1a. Consider a mixture of water and air in a sealed container. Which of the foll
ID: 553154 • Letter: 1
Question
1a. Consider a mixture of water and air in a sealed container. Which of the following changes will increase the amount of nitrogen dissolved in the water? [Select all that apply.]
- The pressure in the container is decreased by increasing its volume.
- Extra oxygen is added to the container, increasing the total pressure inside the container.
- The air in the container is replaced with pure nitrogen, but the total pressure inside the container is unchanged.
- Extra nitrogen is added to the container, increasing the total pressure inside the container.
- The pressure in the container is increased by decreasing its volume.
1b. With all other conditions being equal, which of the following gases would you expect to have a larger Henry's law constant than N2? [Select all that apply.]
- Ne
- He
- Xe
- NH3
Explanation / Answer
Ans
1a :Three choices are correct :
The air in the container is replaced with pure nitrogen , but the total pressure inside the container is unchanged.
Extra nitrogen is added to the container , increasing the total pressure inside the container.
The pressure in the container is increased by decreasing its volume.
The amount of gases dissolved in water is directly proportional to the amount of partial pressure of that gas. If air is replaced by the pure nitrogen , more concentration of it will increase its solubility in water.
Ans 1b) NH3
Henry's law relates the partila pressure of the gas to its solubility in the water. The constant is uniques for each gas , that determines its solubility.
The henry's constant for ammonia is more than that of N2.
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