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Standard XII

Chemistry

Characteristics of Equilibrium Constant

N2O4g ⇌ 2NO2g...

Question

$N_{2} O_{4} (g) ⇌ 2 N O_{2} (g); Δ H = 56.9 k J$
Which of the following will increase the yield of $N O_{2}$ of the equilibrium reaction?

Adding

N_{2} O_{4}

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Heating the reaction container

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Cooling the reaction container

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Adding a catalyst

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Solution

The correct option is B Heating the reaction container
For an endothermic reaction, the increment in temperature will lead the reaction in a forward direction and that change will increase the concentration of the $N O_{2}$
Thus heating the reaction container will increase the yield of $N O_{2}$ .

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Similar questions

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)

In this reaction the dissociation of

N_{2} O_{4}

x

then the how much mole will of

N_{2} O_{4}

and

N O_{2}

at equilibrium.

Q. For the reaction at equilbrium:

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)

, the concentration of

N_{2} O_{4}

and

N O_{2}

at equilibrium are

4.8 \times 10^{- 2}

and

1.2 \times 10^{- 2} mol/L

respectively. The value of

K_{c}

for the reaction is:

Q. For a reaction equilibrium,

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)

, the concentrations of

N_{2} O_{4}

and

N O_{2}

at equilibrium are

4.8 \times 10^{- 2}

and

1.2 \times 10^{- 2} m o l / L

respectively. The value of

K_{c}

, for the reaction is:

Q. When

0.5 m o l

N_{2} O_{4}

is placed in a

4.00 L

reaction vessel and heated at

400 K

79.3

% of the

N_{2} O_{4}

decomposes to

N O_{2}

. Calculate

K_{c}

and

K_{p}

400 K

for the reaction

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)

The reaction N $_{2}$ O $_{4}$ (g) $⇌$ 2NO $_{2}$ (g) is
carried out at 298 K and 20 bar. Five moles of each of N $_{2}$ O $_{4}$ and
NO $_{2}$ , are taken initially. Given: $Δ$ $_{f}$ G $^{\circ}$
(N $_{2}$ O $_{4}$ ) = 100 kJ mol $^{- 1}$ and $Δ$ $_{f}$ G $^{\circ}$
(NO $_{2}$ ) = 50 kJ mol $^{- 1}$ . The reaction proceeds at an initial pressure
of 20 bar. Determine the direction in which the reaction proceeds to achieve
equilibrium. Also determine the amounts of N $_{2}$ O $_{4}$ and NO $_{2}$ when the reaction attains equilibrium.

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N2O4(g)⇌2NO2(g); ΔH=56.9 kJWhich of the following will increase the yield of NO2 of the equilibrium reaction?

The correct option is B Heating the reaction containerFor an endothermic reaction, the increment in temperature will lead the reaction in a forward direction and that change will increase the concentration of the NO2 Thus heating the reaction container will increase the yield of NO2.

$N_{2} O_{4} (g) ⇌ 2 N O_{2} (g); Δ H = 56.9 k J$
Which of the following will increase the yield of $N O_{2}$ of the equilibrium reaction?

The correct option is B Heating the reaction container
For an endothermic reaction, the increment in temperature will lead the reaction in a forward direction and that change will increase the concentration of the $N O_{2}$
Thus heating the reaction container will increase the yield of $N O_{2}$ .