Chemistry Lab/Gas Laws: Difference between revisions
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==Graham's Law== | ==Graham's Law== | ||
==The Ideal Gas Law== | ==The Ideal Gas Law== | ||
PV=nRT | |||
P=Pressure | |||
V=Volume | |||
n=moles | |||
R=Gas constant | |||
T=temperature | |||
====Gas Constants==== | |||
*List 82.055 cm3 atm K-1 mol-1 | |||
*List 0.082055 L atm mol-1 K-1 | |||
*List 8.31434 J mol-1 K-1 | |||
*List 1.9872 cal K-1 mol-1 | |||
*List 8314.34 L Pa mol-1 K-1 | |||
*List 8.31434 Pa m3 mol-1 K-1. | |||
==Memorization== | ==Memorization== | ||
HERE’S AN EASY WAY TO MEMORIZE ALL OF THIS! | HERE’S AN EASY WAY TO MEMORIZE ALL OF THIS! | ||
Revision as of 15:50, 2 December 2015
 | This page is incomplete. |
This page refers to the 2016 focus of Chemistry Lab.
Avogadro's Law
Avogadro's Law, also known as Avogadro's hypothesis or Avogadro's principle, says equal volumes of all gases, at the same temperature and pressure, have the same number of moles. In particular, the volume of a gas is proportional to the number of moles.
Boyle's Law
Charles' Law
Dalton's Law
Gay-Lussac's Law
Graham's Law
The Ideal Gas Law
PV=nRT
P=Pressure V=Volume n=moles R=Gas constant T=temperature
Gas Constants
- List 82.055 cm3 atm K-1 mol-1
- List 0.082055 L atm mol-1 K-1
- List 8.31434 J mol-1 K-1
- List 1.9872 cal K-1 mol-1
- List 8314.34 L Pa mol-1 K-1
- List 8.31434 Pa m3 mol-1 K-1.
Memorization
HERE’S AN EASY WAY TO MEMORIZE ALL OF THIS! Start with the combined gas law: P1V1T2 = P2V2T1 Memorize it. Next, put the fellas’ names in alphabetical order. Boyle’s uses the first 2 variables, Charles’ the second 2 variables & Gay-Lussac’s the remaining combination of variables. What ever doesn’t appear in the formula, is being held CONSTANT!