PART 8-Changes in States, Colligative Properties, and Phase Diagram Reference: Chapter 5, 12 in textbook
PART 8 – Ch i St t Changes in States, Colligative Properties and Phase Properties, and Phase Diagram Reference: Chap , ter 5 12 in textbook 1
States of materials Solid Liquid Gas ,● 器∴
States of Materials Solid Liquid Gas 2
Gas and ideal gas Properties of a Gas Low density, No fixed shape Can be significantly expanded and compressed Can be mixed by any ratios o Ideal gas- Assumption Gas molecules have no volume No intermolecular interaction
Gas and Ideal Gas z Prope es o a Gas rties of a Gas Low density, No fixed shape Can be significantly expanded and compressed Can be mixed by any ratios Can be mixed by any ratios z Ideal Gas Ideal Gas – Assumption Assumption Gas molecules have no volume; No intermolecular interaction 3
Ideal gaS: PV. t P VS. V →P*∨= constant or 。∨vs.T →∨/T= constant or V1/T1=V2/T2 。Pvs.T →P/T= constant or P1/T1=P2/T2 Note: the units of Pv. t 4
Ideal Gas: P, V, T z P sV v s. V Æ P * V = constant or P1 * V1 = P 2 1 1 * V 2 z V vs. T Æ V / T = constant or V1 / T1 = V 2 / T 2 z P vs. T Æ P/T t t P / T = cons tan t o r P1 / T1 = P 2 / T 2 z Note: the units of P V T Note: the units of P, V, T 4
Ideal gas law Ideal Gas equation P*V=n*R*t P: 101.3 kPa =1 atm=760 mmHg =760 torr V:1m3=1×103dm3(L)=1×106cm3(mL) T:K=C°+273.15 ,n: of moles of all gases R=8.31J·mo1K1=0.082atm·L·mo1·K1 Avogadros Law Under same P, T, 1 mole of gas occupies the same V At the Standard Temperature Pressure(STP),1 mole of any ideal gas is 22. 4 liter 5
Ideal Gas Law z Ideal Gas Equation P * V = n * R * T ¾ P： 101 3. kPa = 1 atm = 760 mmHg = 760 = 760 mmHg = 760 torr ¾ V： 1 m3 = 1 × 103 dm3 ( L ) = 1 × 106 cm3 (mL) ¾ T： K = C° + 273.15 ¾ n ： # of moles of all gases ¾ R = 8.31 J • mol-1•K-1 = 0.082 atm • L • mol-1 • K-1 z Avogadro’s Law Under same P T 1 mole of gas occupies the same V Under same P, T, 1 mole of gas occupies the same V. At the Standard Temperature & Pressure (STP), 1 mole of any ideal gas is 22.4 liter. 5