17. Thermal Behavior of Matter 1. Gases 2. Phase Changes 3. Thermal Expansion

What unusual property of water is evident in this photo? Ice is less dense than water.

17.1. Gases The Ideal Gas Law: A piston-cylinder system. k = 1.38  10  23 J / K = Boltzmann’s constant N = number of molecules N A =  = Avaogadro’s number = number of atoms in 12 g of 12 C. n = number of moles (mol) = J / K mol = Universal gas constant All gases become ideal if sufficiently dilute.

Example STP What volume is occupied by 1.00 mol of an ideal gas at standard temperature & pressure (STP), where T = 0  C, & p = kPa = 1 atm? ( last figure subject to round-off error )

Kinetic Theory of the Ideal Gas Kinetic theory ( Newtonian mechanics ): 1.Gas consists of identical “point” molecules of mass m. 2. No interaction between molecules, except when they collide. 3. Random motion. 4. Collisions with wall are elastic.

Molecule i collides with right-hand wall (RHW). Momentum transfer to wall is No intermolecular collision  Next collision with RHW occurs at Average force of i on RHW: Random motion   Ideal gas law is recovered if T ~  K  in out

Example Air Molecule Find  K  of a molecule in air at room temperature ( 20  C = 293K), & determine the speed of a N 2 molecule with this energy. Thermal speed:

Distribution of Molecular Speeds Maxwell-Boltzmann Distribution: (elastic collisions between free particles) High-E tail extends rapidly with T  chemical reaction easier at high T  cooling of liquid ( by escape of high-E molecules) 80 K v th 300K v th

Real Gases Important corrections to the ideal gas model: 1.finite size of molecules  available V reduced. 2.Attractive interaction between molecules (van der Waals forces)  reduced P. van der Waals equation minimum volume 

Real Gases Important corrections to the ideal gas model : 1.finite size of molecules  available V reduced. 2.Attractive interaction between molecules (van der Waals forces)  reduced P. van der Waals equation minimum volume

17.2. Phase Changes T vs t for a block of ice, initially at － 20 ℃, that is supplied with constant power under atmospheric P. Phase changes take place at fixed T = T C until whole system is in the new phase. ( breaking / building bonds raises U but keeps K unchanged ) Heat of transformation L = energy per unit mass needed to change phase. L f = Heat of fusion ( solid  liquid ) L v = Heat of vaporization ( liquid  gas ) L s = Heat of sublimation ( solid  gas ) ice warming melting water warming boiling steam warming

Water:  Same E to melt 1 g ice or heat water by 80  C

GOT IT? You bring a pot of water to boil & then forget about it. 10 min later you come back & find it still boiling. Is its temperature (a) less, (b) greater than, or (c) equal to 100  C ?

Example Meltdown! A nuclear power plant’s reactor vessel cracks, draining all cooling water. Although nuclear fission stops, radioactive decay continues to heat the reactor’s 2.5  10 5 kg uranium core at the rate of 120 MW. Once the melting point is reached, how much energy will it take to melt the core? How long will the melting take? Table 17.1: for U Time to melt the core:

Example Enough Ice? When 200 g of ice at  10  C are added to 1.0 kg of water at 15  C, is there enough ice to cool the water to 0  C? If so, how much ice is left in the mixture? Heat released to bring water down to 0  C Heat required to bring ice up to 0  C  more than enough ice Ice needed:  ice left =

Phase Diagrams Phase diagram: P vs T Sublimation: solid  gas e.g., dry ice ( s-CO 2 ) Critical point : l-g indistinguishable AB: low P, s  g CD: medium P, s  l  g EF: high P, s  l / g GH: medium T, l  g Caution: Phase transition doesn’t occur instantaneously Triple point: s-l-g coexist = K, 0.6 kPa for H 2 O Solid gas liquid Melting Sublimation Boiling C.P. T.P.

17.3. Thermal Expansion Coefficient of volume expansion : Coefficient of linear expansion : Prob. 69 Prob. 72

GOT IT? If a donut-shaped object is heated, will the hole get (a) larger, or (b) smaller ?

Example Spilled Gasoline A steel gas can holds 20 L at 10  C. It’s filled to the brim at 10  C. If the temperature is now increased to 25  C, by how much does the can’s volume increase? How much gas spills out? Table 17.2:   Spilled gas:

Thermal Expansion of Water Reason: Ice crystal is open   ice   water  ice floats max  water occurs at 4  C At 1  C At fixed T  T m, ice melts if P . Application: skating.  > 0  < 0

Application: Aquatic Life & Lake Turnover Anomalous behavior of ice-water makes aquatic life in freezing weather possible. If deep enough, bottom water stays at 4  C even when surface is iced over. In a lake where bottom water stays at 4  C year round, surface & bottom water can mix (turnover) only in spring time when both are at 4  C.