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Heat of Reaction

The gas phase...

Question

The gas phase reaction $2 N O_{2} (g) ⇌ N_{2} O_{4} (g)$ is an exothermic reaction. The decomposition of $N_{2} O_{4}$ in equilibrium mixuture of $N O_{2} (g)$ and $N_{2} O_{4} (g)$ can be increased by:

increasing the pressure

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addition of an inert gas at constant pressure

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lowering the temperature

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addition of an inert gas at constant volume

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Solution

The correct option is B addition of an inert gas at constant pressure
Reaction at equilibrium
$2 N O_{2} (g) ⇌ N_{2} O_{4} (g)$

(1) According to Le chatelier's principle: Increasing the pressure on a gas reaction shifs the position of equilibrium toward the side with fewer molecules.
So, it will move in backward direction which leads to formation of $N_{2} O_{4} (g)$

(2) Addition of an inert gas to constant pressure will increase volume and equilibrium shifts towards more number of molecules i.e. there will be decompostion.

(3) Decomposition of $N_{2} O_{4}$ is endothermic. So, the reaction will move in forward reaction when the temperature is increased.

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Similar questions

Q. At the equilibrium of the reaction,

N_{2} O_{4} (g) ⇌ 2 {N O}_{2} (g)

, the observed molar mass of

N_{2} O_{4}

77.70 g

. The percentage dissociation of

N_{2} O_{4}

is:

9.2 g r a m s

N_{2} O_{4} (g)

is taken in a closed one-litre vessel and heated till the following equilibrium is reached.

N_{2} O_{4} (g) ⇌ 2 {N O}_{2} (g)

At equilibrium,

50

N_{2} O_{4} (g)

is dissociated. What is the equilibrium constant? (in mol litre

^{- 1}

)

[Molecular weight of

N_{2} O_{4} = 92

]

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

Determine the heat of reaction for the above reaction, if the heat of formation,

Δ H_{f}

for

{N O}_{2} (g)

is 34

k J / m o l e

and

N_{2} O_{4} (g)

is 10

k J / m o l e

Q. The decomposition of

N_{2} O_{4}

{N O}_{2}

is carried at

280 K

in chloroform. When equilirbrium has been established,

0.2

mole of

N_{2} O_{4}

and

2 \times 10^{- 3}

mole of

{N O}_{2}

are present in

2

litre solution. The equilibrium constant for the reaction,

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)

is:

Q. Gaseous

N_{2} O_{4}

dissociates into gaseous

{N O}_{2}

according to the reaction

N_{2} O_{4} (g) ⇌ 2 {N O}_{2} (g)

. At

300 K

and

1 a t m

pressure, the degree of dissociation of

N_{2} O_{4}

0.2

. If one mole of

N_{2} O_{4}

gas is contained in a vessel, then the density of the equilibrium mixture is:

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The gas phase reaction 2NO2(g)⇌N2O4(g) is an exothermic reaction. The decomposition of N2O4 in equilibrium mixuture of NO2(g) and N2O4(g) can be increased by:

The gas phase reaction $2 N O_{2} (g) ⇌ N_{2} O_{4} (g)$ is an exothermic reaction. The decomposition of $N_{2} O_{4}$ in equilibrium mixuture of $N O_{2} (g)$ and $N_{2} O_{4} (g)$ can be increased by: