# = atm. 760 mm Hg. = atm. d. 767 torr = 767 mm Hg. = 1.01 atm

Save this PDF as:

Size: px
Start display at page:

Download "= 1.038 atm. 760 mm Hg. = 0.989 atm. d. 767 torr = 767 mm Hg. = 1.01 atm"

## Transcription

1 Chapter 13 Gases 1. Solids and liquids have essentially fixed volumes and are not able to be compressed easily. Gases have volumes that depend on their conditions, and can be compressed or expanded by changes in those conditions. Although the particles of matter in solids are essentially fixed in position (the solid is rigid), the particles in liquids and gases are free to move. 2. The pressure of the atmosphere represents the weight of the several-mile-thick layer of gases pressing down on every surface of the earth. Pressure, in general, represents a force exerted over a particular area, and the pressure of the atmosphere corresponds to a pressure of nearly 15 pounds per square inch on the surface of the earth. 3. A simple mercury barometer is a tube filled with mercury inverted over a reservoir containing mercury that is open to the atmosphere. When the tube is inverted, the mercury falls to a level at which the pressure of the atmosphere is sufficient to support the column of mercury. One standard atmosphere of pressure is taken to be the pressure capable of supporting a column of mercury to a height of mm above the reservoir level. 1 atm 4. a kpa atm kpa b cm g 10 mm g 1 cm g 1 atm atm 760 mm g 1 atm c. 752 mm g 760 mm g d. 767 torr 767 mm g atm 767 torr 1 atm 760 torr 1.01 atm 760 mm g 5. a atm mm g 1 atm 760 mm g b. 225,400 Pa 1691 mm g 101,325 Pa 760 mm g c kpa 748 mm g kpa 760 mm g d atm mm g 1 atm 101,325 Pa 6. a. 774 torr Pa 760 torr 101,325 Pa b atm Pa 1 atm 130

2 Gases 131 c kpa Pa d. 801 mm g 101,325 Pa 760 mm g Pa 7. a. P mm g P mm g V ml V 2? ml V 2 P 1 V 1 P 2 (53.2 ml)(785 mm g) 700 mm g 59.7 ml b. P atm P 2? atm V L V L P 2 P 1 V 1 V 2 (1.67 atm)(2.25 L) 2.00 L 1.88 atm c. P mm g P atm 1148 mm g V L V 2? L V 2 P 1 V 1 P 2 (695 mm g)(5.62 L) 1148 mm g 3.40 L 8. a. P atm P atm V ml V 2? ml V 2 PV 1 1 (1.07 atm)(291 ml) P atm 146 ml b. P mm g P atm 2668 mm g V L V 2? L V 2 PV (755 mm g)(1.25 L) 1 1 P mm g L c. P kpa mm g P 2? mm g V L V L P 2 PV (760.6 mm g)(2.71 L) 1 1 V 2 (3.00 L) 687 mm g 9. If the pressure exerted on the gas in the balloon is decreased, the volume of the gas in the balloon will increase in inverse proportion to the factor by which the pressure was changed. The factor in this example is (1.01 atm/0.562 atm) P mm 1.00 atm P 2? atm V L V ml L P 2 PV (1.00 atm)(1.00 L) 1 1 V 2 ( L) 20.0 atm

3 132 Chapter Absolute zero is the lowest temperature that can exist. Absolute zero is the temperature at which the volume of an ideal gas sample would be predicted to become zero. Absolute zero is the zero-point on the Kelvin temperature scale (and corresponds to 273 C). 12. Charles s law states that the volume of an ideal gas sample varies linearly with the absolute temperature of the gas sample. In an experiment performed to determine absolute zero, the volume of a sample of gas is measured at several convenient temperatures (e.g., between 0 C and 100 C) and the data is plotted. The straight line obtained is then extrapolated to the point where the volume of the gas would become zero. The temperature at which the volume of the gas would be predicted to become zero is then absolute zero. 13. V ml V 2? ml 26.5 C 300 K T C 328 K V 2 P 1 T 2 (45.0 ml)(328 K) (300 K) 49.2 ml 14. a. V L V L 0 C 273 K T 2? C T 2 V 2 V 1 (50.0 L)(273 K) (25.0 L) 546 K 273 C b. V ml V ml 25 C 298 K T 2? C T 2 V 2 V 1 (255 ml)(298 K) (247 ml) 308 K 35 C c. V ml V 2? ml 272 C 1 K T 2 25 C 298 K V 2 V 1 T 2 (1.00 ml)(298 K) (1 K) 298 ml 15. a. V L V L 1150 C 1423 K T 2? C T 2 V 2 V 1 (5.00 L)(1423 K) (2.01 x 10 2 L) 35.4 K 238 C b. V ml V 2? ml 298 K T 2 0 K V 2 V 1 T 2 (44.2 ml)(0 K) (298 K) 0 ml (0 K is absolute zero)

