Learning Path
Question & Answer1
Understand Question2
Review Options3
Learn Explanation4
Explore TopicChoose the Best Answer
A
The pressure of the gas decreases.
B
The gas molecules gain mass.
C
The gas is being compressed.
D
The gas molecules lose energy.
Understanding the Answer
Let's break down why this is correct
Answer
According to the Ideal Gas Law, \(PV = nRT\); if the volume \(V\) rises while the amount of gas \(n\), the temperature \(T\), and the constant \(R\) stay the same, the product \(PV\) must stay constant, so the pressure \(P\) must fall. This means the gas expands because the surrounding pressure has decreased, allowing it to occupy a larger space. For example, a helium balloon rises and expands when the atmospheric pressure drops at higher altitudes. Thus, the most likely cause of the volume increase is a reduction in pressure.
Detailed Explanation
When the size of the container grows and the gas stays the same amount and temperature, the pressure must drop to keep the balance of PV = nRT. Other options are incorrect because Adding more mass would mean adding more gas, which would increase pressure or volume, not just change volume alone; Compression squeezes the gas, which actually reduces volume.
Key Concepts
Ideal Gas Law
Pressure-Volume Relationship
Gas Behavior
Topic
Ideal Gas Law
Difficulty
medium level question
Cognitive Level
understand
Practice Similar Questions
Test your understanding with related questions
1
Question 1If the volume of a gas increases while the temperature remains constant, what happens to the pressure of the gas according to Boyle's Law?
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Practice
2
Question 2If the pressure of a gas increases while the temperature remains constant, what happens to the volume according to the Ideal Gas Law?
hardPhysics
Practice
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