Henry’s law is a gas law which states that at the amount of gas that is dissolved in a liquid is directly proportional to the partial pressure of that gas above the liquid when the temperature is kept constant. The constant of proportionality for this relationship is called Henry’s law constant (usually denoted by ‘k H ‘). The mathematical formula of Henry’s law is given by: P ∝ C ( or ) P = k H × C . Where, ‘P’ denotes the partial pressure of the gas in the atmosphere above the liquid. ‘C’ denotes the concentration of the dissolved gas. ‘k H ’ is the Henry’s law constant of the gas.

For the reaction: 2 NO 2 g ⇌ 2 NO g + O 2 g , K c = 1 .8 × 10 - 6 at 184 o C , R = 0 .0831 J / molK When K p and K c are compared at 184 o C. It is found that

Whether K p is greater than, less than or equal to K c depends upon the total gas pressure.

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Important Questions on Equilibrium

EASY

Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

A solid $XY$ kept in an evacuated sealed container undergoes decomposition to form a mixture of gases $X and Y$ at temperature $T$ .

The equilibrium pressure is $10 bar$ in this vessel. $K_{p}$ for this reaction is?

HARD

Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

$A (g) ⇌ 2 B (g) + C (g)$

For the given reaction, if the initial pressure is $450 mmHg$ and the pressure at time $t$ is $720 mmHg$ at a constant temperature $T$ and constant volume $V$ . The fraction of $A (g)$ decomposed under these conditions is $x \times 10^{- 1}$ . The value of $x$ is (nearest integer)

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Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

State Henry's law.

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For the reaction:

2 {NO}_{2 (g)} ⇌ 2 {NO}_{(g)} + O_{2 (g)},

(K_{c} = 1 .8 \times 10^{- 6} at 184^{o} C), (R = 0 .0831 J / molK)

When

K_{p}

and

K_{c}

are compared at

184^{o} C.

It is found that

EASY

Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

If the equilibrium constant for

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

is K, the equilibrium constant for

\frac{1}{2} N_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ N O (g)

will be:

EASY

Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

Consider the following reversible chemical reactions:

A_{2} (g) + B_{2} (g) \overset{k_{1}}{⇌} 2 A B (g)

.....(1)

6 A B (g) \overset{k_{2}}{⇌} 3 A_{2} (g) + 3 B_{2} (g)

.....(2)

The relation between

K_{1}

and

K_{2}

is:

HARD

Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

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

EASY

Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

List any four important characteristics of a chemical equilibrium.

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Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

Among the following points indicated on the graph, which one represents equilibrium?

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Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

Define 'homogeneous equilibria and heterogeneous equilibria'. Give three examples of each of them.

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Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

For the synthesis of ammonia by the reaction

N_{2} + 3 H_{2} ⇌ 2 {NH}_{3}

in the Haber's process, the attainment of equilibrium is correctly predicted by the curve

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Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

What do you understand by dynamic nature of chemical equilibrium? Give one experiment to prove that equilibrium is dynamic in nature.

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Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

Which of the following statements is correct?

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Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

What do you understand by chemical equilibrium? Explain with one suitable example.

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Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

The strongest conjugate base is:

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Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

Based upon the following hypothetical equilibria at

273 K

{XCl}_{2} \cdot 6 H_{2} O_{(s)} ⇌ {XCl}_{2} \cdot 2 H_{2} O_{(S)} + 4 H_{2} O_{(v)} {; K}_{p} {= 8.1 × 10}^{-11} {atm}^{4}

Y_{2} {HPO}_{4} \cdot 12 H_{2} O_{(s)} ⇌ Y_{2} {HPO}_{4} \cdot 7 H_{2} O_{(v)} + 5 H_{2} O_{(g)} {; K}_{p} {= 3.2 × 10}^{-9} {atm}^{5}

Z_{2} {SO}_{4} \cdot 10 H_{2} O_{(s)} ⇌ Z_{2} {SO}_{4 (s)} + 10 H_{2} O_{(v)} {; K}_{p} {= 1.0 × 10}^{-30} {atm}^{10}

Which is the most effective dehydrating agent at

273 K

? (Aqueous tension at

273 K

6.0 \times 10^{- 3}

atm)

EASY

Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

A compound having the formula

{NH}_{2} {CH}_{2} COOH

will behave

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Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

Which of the following is a reversible reaction?

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Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

In the reaction ${PCl}_{5} (g) ⇌ {PCl}_{3} (g) + {Cl}_{2} (g)$ , which of the graphs is/are correct?

Question Image

EASY

Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

The

{pK}_{a}

of acetyl salicylic acid (aspirin) is 3.5. The pH of gastric juice in human stomach is about 2-3 and pH in the small intestine is about 8. Aspirin will be:

Which concept in economics explains the relationship between price and quantity demanded?

Important Questions on Equilibrium

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