4 Gases 133 c. V ml V 2? ml 298 K T 2 0 C 273 K V 2 V 1 T 2 (44.2 ml)(273 K) (298 K) 40.5 ml C 297 K 272 C 1 K 5.00 L 1 K 297 K L 0.02 L 17. You should be able to answer these without having to set up a formal calculation. Charles s law says that the volume of a gas sample is directly proportional to its absolute temperature. So if a sample of neon has a volume of 266 ml at 25.2 C (298 K), then the volume will become half as big at half the absolute temperature (149 K, 124 C). The volume of the gas sample will become twice as big at twice the absolute temperature (596 K, 323 C) C K 54 C K 500. ml 327 K 298 K 549 ml 19. V ml V 2? L n mol n mol 652 ml mol mol 1143 ml 1.14 L 20. V L V 2? L n g/32.00 g mol 1 n g/32.00 g mol 1 V 2 V 1 n 2 n 1 (100. L)(5.00 g/32.00 g mol 1 ) (46.2 g/32.00 g mol 1 ) 10.8 L Note that the molar mass of the O 2 gas cancels out in this calculation. Since the number of moles of Ne (or any gas) present in a sample is directly proportional to the mass of the gas sample, the problem could also have been set up directly in terms of the masses. 21. Real gases most closely approach ideal gas behavior under conditions of relatively high temperatures (0 C or higher) and relatively low pressures (1 atm or lower). 22. For an ideal gas, PV nrt is true under any conditions. Consider a particular sample of gas (so that n remains constant) at a particular fixed temperature (so that T remains constant also). Suppose that at pressure P 1 the volume of the gas sample is V 1. Then for this set of conditions, the ideal gas equation would be given by P 1 V 1 nrt

5 134 Chapter 13 If we then change the pressure of the gas sample to a new pressure P 2, the volume of the gas sample changes to a new volume V 2. For this new set of conditions, the ideal gas equation would be given by P 2 V 2 nrt Since the right-hand sides of these equations are equal to the same quantity (since we defined n and T to be constant), then the left-hand sides of the equations must also be equal, and we obtain the usual form of Boyle s law. P 1 V 1 P 2 V a. P 782 mm g 1.03 atm T 27 C 300 K V nrt P (0.210 mol)( L atm mol 1 K 1 )(300. K) (1.03 atm) 5.02 L b. V 644 ml L P nrt V ( mol)( L atm mol 1 K 1 )(303 K) (0.644 L) 3.56 atm P 3.56 atm mm g c. P 745 mm atm T PV nr (0.980 atm)(11.2 L) (0.401 mol)( L atm mol 1 K 1 ) 334 K 24. a. T 25 C 298 K V ( mol)( L atm mol 1 K 1 )(298 K) (1.01 atm) L b. V 602 ml L P (8.01 x 10-3 mol)( L atm mol 1 K 1 )(310 K) (0.602 L) atm c. V 629 ml L T 35 C 308 K n (0.998 atm)(0.629 L) ( L atm mol 1 K 1 )(308 K) mol

