Home
Class 12
CHEMISTRY
Henry's law constant for oxygen and nitr...

Henry's law constant for oxygen and nitrogen dissolved in water at `298` K are `2.0 xx 10^(9)` Pa and `5.0 xx 10^(9)` Pa , respectively . A sample of water at a temperature just above `273` K was equilibrated with air (`20%` oxygen and `80%` nitrogen ) at `1` atm. The dissolved gas was separated from a sample of this water and the dried. Determine the composition of this gas.

Text Solution

AI Generated Solution

To determine the composition of the gas dissolved in water after equilibrating with air, we will follow these steps: ### Step 1: Write down the given data - Henry's law constant for Oxygen, \( K_H(O_2) = 2.0 \times 10^9 \, \text{Pa} \) - Henry's law constant for Nitrogen, \( K_H(N_2) = 5.0 \times 10^9 \, \text{Pa} \) - Composition of air: 20% Oxygen and 80% Nitrogen - Total pressure of air, \( P = 1 \, \text{atm} \) ...
Promotional Banner

Topper's Solved these Questions

  • SOLUTIONS

    CENGAGE CHEMISTRY ENGLISH|Exercise Solved Examples|40 Videos

  • SOLUTIONS

    CENGAGE CHEMISTRY ENGLISH|Exercise Exercises (Linked Comprehension)|58 Videos

  • SOLID STATE

    CENGAGE CHEMISTRY ENGLISH|Exercise Ex 1.2 (Objective)|9 Videos

  • SURFACE CHEMISTRY

    CENGAGE CHEMISTRY ENGLISH|Exercise Archives Subjective|2 Videos

Similar Questions

Explore conceptually related problems

Henry law constant for oxygen dissolved in water is 4.34 xx 10^(4) atm at 25^(@) C . If the partial pressure of oxygen in air is 0.4 atm.Calculate the concentration ( in moles per litre) of the dissolved oxygen in equilbrium with air at 25^@C .

At a certain temperature , K_(w) of water is 9.0 xx 10^(-14) . The pH of water at this temperature is

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

Calculate the amount of NH_(4)C1 required to dissolve in 500mL of water to have a pH = 4.5, K_(b) = 2.0 xx 10^(-5) .

Calculate the amount of NH_(4)Cl required to dissolve in 500mL of water to have a pH = 4.5, K_(b) = 2.0 xx 10^(-5) .

The Henry's law constant for the solubility of N_(2) gas in water at 298K 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 298K and 5 atm pressure is

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:

henry's law constant for CO_(2) in water is 2.5xx10^(8) Pa at 298K calcualte mmole of CO_(2) dissolbed in 144 g water at 2.5 atm pressure at 298K. [take 1 atm =10^(6)(N)/(m^(2)) or Pa]

Henry's law constant for CO_(2) in water is 1.67xx10^(8) Pa at 298 K . Calculate the quantity of CO_(2) in 500mL of soda water when packed under 2.5atm CO_(2) pressure at 298 K .

Henry's law constant for CO_(2) in water is 1.67xx10^(8) Pa at 298 K . Calculate the quantity of CO_(2) in 500mL of soda water when packed under 2.5 atm CO_(2) pressure at 298 K .