Which of the following is NOT true about gases?

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SUMMARY

The discussion centers on the properties of gases, specifically addressing the statement that "the volume a gas occupies is directly proportional to its molecular weight," which is identified as false. Participants debate the interpretation of the statement "gases can expand without limit," clarifying that while gases can expand indefinitely in an open environment, their expansion is constrained within a closed container. The conversation highlights the importance of context in physics and chemistry exam questions, emphasizing the need for clarity to avoid ambiguity.

PREREQUISITES
  • Understanding of gas laws, including Boyle's Law and Charles's Law.
  • Familiarity with Standard Temperature and Pressure (STP) conditions.
  • Knowledge of molecular weight and its implications on gas behavior.
  • Basic principles of thermodynamics related to gas expansion.
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  • Research the Ideal Gas Law and its applications in real-world scenarios.
  • Study the differences between ideal gases and real gases, focusing on deviations at high pressures and low temperatures.
  • Explore the concept of gas density and how it changes with pressure and temperature.
  • Learn about the implications of gas expansion in closed versus open systems.
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Students of chemistry and physics, educators preparing exam materials, and anyone interested in the fundamental properties and behaviors of gases.

ace123
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Which of the following is NOT true about
gases?
1. The volume a gas occupies is directly
proportional to its molecular weight.
2. The gas is at STP if it is at 273 K and 1
atm.
3. Gases exert pressure on their surround-
ings.
4. Gases can expand without limit.
5. The density of a gas can be increased by applying increased pressure.

Now I know that 1 is wrong. But I was thinking shouldn't 4 technically be wrong because the gases only expand to fill the container they are in. In other words a gas in bottle can't expand without limit. Is this reasoning correct in any way?
 
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ace123 said:
But I was thinking shouldn't 4 technically be wrong because the gases only expand to fill the container they are in. In other words a gas in bottle can't expand without limit. Is this reasoning correct in any way?
If the system is a closed vessel you are correct. If there is no container, they can expand without limit.
 
Since it didn't state anything about that. So therefore I have an argument?
 
It didn't say there was a container!
 
It didn't say that it wasn't in a container. SO...?
 
Unfortunately there are two sides to physics.
1, Understanding the behaviour of the real world - and what maths to apply where
2, Understanding what exam questions mean.
 
Lol. Good thing chem isn't physics. Therefore exam questions shouldn't be ambiguous.
 

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