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Kinetic-Molecular Theory (KMT)

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Presentation on theme: "Kinetic-Molecular Theory (KMT)"— Presentation transcript:

1 Kinetic-Molecular Theory (KMT)
motion of particles (energy, collisions) 1) constant particle motion 2) Pressure caused by collisions 3) IMAFs are negligible 4) Volume of particles is negligible compared to total volume (Vgas = Vcontainer – Vparticles) 5) Average KE directly proportional to Kelvin Temp (T , KE)

2 PV = nRT P ↑ , V ↓ T ↑ , V ↑ P1V1 n1T1 P2V2 n2T2 = T ↑ , P ↑ n ↑ , V ↑
R = L∙atm/mol∙K inverse T ↑ , V ↑ P1V1 n1T1 P2V2 n2T2 = T ↑ , P ↑ (changes in P,V,T,n) n ↑ , V ↑ direct Ptotal = PA + PB + PC + … PA = Ptotal x XA XA: mol fraction moles of A Molar Volume: 22.4 L/mol XA = @STP total moles

3 Temp, KE, & Molecular Speed
KE = ½ mv2 ↑T a ↑KE KMT states: KE = ½ mv2 ½ mv2 = ½ mv2 At same T : (same KE) ↑M , ↓v

4 Ideal Gas vs Non-Ideal Gas
T: ↑ P: ↓ NON T: ↓ P: ↑ more KE weaker IMAFs more Vtotal less KE stronger IMAFs less Vtotal IMAFs (ideal P) (ideal V) n2a V2 ) (V ) = nRT (P + − nb “observed” V too high b/c size of particles not negligible compared to total volume “observed” P too low b/c attractive forces not negligible, collisions less frequent and of less force Vgas = Vcontainer – Vparticles


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