6 Gases molar mass of N g 58.2 C 331 K n 4.24 g N 2 1 mol N g N mol N 2 V nrt/p (0.151 mol)( L atm mol 1 K 1 )(331 K) (2.04 atm) The number of moles of any ideal gas that can be contained in the tank under the given conditions can first be calculated. T 24 C 297 K n PV (135 atm)(200 L) RT ( L atm mol 1 K 1 )(297 K) mol gas Molar masses: e, g; 2, g for e: mol e g g e 4.44 kg e 1 mol for 2 : mol g g kg 2 1 mol 27. Molar mass of N g 16.3 g N 2 1 mol mol N g T PV nr (1.25 atm)(25.0 L) (0.582 mol)( L atm mol 1 K 1 ) 654 K 381 C 28. Molar mass of O g 56.2 kg g g 1 mol g mol T 21 C 294 K P nrt V (1.76 x 10 3 mol)( L atm mol 1 K 1 )(294 K) (125 L) 340 atm 29. P atm P atm V ml V 2? ml 100 C 373 K T 2 25 C 298 K V 2 P 1 V 1 T 2 P 2 (0.981 atm)(125 ml)(298 K) (1.15 atm)(373 K) 85.2 ml 30. P atm P atm V ml V 2? ml

7 136 Chapter C 300. K V 2 P 1 V 1 T 2 P 2 (1.05 atm)(459 ml)(288 K) (0.997 atm)(300 K) T 2 15 C 288 K 464 ml 31. In deriving the ideal gas law, we assume that the molecules of gas themselves occupy no volume, and that the molecules do not interact with each other. Under these conditions, there is no difference between gas molecules of different substances (other than their masses) as far as the bulk behavior of the gas is concerned. Each gas behaves independently of other gases present, and the overall properties of the sample are determined by the overall quantity of gas present. P total P 1 + P P n where n is the number of individual gases present in the mixture 32. As a gas is bubbled through water, the bubbles of gas become saturated with water vapor, thus forming a gaseous mixture. The total pressure in a sample of gas that has been collected by bubbling through water is made up of two components: the pressure of the gas of interest and the pressure of water vapor. The partial pressure of the gas of interest is then the total pressure of the sample minus the vapor pressure of water. 33. molar masses: O 2, g; e, g 65 C K 4.0 g O 2 1 mol O g O mol O g e 1 mol e g e mol e P oxygen n oxygen RT/V (0.125 mol)( L atm mol 1 K 1 )(338 K) (5.0 L) P oxygen atm 0.69 atm P helium n helium RT/V (0.999 mol)( L atm mol 1 K 1 )(338 K) (5.0 L) P helium 5.54 atm 5.5 atm P total atm atm atm 6.2 atm 34. Total moles of gas 3.0 mol mol mol 6.0 mol 3.0 mol P nitrogen 10.0 atm 5.0 atm 6.0 mol 2.0 mol P oxygen 10.0 atm 3.3 atm 6.0 mol 1.0 mol P carbon dioxide 10.0 atm 1.7 atm 6.0 mol 35. P oxygen P total P water vapor torr

8 Gases P oxygen P total P water vapor mm g atm T 24 C K V 500. ml L n PV/RT ( atm)(0.500 L) ( L atm mol 1 K 1 )(297 K) mol O CaCO 3 (s) CO 2 (g) + CaO(s) molar mass CaCO g 15.2 g CaCO 3 1 mol CaCO g CaCO mol CaCO 3 From the balanced chemical equation, if mol CaCO 3 reacts, mol of CO 2 will result. STP: 1.00 atm, 273 K V nrt/p (0.152 mol)( L atm mol 1 K 1 )(273 K) (1.00 atm) 3.41 L 38. C 3 8 (g) + 5O 2 (g) 3CO 2 (g) O(g) 25 C K molar mass C g 5.53 g C mol C g C mol C mol C mol O 2 1 mol C mol O 2 V nrt/p ( mol O 2 )( L atm mol 1 K 1 )(298 K) (1.04 atm) 14.7 L O C 300 K 26 C 299 K mol N 3 present (1.02 atm)(4.21 L) ( L atm mol 1 K 1 )(300 K) mol N 3 mol Cl present (0.998 atm)(5.35 L) ( L atm mol 1 K 1 )(299 K) mol Cl N 3 and Cl react on a 1:1 basis: N 3 is the limiting reactant. molar mass N 4 Cl g mol N 3 1 mol N Cl g N Cl 4 1 mol N 3 1 mol N 4 Cl 9.31 g N 4 Cl produced

