a l)$ the increase in

temperature would

Favour the formation of N₂O₄

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Favour the decomposition of N₂O₄

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Not alter the equilibrium

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Stop the reaction

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Solution

The correct option is B
Favour the decomposition of N₂O₄

The reaction is endothermic in reverse direction and hence increase in

temperature will favour reverse reaction.

Suggest Corrections

Similar questions

Q. For equilibrium,

2 N O_{2} (g) ⇌ N_{2} O_{4} (g) + 14.6 k c a l

increases of temperature would

Q. For the equilibrium, an increase of temperature will,

{2 N O}_{2} (g) ⇌ N_{2} O_{4} (g) + 14.6 k c a l

Q. The gas phase reaction

2 N O_{2} (g) \to N_{2} O_{4} (g)

is an exothermic reaction The decomposition of

N_{2} O_{4} (g)

, in equilibrium mixture of

2 N O_{2}

(g) and

N_{2} O_{4} (g)

, can be increased by:

Assertion (A): For the reaction,

2 {N O}_{(g)} + O_{2 (g)} ⇌ 2 {N O}_{2 (g)}

, increase in pressure favours the formation of

{N O}_{2}

Reason (R): The reaction is exothermic.

N_{2} O_{4}

dissociates as,

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)

55^{o} C

and

1.2

atmosphere,

%

decomposition of

N_{2} O_{4}

50.0 %

.
At what pressure and same temperature, the equilibrium mixture has the ratio of

N_{2} O_{4} : N O_{2}

1 : 8

?
(Report the answer upto two decimal)

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For the equilibrium 2NO2(g) ⇌ N2O4(g) + heat(14.6 kcal) the increase in temperature would

The correct option is B Favour the decomposition of N2O4 The reaction is endothermic in reverse direction and hence increase in temperature will favour reverse reaction.

For the equilibrium $2 N O_{2} (g) ⇌ N_{2} O_{4} (g) + h e a t (14.6 k c a l)$ the increase in

temperature would

The correct option is B
Favour the decomposition of N₂O₄

The reaction is endothermic in reverse direction and hence increase in

temperature will favour reverse reaction.