Gas Law's Unit Assessment

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Last updated 12:05 PM on 9/19/25
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15 Terms

1
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Kinetic Molecular Theory

A theory that applies to the Ideal Gas Law and that explains the states of matter and is based on the idea that matter is composed of tiny particles that are always in motion; explains observable properties and behaviors in solids, liquids, and gases

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Why is KMT important?

It explains gas laws, it predicts gases behaviors, it provides a model for understanding motion of molecules, and its real-world applications

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What are the 3 assumptions of KMT?

  1. Gas atoms/molecules move rapidly and randomly

  2. Gas particles are really spaced out

  3. Gas particles bounce off each other without losing energy


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Gas atoms/molecules move rapidly and randomly

The fast motion of gas particles is random and give them a relatively large amount of kinetic energy; at higher temperatures, the gas particles have even more energy and move even faster

Ex: Gas leaking from a stove, which is why you can smell it so quickly

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Gas particles are really spaced out

The size of the particles doesn’t matter, all gases are treated the same meaning you can compress gases; The particles of gas may either be atoms or molecules

Ex: Squeezing a balloon; under normal conditions the balloon is flexible and can expand or contract

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Gas particles bounce off each other without losing energy

They bounce off each other without losing energy. Although their direction or speed may change after collisions, the total kinetic energy of the gas remains constant. This allows gas particles to keep moving rapidly and randomly, maintaining the gas’s temperature and pressure without slowing down or settling

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Kinetic Energy

The energy an object possesses because of its motion

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Ideal Gas

An imaginary gas whose behaviour perfectly fits the assumptions of KMT

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Real Gases

Gases that don’t follow KMT assumptions

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Gay-Lussac Law

  • At constant volume (v) and moles (n); Pressure (P) & Temperature (T) are directly related

  • Equation: P1 / T1 = P2 / T2

  • Acronym: GPT


<ul><li><p>At constant volume (v) and moles (n); Pressure (P) &amp; Temperature (T) are directly related</p></li><li><p>Equation: P<sub>1</sub> / T<sub>1 </sub>= P<sub>2 </sub>/ T<sub>2</sub></p></li><li><p>Acronym: GPT</p></li></ul><p></p>
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Charles Law

  • At constant pressure and moles, Volume (V) and Temperature (T) are directly related

  • Equation: V1 / T1 = V2 / T2

  • Acronym: CVT


<ul><li><p>At constant pressure and moles, Volume (V) and Temperature (T) are directly related</p></li><li><p>Equation: V<sub>1 </sub>/ T<sub>1 </sub>= V<sub>2 / </sub>T<sub>2</sub></p></li><li><p>Acronym: CVT</p></li></ul><p></p>
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Boyles Law

At constant temperature and moles; Pressure (P) and Volume (V) are inversely related

<p>At constant temperature and moles; Pressure (P) and Volume (V) are inversely related</p>
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Ideal Gas Law

PV=nRT or (P1⋅V1) ÷ (N1 T1) = (P2⋅V2) ÷ (N2 T2)

<p>PV=nRT or (P<sub>1</sub>⋅V<sub>1</sub>) ÷ (N<sub>1</sub> T<sub>1</sub>) = (P<sub>2</sub>⋅V<sub>2</sub>) ÷ (N<sub>2</sub> T<sub>2</sub>)</p>
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What are the equations to solve for each variable?

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Combined Gas Law

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