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https://chem.libretexts.org/Core/Physical_and_Theoretical_Chemistry/Physical_Properties_of_Matter/States_of_Matter/Properties_of_Gases/Gas_Laws/The_Ideal_Gas_Law

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"1 atm = 760 mmHg = 760 torr = 101.3 kPa" and well as "T = Degrees C + 273.15"

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Taking the decreased pressure and volume and linking that to the initial temperature would result in finding the overall change that is pressured on these factors to get the final calculations.

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P1V1/T1 = P2V2/T2

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Resource: http://chemistry.tutorcircle.com/inorganic-chemistry/combined-gas-law.html

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*With all of these views in mind we can attempt even more complex calculations that focus on all three factors.

Key Phrase: "Combination"

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Pressure is generally shown as kilopascals, atmospheres, or mmHg.

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*Comparing decreased pressure to increased pressure divided by the temperature alteration that impacts the resulting values of both factors will allow chemists to determine the hidden value. It's as if you were determining a percentage by converting the pressure and temperature separately and dividing afterward.

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P1/T1 = P2/T2

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*When contemplating temperature and pressure there is a similar calculation to the Charles' Law that will allow precise calculations.

Key Phrase: "Direct Proportionality"

*When it is hotter in an area there are particles that are more desperate to tap into this new booster shot of energy that they are experiencing. In doing so the pressure intensifies rather than dropping when there is hardly any heat and materials are freezing up all around them.

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The most important aspect of this law is Kelvins as a unit form rather than degrees celsius.

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*With decreased volume divided by decreased temperature is the same as concluding the increased volume divided by increased temperature, since both sides have numerical values going up or down.

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V1/T1 = V2/T2

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Resource: https://www.visionlearning.com/es/library/Qu%C3%ADmica/1/Kinetic-Molecular-Theory/251

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*This law focuses on temperature and volume rather than considering the effects of pressure when studying the activity of gases.

Key phrase: "Direct proportionality!"

*This means that when you have a really cold environment there will be very little volume in that area since the gas particles in ice are too stiff for a great deal of activity. When it gets really warm, the ice becomes water and the gas particles are flinging about enjoying the heat and the enhanced arena they have to enjoy because of state alteration of their hostess.

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According to the textbook for this course the SI units are litres for volume and kilopascals, atmospheres, or mmHg, depending on the information given.

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*If increased pressure is multiplied by decreased volume, it would be the same thing as multiplying decreased pressure by increased volume (if the units are the same of course), which is why they are set equal to each other.

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P1V1 = P2V2

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Resource: https://sites.google.com/site/svgphysics/topics2012_2013/gas-laws/gas-laws---boyle-s-law

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*This law concludes that the volume and pressure of initial and final numerical values can be multiplied together and set equal to each other for precise calculations.

Key phrase: "inverse proportionality!"

*This means that when there is an extensive amount of volume available for gases to dance around in, there will understandably be a limited amount of pressure holding those particles back from meeting exploring their surroundings thoroughly. The diagram shows this idea and it also shows that when volume/room is cut down (as if the particles are being huddled together) the gases are more confined to swaying back and forth than leaping about the room and thus there is more pressure to hold them where they are.