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Stoichiometric Relationships, Kinetic Molecular Theory - Coggle Diagram
Stoichiometric Relationships, Kinetic Molecular Theory
States
Solid
- Lowest energy + closest together
- Rotate and vibrate about fixed positions
- Strong forces of attractions between particles
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Liquid
- More energy and further apart than solid
- Move freely in close proximity
- Moderate forces of attraction between particles
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Gas
- Far apart and highest energy
- Move rapidly, randomly, haphazardly into available space
- Little forces of attraction between particles
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Definitions
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Mixture
Combination of 2 or more substances separated by physical methods
- Heterogenous: 2 or more unevenly distributed throughout = non-uniform composition, varying properties
- Homogenous: 2 or more substances evenly distributed throughout = uniform composition, properties
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Molar Mass (M)
Mass of substance in grams that contains one mole of particles (same value as Mr and Ar)
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Relative Atomic Mass
Weighted average of the atomic masses of its isotopes and their relative abundance compared to 1/12 the mass of 1 C-12 atom
Mole Concept
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Volume of gas/22.7dm^3mol^-1
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Volume of gas/24.8dm^3mol^-1
Gases
Ideal Gas
- Simplistic assumptions
- Good estimations of measurement
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Collisions are elastic
- No loss of kinetic energy
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Small particles separated by large distances
- Mostly empty space = particles negligible volume
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Hypothetical State approached in:
- High temperature (KE > intermolecular forces of attraction = insignificant)
- Low pressure (Size of molecules are negligible compared to volume)
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Maxwell Boltzmann Speed Distribution 
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At the same temperature, lighter atoms move faster
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pV = nRT
- p = pressure in pascal/Nm^-2 (1atm = 1.00 * 10^5Pa)
- V = volume in m^3
- n = molecules of gas
- T = temperature in Kelvin (C +273)
- R (gas constant) = 8.31JK^-1mol^-1
Flat Line
- PV/T against P, V or T
- Temperature constant: PV against P or V
Going Up
- Temperature constant: P against 1/V
- Pressure constant: V against T --> V1/T1 = V2/T2
Negative exponential but all positive
- Temperature constant: P against V
- Temperature constant = PV constant, P1V1 = P2V2