Review Answers - Chapter 13 and 14

Honors Chemistry Chapter 13 and 14 Review Packet Name: Key Chapter 13: States of Matter tion 1. The Nature of Gusex 1. What are the three assumptions of kinetic molecular theory? 1. Particlerin a gas have insignificant volume 2. gas particle motion is kapid, constant, and Random 3. gas particle collisions are perfectly elastic 2. What causes pressure? continuous collisions of particles with container 3. What is the relationship between kinetic energy and temperature? as temperature increases, Kinetic energy increases Section 2 The Nature of Liquids 1. What is the difference between the particles in a liquid vs. the particles in a solid? particles in a liquid have more space between them. 2. Why does evaporation tend to occur at higher temperatures? higher temp-higher kinetic energy to prenecome liquid barticle attraction. . What is the relationship between the rate of evaporation and the rate of condensation in a closed system 3 under conditions of dynamic equilibrium? rate condensation = Rate evaporation Section 3. The Nature of Solids 1. What is the structure of most solids? closely racked particles, dense, particles vibrate, Crystal Lattice structure 2. What is a unit cell? smallest group of particles in a crystal that ketain geometric share. is an allotrope? What is an example of an allotrope? 3. What is 2. of more different molecular culare forms of the same Prement in the same physical state le carbon diamond graphite 4. What is an amorphous a solid lacking an ordered internal structure Section 4: Changes of State 1. Circle the phase changes that will lead to an increase in energy. Melting Evaporation Deposition Condensation Sublimation Solidification Honors Chemistry Chapter 13 and 14 Review Packet Name: 2. Complete the phase change chart: Starting Phase Solid Ending Phase Liquid gas solld gas Gas Solid Liquid Solid Gas Liguld Key Phase Change melting Evaporation Sublimation Deposition Solidification Condensation 3. What is the major difference between the phase diagram of water in comparison to other phase diagrams? Slope of line between sund liquid is to the left. 4. Answer the following questions about the phase diagram below: Paran Bagram for mysteratus comp a. What phase is the compound in: i. At 70 atm and 200 deg * C ? ii. At 700 deg * C and 20 atım? iii. At 500 deg * C and 80 atm? iv. At 60 atm and 400 deg * C Tempest idegrees C Solid aas. 1iquid 119 liquid b. What phase change(s) would occur under the following conditions: 1. The substance at 100 deg * C changes from 20 atm to 40 atm Deposition ii. The substance at 80 atm changes from 300 deg * C to 600 deg * C Melting iii. The substance at 70 atm changes from 200 deg * C to 800 deg * C melting, evaporation iv. The substance at 90 atm and 400 deg * C drops to 50 atm melting, evaporation c. On the diagram: 1. Circle the triple point. ii. Draw a triangle around the critical point. d. Is it possible to use this phase diagram to determine the normal boiling point of the substance? Why or why not? ND. I atm of pressure isn't on the y axis. C+ 3 = x tion 1. Properties of Gaxex 1. Complete the following conversions: a 90 atm to kPa 9,117 кра b. 40 deg * C K 313K Honors Chemistry Chapter 13 and 14 Review Packet Name: Key Chapter 14: The Behavior of Gas am =10| kPa 760mmHg c. mmllg to atm 2.3480tm a) 900tm 101.3kha Hatm 1800mmitg lat 760mmitg d. 8675.3 kPa to atm 85. 104am d) 8675.3 kPa Latm c. 498K * 10 deg * C 22500 0 deg * C to K 273K g. 13.2 kPa to mmHg. 99.03mmt19 9) 13.2 kPa Tuompt19 101-3KPA h. 400 Torr to alm 0.524 atm Doc and I atra Equation P_{1}*V_{1} = P_{2}*V_{2} 2. Circle the term to best complete each statement: a. As volume increases, pressure.... increases/decreases n) 400 Tore Latm... TOOTORR b. As temperature increases, pressure... increases/decreases c. As pressure decreases, volume... increases decreases d. As temperature increases, volume.... increases/ decreases e. As amount of gas increases, pressure... increases/decreases f. As the number of particle collisions decreases, pressure... increases/ decreases Sections 2 and 3: Gas Laws 1. What are the values for STP? 2. Complete the gas law chart: Name of Gas Law Boyle's Law Value Held Constant Required Units (If necessary) Same on both sides Charles Law P Gay-Lussac's Law Tin Kelvin Temperature in Kelvin V Combined Gas Law NIA I deal Gas Law PV RT N/A Dalton's Law T Tin Kelvin Tinkelvin Rdepends on P All same pressure units Graham's Law RAKA MINIS N/A 3. Sample problems for each gas law: a. Boyle If 85.2 1. of nitrogen at 0.750 atm are compressed to 760 mmHg at constant temperature, determine the final volume of nitrogen. (570mmHg) (85.21)=(140mmtig) (V2) V_{2} = U * 3.9L P_{1} / T_{1} = P_{2} / I_{32} P total = P_{1} + P_{2} +... V_{1} / T_{1} = V_{2} / T_{2}