Le Chatelier'...

Le Chatelier's Principle for Del N Greater Than Zero

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Q. Which of the following reactions proceed at low pressure?

$P C l_{5} ⇌ P C l_{3} + C l_{2}$
$N_{2} + O_{2} ⇌ 2 N O$
$N_{2} + 3 H_{2} ⇌ 2 N H_{3}$
$H_{2} + I_{2} ⇌ 2 H I$

Q. Which one of the following conditions will favour maximum formation of the product in the reaction,

A_{2} (g) + B_{2} (g) ⇌ X_{2} (g); Δ_{r} H = - X k J

?

 NEET 2018

High temperature and low pressure
Low temperature and high pressure
High temperature and high pressure
Low temperature and low pressure

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For an equilibrium $H_{2} O (s) ⇌ H_{2} O (l)$ , which of the following statements is true?

The pressure changes do not affect the equilibrium
More of ice melts if pressure on the system is increased
More of liquid freezes if pressure on the system is increased
The pressure changes may increase or decrease the degree of advancement of the reaction depending upon the temperature of the system

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Q. For the reaction,

P C l_{5} (g) ⇌ P C l_{3} (g) + C l_{2} (g)

the forward reaction at constant temperature is favoured by

introducing an inert gas at constant volume
introducing an inert gas at constant pressure
increasing the volume of the container
introducing $P C l_{5}$ at constant volume

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Q. Thermal decomposition of gaseous

X_{2}

to gaseous X at 298 K takes place according to the following equation:

X_{2} (g) ⇌ 2 X (g)

The standard reaction Gibbs energy,

Δ_{r} G^{0},

of this reaction is positive. At the start of the reaction, there is one mole of

X_{2}

and no X. As the reaction proceeds, the number of moles of X formed is given by

β

. Thus,

β_{e q u i l i b r i u m}

is the number of moles of X formed at equilibrium. The reaction is carried out at a constant total pressure of 2 bar. Consider the gases to behave ideally. (Given: R = 0.083 L bar

K^{- 1} m o l^{- 1}

)

The equilibrium constant

K_{p}

for this reaction at 298 K, in terms of

β_{e q u i l i b r i u m},

is:

$\frac{8 β_{e q u i l i b r i u m}^{2}}{4 - β_{e q u i l i b r i u m}^{2}}$
$\frac{4 β_{e q u i l i b r i u m}^{2}}{2 - β_{e q u i l i b r i u m}}$
$\frac{4 β_{e q u i l i b r i u m}^{2}}{4 - β_{e q u i l i b r i u m}^{2}}$
$\frac{8 β_{e q u i l i b r i u m}^{2}}{2 - β_{e q u i l i b r i u m}}$

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Q. Thermal decomposition of gaseous

X_{2}

to gaseous X at 298 K takes place according to the following equation:

X_{2} (g) ⇌ 2 X (g)

The standard reaction Gibbs energy,

Δ_{r} G^{0},

of this reaction is positive. At the start of the reaction, there is one mole of

X_{2}

and no X. As the reaction proceeds, the number of moles of X formed is given by

β

. Thus,

β_{e q u i l i b r i u m}

is the number of moles of X formed at equilibrium. The reaction is carried out at a constant total pressure of 2 bar. Consider the gases to behave ideally. (Given: R = 0.083 L bar

K^{- 1} m o l^{- 1}

).

The INCORRECT statement among the following, for this reaction is:

Decrease in the total pressure will result in formation of more moles of gaseous X
At the start of the reaction, dissociation of gaseous $X_{2}$ takes place spontaneously
$K_{c} < 1$
$β_{e q u i l i b r i u m} = 0.7$

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Q. Which of the following reactions proceed at low pressure ?

$N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g)$
$H_{2} (g) + I_{2} (g) ⇌ 2 H I (g)$
$N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)$
$P C l_{5} (g) ⇌ P C l_{3} (g) + C l_{2} (g)$

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Q. Acetic acid

C H_{3} C O O H

can form a dimer

(C H_{3} C O O H)_{2}

in the gas phase. The dimer is held together by two H-bonds with a total strenght of 66.5 kJ per mol of dimer

If at

25^{o} C,

the equilibrium constant for the dimerization is

1.3 \times 10^{3} .

Calculate

△ S^{o}

for the reaction:

2 C H_{3} C O O H (g) ⇌ (C H_{3} C O O H)_{2} (g)

$- 0.263 k J$
$- 0613 k J$
$- 0.463 k J$
$- 0.163 k J$

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Q. For a given reaction:

C (s) + O_{2} (g) \to C o (g) + H_{2} (g)

25^{o} C

Δ H = 131 k J / m o l

Given:

K_{p}

9.36 \times 10^{- 17}

Calculate the value of reaction constant at

700^{o} C

$0.915$
$0.214$
$0.583$
$0.797$

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Q. The exothermic formation of

C I F_{3}

is represented by the equation:

C l_{2} (g) + 3 F_{2} (g) ⇌ 2 C I F_{3} (g); △ H = - 329 k J

Which of the following will increase the quantity of

C I F_{3}

in an equilibrium mixture of

C l_{2}, F_{2} a n d C I F_{3}

By addition of $F_{2}$
Increasing the volume of the container
By removal of $C l_{2}$
Increasing the temperature

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