Henry's Law

Q. The partial pressure of hydrogen in a flask containing $2g$ of hydrogen and $32g$ of sulphur dioxide is:

1. $1/{16}^{th}$ of the total pressure
2. $1/9^{th}$ of the total pressure
3. $2/3^{rd}$ of the total pressure
4. $1/8^{th}$ of the total pressure

Q.

A binary liquid solution is prepared by mixing n-heptane and ethanol. Which one of the following statements is correct regarding the behaviour of the solution ?

1. The solution is non-ideal, showing positive deviation form Raoult's Law

2. The solution is non-ideal, showing negative deviation from Raoult's Law

3. n-heptane shows positive deviation while ethanol shows negative deviation from Raoult's Law

4. The solution formed is an ideal solution

Q. The partial pressure of ethane over a saturated solution containing 0.0656g of ethane is 1 bar. If the solution contains 0.0500g of ethane, then what should be the partial pressure of the gas?

1. 0.762 bar
   
2. 0.755 bar
   
3. 0.764 bar
   
4. 0.772 bar

Q. Which of the following is true regarding Henry's Law constant for different aqueous solutions of $C{O}_2\left(g\right)$ and $O_2\left(g\right)$ at a given temperature?
(Assume both the gases have same partial pressure)

1. $K_H\left(C{O}_2\right)=K_H\left(O_2\right)$
2. Cannot be predicted
3. $K_H\left(C{O}_2\right)>K_H\left(O_2\right)$
4. $K_H\left(C{O}_2\right)<K_H\left(O_2\right)$

Q. " 0.003 moles of a gas are dissolved in 900 g of water under a pressure of 1 atm . Also, 0.006 moles of same gas get dissolved in 900 g of water under a pressure of 2 atm"
Considering the above statement to be true, it illustrates the applicability of :

1. Dalton's law of partial pressure
2. Henry's Law
3. First Law of thermodyanics
4. Graham's Law of diffusion

Q. For a given gas , predict the relationship between $K_{H_1},K_{H_2},K_{H_3}$ from the given graph.
(where $K_H$ is henry's law constant)

1. $K_{H_1}>K_{H_2}>K_{H_3}$
2. $K_{H_1}<K_{H_2}<K_{H_3}$
3. $K_{H_1}<K_{H_2}>K_{H_3}$
4. $K_{H_1}=K_{H_2}=K_{H_3}$

Q. Consider the following statements:
Statement I:
The tanks used by scuba divers are filled with air diluted with helium.
Statement II:
For scuba divers , increased pressure increases the solubility of atmospheric gases in blood, thus more $N_2$ is dissolved in blood underwater at high pressure

1. Both the statements are correct.
2. Both the statements are incorrect.
3. Statement I is correct whereas statement II is incorrect
4. Statement I is incorrect whereas statement II is correct

Q. The mixture which shows positive deviation from Raoult’s law is

1. Chloroethane + bromoethane
2. Ethanol + acetone
3. Benzene + toluene
4. Acetone + chloroform

Q. $CO\left(g\right)$ is dissolved in $H_{2}O$ at ${25}^{o}C$ and 0.010 atm. Henry's law constant for this system is $5.80\times {10}^4$ atm. Thus, mole fraction of $CO\left(g\right)$ is

1. $8.28\times {10}^{-7}$
2. $0.01$
3. $0.99$
4. $1.72\times {10}^{-7}$

Q. $H_{2}S$ is a toxic gas with rotten egg smell is used for the qualitative analysis. If the solubility of $H_{2}S$ in water at STP is $0.2m$, calculate Henry's constant.

Q.

Two non-reactive monoatomic ideal gases have their atomic masses in the ratio $2:3$. The ratio of their partial pressure, when enclosed in a vessel kept at a constant temperature is $4:3$. The ratio of their densities is

Q. Aquatic species feel more comfortable in winter than in summer because -

1. $\%$ of $O_2$ in air decreases in summer due to high temperature
2. Atmospheric pressure decreases in summer leading to reduced solubility of gases in water
3. Solubility of gases in water decreases as the temperature increases due to increased Henry’s constant
4. Aquatic species feel skin burn due to increased temperature of the water.

Q. $H_{2}S$ , a toxic gas with a rotten egg like smell is used for the qualitative analysis. If the solubility of $H_{2}S$ in the water at STP is $0.195m$, then Henry's law constant (in atm) is nearly :

1. 2890.4
2. 145.2
3. 285
4. 28.94

Q. $CO\left(g\right)$ is dissolved in $H_{2}O$ at ${25}^{o}C$ and 0.010 atm. Henry's law constant for this system is $5.80\times {10}^4$ atm. Thus, mole fraction of $CO\left(g\right)$ is

Q. Choose the correct statment(s) for Henry's law to be valid :

1. Pressure of the gas should not be too high.
2. Pressure of the gas should be high.
3. Gas should not undergo any reaction with the solvent and dissociation ​or association in the solvent.
4. Temperatuure of the gas should not be too low or high.

Q. In which of the following conditions , Henry's law is applicable?

1. When temperature of the gas is too low
2. Gas undergoes endothermic reaction with the solvent.
3. Gas should not undergo any association/dissociation with the solvent
4. Gas undergoes exothermic reaction with the solvent.

Q.

A mixture of white bauxite powder and coke is heated in nitrogen gas very strongly . The products are

1. Al₂O₃ , C₂N₂

2. Al (NO₃)₃ , CO

3. AlN , CO, Si Vapour

4. Al₂ (CO₃)₃, N₂O

Q. Ratio of Henry’s constant, $K_H$ of two inert gases A $\&$ B is 2 at a given temperature. A mixture containing 4 moles of gas A and 8 moles of gas B is bubbled through water covered from top and solution is allowed to attain equilibrium. Assuming the absence of any other gases, what will be the ratio of mole fractions of gases in the solution.

1. 1:1
2. 8:9
3. 7:8
4. 1:2

Q. What is the reason of forming gas bubbles when a coke bottle is opened?

1. Increase in pressure
2. Decrease in pressure
3. Coke reacts with gases in air
4. None of the above

Q. The value of Henry’s law constant does not change irrespective of the gas.

1. True
2. False

Q. If $He\left(g\right)$ is bubbled through the water at $298K$, how many millimoles of $He\left(g\right)$ would dissolve in one litre of water?
Assume that $He\left(g\right)$ exerts a partial pressure of $0.5bar$
Take Henry's Law constant for $He\left(g\right)$ at $298K$ as $145kBar$

Q.

The Henry's law constant for the solubility of N₂ gas in water at 298K is 1.0 x 10⁵ atm. The mole fraction of N₂ is 0.8. The number of moles of N₂ from air dissolved in 10 moles of water at 298K and 5 atm pressure is

1. 4 x 10^-4

2. 4 x 10^-5

3. 5 x 10^-4

4. 4 x 10^-6

Q. Which of the following mathematical expression correctly represents the Henry's law?
(Where $p$ is the partial pressure of gas over the solution, $K_H$ is Henry’s law constant and $\chi$ is mole fraction of the gas in the solution.)

1. $p^2\times \chi =K_H$
2. $\chi =\frac{p}{K_H}$
   
3. $p\times {\chi }^2=K_H$
4. None of the above

Q. Ratio of Henry’s constant, $K_H$ of two inert gases A $\&$ B is 2 at a given temperature. A mixture containing 4 moles of gas A and 8 moles of gas B is bubbled through water covered from top and solution is allowed to attain equilibrium. Assuming the absence of any other gases, what will be the ratio of mole fractions of gases in the solution.

1. 1:1
2. 8:9
3. 7:8
4. 1:2