A 0.316 mol sample of nitrogen gas, N2(g), is placed in a 4.00 L container at 315K
1 answer:
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At a particular temperature, the solubility of He in water is 0.060 M when the partial pressure is 0.90 atm. 2.27 atm is the partial pressure of Kr would give a solubility of 0.150 M.
<h3>What is Henry's Law ?</h3>- According to Henry's law, the weight of a gas dissolved by a liquid is proportional to the pressure of the gas onto the liquid.
- With very few exceptions, a solute molecule in an extremely diluted solution will only have solvent molecules as its close neighbors. This means that the likelihood that a specific solute molecule will escape into the gas phase is predicted to be independent of the total concentration of solute molecules.
Solution:
The solubility of gas is directly proportional to partial pressure. It is expressed as:
S =
where, S = Solubility of gas
= Henry's Law constant
= Partial pressure of gas
Now, put the values in above expression we get
0.060M = × 0.9 atm
= = 0.066 M/atm
Now we have to find the partial pressure of He
0.150 M = 0.066 M/atm ×
= 2.27 atm
Learn more about the Henry's Law : brainly.com/question/23204201
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