Henry's Law Gas Solubility Quiz

1. What are some important applications of Henry's law?

In packing soda cans

In respiration

In the production of carbonated beverages

All of the above

Henry's law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. This law has various applications. In packing soda cans, Henry's law is utilized to determine the appropriate amount of carbon dioxide to be dissolved in the liquid to achieve the desired carbonation. In respiration, Henry's law explains how oxygen is absorbed from the air into the bloodstream. In the production of carbonated beverages, Henry's law is used to control the amount of carbon dioxide dissolved in the beverage. Therefore, all of the given applications are important uses of Henry's law.

Explanation

Henry's law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. This law has various applications. In packing soda cans, Henry's law is utilized to determine the appropriate amount of carbon dioxide to be dissolved in the liquid to achieve the desired carbonation. In respiration, Henry's law explains how oxygen is absorbed from the air into the bloodstream. In the production of carbonated beverages, Henry's law is used to control the amount of carbon dioxide dissolved in the beverage. Therefore, all of the given applications are important uses of Henry's law.

2. What does k_H denote in Henry's law?

Partial pressure

Henry’s law temperature constant

Henry’s law constant

All of the above

kH denotes Henry's law constant. This constant represents the proportionality between the concentration of a gas in a liquid and the partial pressure of that gas above the liquid. According to Henry's law, the concentration of a gas in a liquid is directly proportional to its partial pressure. Therefore, kH is used to calculate the concentration of a gas in a liquid based on its partial pressure, or vice versa.

Explanation

kH denotes Henry's law constant. This constant represents the proportionality between the concentration of a gas in a liquid and the partial pressure of that gas above the liquid. According to Henry's law, the concentration of a gas in a liquid is directly proportional to its partial pressure. Therefore, kH is used to calculate the concentration of a gas in a liquid based on its partial pressure, or vice versa.

3. According to Henry's law, the partial pressure of the gas (Pgas) is directly proportional to __________ of gas in the dissolved state.

Atomic mass

Molar mass

The mole fraction

Molecular mass

According to Henry's law, the partial pressure of a gas in a solution is directly proportional to the mole fraction of the gas in the dissolved state. This means that as the mole fraction of the gas increases, the partial pressure of the gas also increases. The mole fraction is a measure of the amount of a particular gas compared to the total amount of all gases in the solution. Therefore, the correct answer is "the mole fraction".

Explanation

According to Henry's law, the partial pressure of a gas in a solution is directly proportional to the mole fraction of the gas in the dissolved state. This means that as the mole fraction of the gas increases, the partial pressure of the gas also increases. The mole fraction is a measure of the amount of a particular gas compared to the total amount of all gases in the solution. Therefore, the correct answer is "the mole fraction".

4. What is the unit of Henry's Law constant?

Ml L–1 bar–1

Gas/ L–1 bar–1

Mol L–1 bar–1

Mol KL–1 bar–1

The unit of Henry's Law constant is mol L-1 bar-1.

Explanation

The unit of Henry's Law constant is mol L-1 bar-1.

5. What is the formula of Henry's law?

P ∝ C (or) P = kH.P

P ∝ C (or) P = kH.C

P ∝ C (or) P = kH/C

None of the above

Henry's law states that the pressure of a gas above a liquid is directly proportional to the concentration of the gas in the liquid. Mathematically, this can be represented as P ∝ C (or) P = kH.C, where P is the pressure of the gas, C is the concentration of the gas in the liquid, and kH is the proportionality constant. This formula shows the relationship between pressure and concentration according to Henry's law.

Explanation

Henry's law states that the pressure of a gas above a liquid is directly proportional to the concentration of the gas in the liquid. Mathematically, this can be represented as P ∝ C (or) P = kH.C, where P is the pressure of the gas, C is the concentration of the gas in the liquid, and kH is the proportionality constant. This formula shows the relationship between pressure and concentration according to Henry's law.

6. The value of Henry's law constant of a gas is dependent on which factors?

The nature of the solvent

The nature of the gas

Temperature & pressure

All of the above

The value of Henry's law constant of a gas is dependent on the nature of the solvent, the nature of the gas, as well as temperature and pressure. The nature of the solvent affects the solubility of the gas, while the nature of the gas determines its ability to dissolve in the solvent. Temperature and pressure also play a crucial role in determining the solubility of the gas in the solvent. Therefore, all of these factors contribute to the value of Henry's law constant.

