atmospheric chemistry
In the study of gases, several key principles and variables are crucial for understanding their behavior and properties. Gases are highly compressible and do not have a fixed shape, adapting to the volume of their containers.
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T = 298.15K P = 100kPa T = 273.15K P =100kPa SATP collisions kinetic energy ∝ temperature Avogadro's Law Density Lots of space between particles Gas condition STP Planetary atmospheres Atmospheric Composition Greenhouse Gases Standard atmospheric conditions climate change mol mole fraction ratio of moles of one substance vs. total substances in gas mixture partial pressure molar mass g/mol Molar Constant (R) Ideal Gas Law Combined Gas Law particles are small, spehrical entities -273.13 Gas is highly condensable, no fixed shape Charles's Law Gay-Lussac's law Boyle's Law Impacts from particles on surfaces create pressure particles Pressure (P) Temperature (T) Melting/Fusion state changes Liquids Solid Particle theory KMT States of Matter Absolute Temperature number of particles (n) °C S.I. Units K Pa L atmospheric chemistry Gas 4 Main variables Volume (V) Properties Gas Laws
