Home
Class 12
CHEMISTRY
For the solution of the gases W, X, Y ...

For the solution of the gases ` W, X, Y ` and z in water at 298 K , the Henrys law constants (`K _ H `) are 0.5, 2, 35 and 40 kbar, respectively. The correct plot for the given data is :

A

B

(2)

C

(3)

D

(4)

Text Solution

AI Generated Solution

To solve the problem, we need to analyze the relationship between the partial pressure of the gases and their mole fractions in water using Henry's Law. Here is a step-by-step solution: ### Step 1: Understand Henry's Law Henry's Law states that the partial pressure of a gas in a solution is directly proportional to its mole fraction in that solution. Mathematically, it can be expressed as: \[ P = K_H \cdot x \] where: - \( P \) is the partial pressure of the gas, - \( K_H \) is the Henry's Law constant, ...
Promotional Banner

Topper's Solved these Questions

  • JEE Main Revision Test-9 | JEE-2020

    VMC MODULES ENGLISH|Exercise CHEMISTRY SECTION 2|5 Videos

  • JEE Main Revision Test-6 | JEE-2020

    VMC MODULES ENGLISH|Exercise CHEMISTRY|25 Videos

  • JEE MAIN REVISON TEST-23

    VMC MODULES ENGLISH|Exercise CHEMISTRY (SECTION 1)|25 Videos

Similar Questions

Explore conceptually related problems

For the solution of the gases W, X, Y and Z in water at 298 K , the Henry's law constants ( K _ H ) are 0.5, 2, 35 and 40 kbar, respectively. The correct plot for the given data is :

For the solution of the gases w,x,y and z in water at 298 K the Henry's law constant (K_(H)) are 0.5,2,35 and 40 k bar ,respectively. The correct plot for the given data is :

The air is a mixture of a number of gases. The maojr components are oxygen and nitrogen with approximate proportion of 20% is to 79% by volume at 298 K. The water is in equilibrium with air at a pressure of 10 atm. At 298 K if the Henry's law constants for oxygen and nitrogen at 298 K are 3.30xx10^(7) mm and 6.51xx10^(7) mm respectively, calculate the composition of these gases in water.

Four gases alpha, beta, gamma and delta have K_H values 50kbar, 20 kbar, 2xx10^(-3) kbar and 2 kbar respectively. then ?

Henry's law constant of CO_2 in water at 298K is 5/3K bar. IF pressure of CO_2 is 0.01 bar, find its mole fraction.

The Henry's law constant for CO_(2) in water at 298 K is 1.67 kbar. Calculate the solubility of CO_(2) at 298 K when the pressure of CO_(2) is one bar.

For a solution of acetone in chloroform, Henry's law constant is 150 torr at a temperature of 300 K. (a) Calculate the vapour pressure of acetone when the mole fraction is 0.12. (b) Assuming that Henry's law is applicable over sufficient range of composition to make the calculation valid, calculate the composition at which Henry's law pressure of chloroform is equal to Henry's law pressure of acetone at 300 K. (Henry's law constant for chloroform is 175 torr.)

1 kg of water under a nitrogen pressure of 1 atmosphere dissolves 0.02 gm of nitrogen at 293 K. Calculate Henry' s law constant :

The Henry's law constant for the solubility of N_(2) gas in water at 298 K is 1.0 xx 10^(5) atm . The mole fraction of N_(2) in air is 0.8 . The number of moles of N_(2) from air dissolved in 10 moles of water at 298 K and 5 atm . Pressure is:

When a gas is bubbled through water at 298 K, a very dilute solution of gas is obtained . Henry's law constant for the gas is 100 kbar. If gas exerts a pressure of 1 bar, the number of moles of gas dissolved in 1 litre of water is