Explanation

The value of Henry's law constant of a gas is dependent on the nature of the solvent, the nature of the gas, as well as temperature and pressure. The nature of the solvent affects the solubility of the gas, while the nature of the gas determines its ability to dissolve in the solvent. Temperature and pressure also play a crucial role in determining the solubility of the gas in the solvent. Therefore, all of these factors contribute to the value of Henry's law constant.

7. When is Henry's law applicable?

At a constant temperature

At a variable osmotic pressure

Both A and B

None of the above

Henry's law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid, at a constant temperature. This means that as the pressure of the gas increases, more gas molecules will dissolve in the liquid. However, Henry's law does not depend on the osmotic pressure, which is the pressure required to prevent the flow of solvent into a solution through a semipermeable membrane. Therefore, the correct answer is "at a constant temperature".

Explanation

Henry's law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid, at a constant temperature. This means that as the pressure of the gas increases, more gas molecules will dissolve in the liquid. However, Henry's law does not depend on the osmotic pressure, which is the pressure required to prevent the flow of solvent into a solution through a semipermeable membrane. Therefore, the correct answer is "at a constant temperature".

8. The limitation(s) of Henry's law is/are:

If gases are placed under high pressure, it doesn't work.

It is only applicable when the system molecules are in an equilibrium state.

Both A and B

None of the above

The correct answer is "Both A and B". Henry's law is limited in two ways. Firstly, it does not work when gases are placed under high pressure. This is because at high pressures, the gas molecules are forced closer together, which can cause them to interact and deviate from the ideal behavior assumed by Henry's law. Secondly, Henry's law is only applicable when the system molecules are in an equilibrium state. This means that the system must be at a steady state where the rate of gas molecules entering and leaving the liquid phase is equal.

Explanation

The correct answer is "Both A and B". Henry's law is limited in two ways. Firstly, it does not work when gases are placed under high pressure. This is because at high pressures, the gas molecules are forced closer together, which can cause them to interact and deviate from the ideal behavior assumed by Henry's law. Secondly, Henry's law is only applicable when the system molecules are in an equilibrium state. This means that the system must be at a steady state where the rate of gas molecules entering and leaving the liquid phase is equal.

9. Which gases do not obey Henry's law?

NH3

CO2

HCl

All of the above

Henry's law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. However, NH3 (ammonia), CO2 (carbon dioxide), and HCl (hydrochloric acid) do not obey Henry's law. These gases exhibit deviations from the ideal behavior due to factors such as hydrogen bonding, ionization, or molecular interactions. Therefore, the correct answer is "All of the above" as all the mentioned gases do not follow Henry's law.

Explanation

Henry's law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. However, NH3 (ammonia), CO2 (carbon dioxide), and HCl (hydrochloric acid) do not obey Henry's law. These gases exhibit deviations from the ideal behavior due to factors such as hydrogen bonding, ionization, or molecular interactions. Therefore, the correct answer is "All of the above" as all the mentioned gases do not follow Henry's law.

10. What is the solubility of gaseous oxygen in water at a temperature of 293 K when the partial pressure exerted by O₂ is 1 bar? (Given: k_H for O₂ 34840 bar.L.mol-1)

3.87*10-4 M

3.87*10-5 M

2.87*10-4 M

2.87*10-5 M

The solubility of gaseous oxygen in water at a temperature of 293 K when the partial pressure exerted by O2 is 1 bar is 2.87*10-5 M. This is determined using Henry's Law, which states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. The proportionality constant, known as the Henry's Law constant (kH), is given as 34840 bar.L.mol-1 for O2. By substituting the given values into the equation, we can calculate the solubility of O2 in water.

Explanation

The solubility of gaseous oxygen in water at a temperature of 293 K when the partial pressure exerted by O2 is 1 bar is 2.87*10-5 M. This is determined using Henry's Law, which states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. The proportionality constant, known as the Henry's Law constant (kH), is given as 34840 bar.L.mol-1 for O2. By substituting the given values into the equation, we can calculate the solubility of O2 in water.