Le Chatelier'...

Le Chatelier's Principle for Del N Lesser Than Zero

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Q. In the following reversible reaction

2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g) Δ H = - Q C a l

, where Q is positive. Most suitable condition for the higher production of

S O_{3}

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

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What is the physical significance of first law of thermodynamics?

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Q. In which of the following reactions, the increase in volume of the container will favour the formation of products?

$C (s) + H_{2} O (g) ⇌ C O (g) + H_{2} (g)$
$H_{2} (g) + I_{2} (g) ⇌ 2 H I (g)$
$4 N H_{3} (g) + 5 O_{2} (g) ⇌ 4 N O (g) + 6 H_{2} O (l)$
$3 O_{2} (g) ⇌ 2 O_{3} (g)$

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Can the First Law of Thermodynamics be violated?

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Under NTP conditions, which temperature is taken into account ?

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Q. When the value of

K_{c}

is very small then:

Reaction is at start
Product conc. is maximum
Reactant conc. is minimum
Reaction is completed

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Q. For a hypothetical reaction of the kind

A B_{2} (g) + \frac{1}{2} B_{2} (g) ⇌ A B_{3} (g); Δ H = - x k J

A B_{3}

could be produced at equilibrium by:

Using a catalyst
Removing some of $B_{2}$
Increasing the temperature
Increasing the pressure

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In the reaction $A (g) + 2 B (g) ⇌ C (g) + Q k J,$ greater product will be obtained

or the forward reaction is favoured by

At high temperature and high pressure
At high temperature and low pressure
At low temperature and high pressure
At low temperature and low pressure

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Q. Consider two reactions given below:
Reaction 1 :

A (a q .) ⇌ A^{n +} (a q .) + n e^{-}

E^{\circ} = 1.88 V

Reaction 2:

B (a q .) ⇌ B^{n +} (a q .) + n e^{-}

E^{\circ} = - 2.88 V

Which of the following option(s) is/are correct?

Reactant A has the tendency to get oxidised
Reactant B has the tendency to get reduced
Reactant A has the tendency to get reduced
Reactant B has the tendency to get oxidised

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Q. Consider two reactions given below:
Reaction 1 :

A (a q .) ⇌ A^{n +} (a q .) + n e^{-}

E^{\circ} = 1.88 V

Reaction 2:

B (a q .) ⇌ B^{n +} (a q .) + n e^{-}

E^{\circ} = - 2.88 V

Which of the following options is correct?

Reactant A has the tendency to get oxidised
Reactant B has the tendency to get reduced
Reactant A has the tendency to get reduced
Both (a) and (b)

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Q. Find out the value of

K_{C}

for each of the following equilibrium respectively from the value of

K_{P}

.
(i)

2 N O C l (g) ⇌ 2 N O (g) + C l_{2} (g); K_{P} = 1.8 \times 10^{- 2}

500

K
(ii)

C a C O_{3} (s) ⇌ C a O (s) + C O_{2} (g); K_{P} = 167

1073

$4.4 \times 10^{- 4}$ & $1.90$
$8.8 \times 10^{- 4}$ & $3.8$
$8.8 \times 19^{4}$ & $3.8$
$4.4 \times 10^{4}$ & $1.90$

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Q. A hypothetical reaction;

A_{2} + B_{2} \to 2 A B

follows the mechanism given below:

A_{2} ⇌ A + A (f a s t)

A + B_{2} \to A B + B (s l o w)

A + B \to A B (f a s t)

The order of the overall reaction is:

$2$
$1$
$1 \frac{1}{2}$
$0$

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Q. In the following reversible reaction,

2 S O_{2} + O_{2} \to 2 S O_{3} Δ H = - Q c a l

Most suitable condition for the higher production of

S O_{3}

is:

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

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Q. If the equilibrium constants of a reaction at

298 K

and

308 K

are

1.0 \times 10^{- 2}

and

2 \times 10^{- 2}

respectively, then the reaction is:

endothermic
exothermic
may be endothermic or exothermic
cannot be predicted

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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 kJ

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

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State whether the given statement is true or false:

A reaction for which

Δ S

is positive is always spontaneous.

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C a C O_{3} (s) ⇌ C a O (s) + C O_{2} (g), K = 10^{- 9}

300 K

. The value of

p_{c o_{2}}

10^{- x}

x

is ____.

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Q. The rate constant of forward and backward reactions for certain hypothetical reaction are

1.1 \times 10^{- 2}

and

1.5 \times 10^{- 3}

respectively. The equilibrium constant of the reaction is:

7.33
0.733
73.3
733

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Q. For the reaction :

C a C O_{3} (s) ⇌ C a O (s) + C O_{2} (g), K_{p} = 1

atm at

927^{o} C

. If 20g of

C a C O_{3}

were kept in a 10 litre vessel at

927^{o} C

, then calculate percentage of

C a C O_{3}

remaining at equilibrium:

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Q. For which of the following reactions will the equilibrium mixture contain an appreciable concentration of both reactants and products?

