What gases are not able to be collected over water due to their solubility?

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SUMMARY

In a laboratory setup for collecting gases via water displacement, ammonia (NH3) cannot be collected over water due to its high solubility. The discussion identifies that carbon dioxide (CO2), nitric oxide (NO), and oxygen (O2) can be collected, while methane (CH4) is insoluble in water. The solubility of gases is influenced by their polarity and the potential for hydrogen bonding with water molecules, with NH3 exhibiting the strongest interactions due to its polarity and ability to form hydrogen bonds.

PREREQUISITES
  • Understanding of gas solubility principles
  • Knowledge of intermolecular forces, particularly hydrogen bonding
  • Familiarity with polar and nonpolar molecules
  • Basic laboratory techniques for gas collection
NEXT STEPS
  • Research the solubility of gases in water and the factors affecting it
  • Study the concept of hydrogen bonding in molecular interactions
  • Explore the properties of polar vs. nonpolar molecules
  • Learn about laboratory techniques for gas collection, including water displacement methods
USEFUL FOR

Chemistry students, laboratory technicians, and educators involved in gas solubility and collection methods will benefit from this discussion.

TT0
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Homework Statement


In a proper laboratory setup for collecting a gas by water displacement, which of these gases could NOT be collected over H2O because of its solubility?

A. CO2
B. NO
C. O2
D. NH3
E. CH4

Homework Equations


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The Attempt at a Solution


I know E is definitely wrong because its organic so its insoluble in water. Water is polar so polar gases should be soluble in it, B and D are polar. Also carbon dioxide should be soluble in water because CO2 + H2O -> H2CO3. This gives me 3 gases that will be be able to be collected over water but there should only be one.

Thanks!
 
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All gasses are soluble to some extent in liquid water, but one of these molecules in particular will have very strong interactions with water molecules. Think of the potential intermolecular interactions each of these molecules would form with water.
 
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Both B and D are polar but B has less difference in electronegativity so D would be the most polar so most soluble, right?
 
Again: think of intermolecular interactions. Just being polar is not everything.
 
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Hydrogen bonding!
 
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