9 138 Chapter Molar mass of Mg 3 N g 10.3 g Mg 3 N 2 1 mol g mol Mg 3N 2 From the balanced chemical equation, the amount of N 3 produced will be mol Mg 3 N 2 2 mol N 3 1 mol Mg 3 N mol N 3 T 24 C 297 K P 752 mm g atm V nrt P (0.204 mol)( L atm mol 1 K 1 )(297 K) (0.989 atm) 5.03 L This assumes that the ammonia was collected dry. 41. Molar masses: e, g; 2, g 14.2 g e 1 mol e g e 3.55 mol e 21.6 g 2 1 mol g mol total moles 3.55 mol mol 14.3 mol 28 C 301 K V nrt P (14.3 mol)( L atm mol 1 K 1 )(301 K) (0.985 atm) 359 L 42. P atm P atm (standard pressure) V ml V 2? ml 44 C 317 K T 2 0 C 273 K (standard temperature) V 2 P 1 V 1 T 2 P 2 (1.47 atm)(145 ml)(273 K) (1.00 atm)(317 K) 184 ml 43. molar masses: O 2, g; N 2, g; CO 2, g; Ne, g 5.00 g O 2 1 mol O g O mol O g N 2 1 mol N g N mol N g CO 2 1 mol CO g CO mol CO 2

10 Gases g Ne 1 mol Ne g Ne mol Ne Total moles of gas mol 22.4 L is the volume occupied by one mole of any ideal gas at STP. This would apply even if the gas sample is a mixture of individual gases mol 22.4 L L 15.6 L 1 mol The partial pressure of each individual gas in the mixture will be related to what fraction on a mole basis each gas represents in the mixture. P oxygen 1.00 atm mol O mol total P nitrogen 1.00 atm mol N mol total atm O atm N 2 P carbon dioxide 1.00 atm mol CO mol total atm CO 2 P neon 1.00 atm mol Ne mol total atm Ne 44. 2Na(s) + Cl 2 (g) 2NaCl(s) molar mass Na g mol Na g Na mol Na mol Na 1 mol Cl 2 2 mol Na mol Cl mol Cl L 1 mol 2.34 L Cl 2 at STP 45. 2K 2 MnO 4 (aq) + Cl 2 (g) 2KMnO 4 (s) + 2KCl(aq) molar mass KMnO g 10.0 g KMnO 4 1 mol KMnO g KMnO mol KMnO mol KMnO 4 1 mol Cl 2 2 mol KMnO mol Cl mol Cl L 1 mol L 709 ml 46. A law is a statement that precisely expresses generally observed behavior. A theory consists of a set of assumptions/hypotheses that is put forth to explain the observed behavior of matter. Theories attempt to explain natural laws.

11 140 Chapter A theory is successful if it explains known experimental observations. Theories that have been successful in the past may not be successful in the future (for example, as technology evolves, more sophisticated experiments may be possible in the future). 48. We assume that the volume of the molecules themselves in a gas sample is negligible compared to the bulk volume of the gas sample: this helps us to explain why gases are so compressible. 49. Chemists believe the pressure exerted by a gas sample on the walls of its container arises from collisions between the gas molecules and the walls of the container. 50. kinetic energy 51. The temperature of a gas reflects, on average, how rapidly the molecules in the gas are moving. At high temperatures, the particles are moving very fast and collide with the walls of the container frequently, whereas at low temperatures, the molecules are moving more slowly and collide with the walls of the container infrequently. The Kelvin temperature is directly proportional to the average kinetic energy of the particles in a gas. 52. If the temperature of a sample of gas is increased, the average kinetic energy of the particles of gas increases. This means that the speeds of the particles increase. If the particles have a higher speed, they will hit the walls of the container more frequently and with greater force, thereby increasing the pressure. 53. Any gas that does not follow the ideal gas law is not behaving ideally. In addition, if there are reasons to believe that the assumptions of the kinetic-molecular theory are poor assumptions, the gas sample is not behaving ideally. The fact that gases condense into liquids, for example, shows nonideal behavior. 54. When the volume of a gas is decreased, the gas particles take up a greater percentage of the volume of the container. The assumption in the KMT that gas particles take up a negligible volume is less correct. 55. First determine what volume the helium in the tank would have if it were at a pressure of 755 mm g (corresponding to the pressure the gas will have in the balloons) atm 6384 mm g V 2 (25.2 L) 6384 mm g 755 mm g 213 L Allowing for the fact that 25.2 L of e will have to remain in the tank, this leaves L of e for filling the balloons L e 1 balloon 1.50 L e 125 balloons 56. A decrease in temperature would tend to make the volume of the weather balloon decrease. Since the overall volume of a weather balloon increases when it rises to higher altitudes, the contribution to the new volume of the gas from the decrease in pressure must be more important than the decrease in temperature (the temperature change in kelvins is not as dramatic as it seems in degrees Celsius).