$C l_{2} (g) ⇌ 2 C l (g); K_{c} = 6.4 \times 10^{- 39}$
$C l_{2} (g) + 2 N O (g) ⇌ 2 N O C l (g); K_{c} = 3.7 \times 10^{8}$
$C l_{2} (g) + 2 N O (g) ⇌ 2 N O_{2} C l (g); K_{c} = 1.8$
$H_{2} (g) + I_{2} (g) ⇌ 2 H I (g) . K_{c} = 49$

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Q. Which of the following is correct for a spontaneous reaction at any temperature?

$Δ H = - v e, Δ S = + v e, Δ G = - v e$
$Δ H = - v e, Δ S = - v e, Δ G = - v e$
$Δ H = + v e, Δ S = + v e, Δ G = - v e$
$Δ H = - v e, Δ S = + v e, Δ G = + v e$

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Q. In the following equilibrium reaction involving the dissociation of

C a C O_{3}

, the equilibrium constant is given by:

C a C O_{2} (s) ⇌ C a O (s) + C O_{2} (g)

$\frac{P_{C a O} \times P_{C O_{2}}}{P_{C a C P_{3}}}$
$C_{C a O} \times \frac{P_{C O_{2}}}{C_{C a C O_{3}}}$
$\frac{P_{C a O}}{P_{C a C O_{3}}}$
$P_{C O_{2}}$

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Q. In a reversible reaction, some amount of heat energy is liberated in the forward reaction. Name the reaction. What change in temperature favours the forward reactions?

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Q. Identify the correct statement from the following in a chemical reaction.

The change in entropy along with suitable change in enthalpy decides the rate of reaction
The entropy always increases
The enthalpy always decreases
Both the enthalpy and the entropy remains constant

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Q. In which of the following case,

E_{a}

of the backward reaction is greater than that of the forward reaction?

$A + 10 k c a l \to B, E_{a} = 50 k c a l$
$A + 20 k c a l \to B, E_{a} = 40 k c a l$
$A + 40 k c a l \to B, E_{a} = 10 k c a l$
$A - 40 k c a l \to B, E_{a} = 20 k c a l$

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For a spontaneous reaction the $Δ G$ , equilibrium constant $(K_{e q})$ and $E_{c e l l}^{0}$ will be respectively

-ve , >1 , -ve
-ve , <1 , -ve
+ve , >1 , -ve
-ve , >1 , +ve

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Q. If

K_{1}

and

K_{2}

are the respective equilibrium constants for the two reactions:

X e F_{6} (g) + H_{2} O (g) \Leftrightarrow X e O F_{4} (g) + 2 H F (g)

X e O_{4} (g) + X e F_{6} (g) \Leftrightarrow X e O F_{4} (g) + X e O_{3} F_{2} (g)

The equilibrium constant of the reaction

X e O_{4} (g) + 2 H F (g) \Leftrightarrow X e O_{3} F_{2} (g) + H_{2} O (g)

will be:

$\frac{K_{1}}{K_{2}}$
$K_{1} \times K_{2}$
$\frac{K_{2}}{K_{1}}$
$\frac{K_{1}}{(K_{2})^{2}}$

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Q. A sample of

C a C O_{3} (s)

is introduced into a sealed container of volume 0.821 litre & heated to 1000 K until equilibrium is reached. The equilibrium constant for the reaction

C a C O_{3} (s) ⇌ C a O (s) + C O_{2} (g)

4 \times 10^{2} a t m

at this temperature. Calculate the mass of CaO present at equilibrium

$112$ mg
$224$ mg
$448$ mg
None of these

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In the reaction A(g) + 2B(g) $⇌$ C(g) + Q kJ of heat, more product will be obtained

or the forward reaction is favoured by

At high temperature and high pressure
At high temperature and low pressure
At low temperature and high pressure
At low temperature and low pressure

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Q. The following reactions occurs at 500K . Arrange them in order of increasing tendency to proceed to completion.
1)

2 N O C I (g) ⇌ 2 N O (g) + C l_{2} (g); K_{p} = 1.7 \times 10^{- 2}

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g); K_{p} = 1.5 \times 10^{- 3}

2 S O_{3} (g) ⇌ S O_{2} (g) + O_{2} (g); K_{p} = 1.3 \times 10^{- 5}

2 N O_{2} (g) ⇌ 2 N O (g) + O_{2} (g); K_{p} = 5.9 \times 10^{- 5}

1 < 3 < 4 < 2
4 < 3 < 1 < 2
2 < 1 < 4 < 3
3 < 4 < 2 < 1

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