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Standard VII

Physics

Measurement of Volume

At the equili...

Question

At the equilibrium of the reaction :
$A_{(g)} + 2 B_{(s)} ⇌ C_{s} + 2 D_{(s)} + E_{(g)},$ A reacts to the extent of 20% at 400 K and to the extent of 25% at 300K. The equilibrium shifts in forward direction

On increasing both pressure and temperature

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On decreasing both pressure and temperature

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On decreasing temperature only

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On using the catalyst

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Solution

The correct option is C
On decreasing temperature only

K will increase on decreasing temperature. So the reaction is exothermic

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Similar questions

At the equilibrium of the reaction :
$A_{(g)} + 2 B_{(s)} ⇌ C_{s} + 2 D_{(s)} + E_{(g)},$ A reacts to the extent of 20% at 400 K and to the extent of 25% at 300K. The equilibrium shifts in forward direction

N_{2} O_{4}

at an initial pressure of

2 a t m

and

300 K

dissociates to an extent of

20

% at the same temperature by the time equilibrium is established.

K_{p}

for this reaction

2 N O_{2} ⇌ N_{2} O_{4}

is:

Q. Assertion :Assertion : In the dissociation of

P C l_{5}

at constant pressure and temperature addition of helium at equilibrium increases the dissociation of

P C l_{5}

. Reason: Reason : Helium reacts with

C l_{2}

and hence shifts the equilibrium in forward direction.

Q. Equilibrium constant,

K_{C}

for the reaction

N_{2} (g) + 3 H_{2} (g) ⇋ 2 N H_{3} (g)

at 500 K is 0.061
At a particular time, the analysis shows that composition of the reaction mixure is

3.0 m o l L^{- 1}

N_{2}, 2.0

m o l L

^{- 1} H_{2}

and

0.5 m o l L^{- 1}

N H_{3}

. Is the reaction at equilibrium and if not in which direction does the reaction tend to proceed to reach equilibrium?

Q. IF

P C l_{5}

dissociate to an extent of 80% at 523 K.Calculate the vapour density of the equilibrium mixture at 523 K.

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At the equilibrium of the reaction : A(g)+2B(s)⇌Cs+2D(s)+E(g), A reacts to the extent of 20% at 400 K and to the extent of 25% at 300K. The equilibrium shifts in forward direction

The correct option is C On decreasing temperature only K will increase on decreasing temperature. So the reaction is exothermic

At the equilibrium of the reaction :
$A_{(g)} + 2 B_{(s)} ⇌ C_{s} + 2 D_{(s)} + E_{(g)},$ A reacts to the extent of 20% at 400 K and to the extent of 25% at 300K. The equilibrium shifts in forward direction

The correct option is C
On decreasing temperature only

K will increase on decreasing temperature. So the reaction is exothermic