At constant temperature, the equilibrium constant ( K p ) for the decomposition reaction: N 2 O 4 ⇌ 2 NO 2 , is expressed by K p = 4 x 2 P ( 1 - x 2 ) , where P is the pressure and x is the extent of decomposition. Which of the following statements is true?

K p remains constant with change in P and x .

K p increases with increase in P .

K p increases with increase in x .

K p increases with decrease in x .

The exothermic formation of ClF 3 is represented by the following equation: Cl 2 g + 3 F 2 g ⇌ 2 ClF 3 g ; ΔH = - 329 kJ Which of the following will increase the quantity of ClF 3 in the equilibrium mixture of Cl 2 , F 2 and ClF 3 ?

Increasing the volume of the container.

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A buffer solution is prepared by mixing $' a'$ moles of ${CH}_{3} COONa$ and $' b'$ moles of ${CH}_{3} COOH$ such that $(a + b) = 1,$ into water to make $1 L$ buffer solution. If the instantaneous (differential) buffer capacity of this buffer solution is plotted against moles of salt ${CH}_{3} COONa$ $(a),$ then the plot obtained will be (to the scale) approximately:

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Important Questions on Equilibrium

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Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-2>Q 183

An acid-base indicator which is a weak acid has a

{pK}_{In}

value

= 5.45

. At what concentration ratio of sodium acetate to acetic acid would the indicator show a colour halfway between those of its acid and conjugate base forms? [

{pK}_{a}

of acetic acid

= 4.75, \log 2 = 0.3

]

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Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-2>Q 184

If the indicator is a weak acid with

K_{In} = 4 \times 10^{- 4},

for indication of equivalence point of which of the following neutralisation(s), would the indicator be useful?

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Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-3>Q 1

The incorrect expression among the following is

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Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-3>Q 2

For the chemical reaction,

3 X (g) + Y (g) ⇌ X_{3} Y (g)

the amount of

X_{3} Y

at equilibrium is affected by:

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Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-3>Q 3

For the reversible reaction,

N_{2} (g) + 3 H_{2} (g) ⇌ 2 {NH}_{3} (g)

500 ° C

, the value of

K_{p}

1.44 \times 10^{- 5}

when partial pressure is measured in atmospheres. The corresponding value of

K_{c}

, with concentration in

mole {litre}^{- 1}

, is

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Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-3>Q 4

At constant temperature, the equilibrium constant ( $K_{p}$ ) for the decomposition reaction: $N_{2} O_{4} ⇌ 2 {NO}_{2},$ is expressed by $K_{p} = \frac{4 x^{2} P}{(1 - x^{2})}$ , where $P$ is the pressure and $x$ is the extent of decomposition. Which of the following statements is true?

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Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-3>Q 5

Consider the following equilibrium in a closed container,

N_{2} O_{4} (g) ⇌ 2 {NO}_{2} (g)

. At a fixed temperature, the volume of the reaction container is halved. For this change which of the following statements holds true regarding the equilibrium constant

(K_{p})

and degree of dissociation

(α)

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Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-3>Q 6

The thermal dissociation equilibrium of

{CaCO}_{3} (s)

is studied under different conditions.

{CaCO}_{3} (s) ⇌ CaO (s) + {CO}_{2} (g)

For this equilibrium, the correct statement(s) is (are) :

Important Questions on Equilibrium

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