12 Gases S(s) + 3O 2 (g) 2SO 3 (g) 350. C K molar mass S g 5.00 g 1 mol S g S mol S mol 3 mol O 2 2 mol S mol O 2 V nrt/p ( mol)( L atm mol 1 K 1 )(623 K) (5.25 atm) 2.28 L O Assume the pressure at sea level to be 1 atm (760 mm g). Calculate the volume the balloon would have if it rose to the point where the pressure has dropped to 500 mm g. If this calculated volume is greater than the balloon's specified maximum volume (2.5 L) the balloon will burst. 2.0 L 760 mm g 500 mm g 3.0 L > 2.5 L. The balloon will burst C K 100 C K 729 ml 373 K 295 K 922 ml 60. P atm P torr atm V L V 2? 23 C K T 2 31 C 242 K V 2 T 2 P 1 V 1 P 2 (242 K)(1.0 atm)(1.0 L) (295 K)(0.289 atm) 2.8 L 61. 2Cu 2 S(s) + 3O 2 (g) 2Cu 2 O(s) + 2SO 2 (g) molar mass Cu 2 S g 25 g Cu 2 S 1 mol Cu 2 S g Cu 2 S mol Cu 2S mol Cu 2 S 3 mol O 2 2 mol Cu 2 S mol O C K V oxygen ( mol)( L atm mol 1 K 1 )(301 K) (0.998 atm) 5.8 L O mol Cu 2 S 2 mol SO 2 2 mol Cu 2 S mol SO 2

13 142 Chapter 13 V sulfur dioxide ( mol)( L atm mol 1 K 1 )(301 K) (0.998 atm) V sulfur dioxide 3.9 L SO molar masses: e, g; Ar, g; Ne, g 5.0 g e 1.0 g Ar 3.5 g Ne 1 mol e g e 1 mol Ar g Ar 1 mol Ne g Ne mol e mol Ar mol Ne Total moles of gas mol 22.4 L is the volume occupied by one mole of any ideal gas at STP. This would apply even if the gas sample is a mixture of individual gases mol 22.4 L 32 L total volume for the mixture 1 mol The partial pressure of each individual gas in the mixture will be related to what fraction on a mole basis each gas represents in the mixture. P e 1.00 atm P Ar 1.00 atm P Ne 1.00 atm mol e mol total mol Ar mol total mol Ne mol total 0.86 atm atm 0.12 atm atm P 1 72 cm g 720 mm g 760 mm g 0.95 atm P atm V ml V 2? n 1 x n 2 2/3x (1/3 of gas removed) 27 C 300 K T K PV nrt or R PV nt Thus, P 1 V 1 n 1 P 2 V 2 n 2 T 2 constant (0.95 atm)(350 ml) (x)(300. K) (1.00 atm)(v 2 ) (2/3x)(600. K) Thus, V ml

14 Gases A balloon is essentially a constant pressure container. Thus, P and n are constant. PV nrt or nr P V T constant Thus, V 1 V 2 T L 293 K 2.00 L T 2 T K 508 C 65. PV nrt or T PV nr P atm Assume V 1.00 L 1.00 L 1000 cm L x 1.4 g 1400 g gas 3 1 cm 1400 g 1 mol 2.00 g 700 mol gas Thus, T (1.3 x 10 9 atm)(1.00 L) (700 mol)( L atm mol 1 K 1 ) K 66. If we can determine the molar mass of X 4 10, we can determine X. PV nrt or n PV RT P 801 mm g 1 atm 760 mm g 1.05 atm V 30.0 cm L L 1000 cm 3 T 20 C K n (1.05 atm)( L) ( L atm mol 1 K 1 )(293 K) mol g molar mass of X g/mol 1.31 x 10-3 mol Thus, 4(atomic mass of X) + 10(1.008) 54.3 atomic mass of X 11.1 This is closest to boron (B), which has an atomic mass of 10.8.

15 144 Chapter PV nrt or n PV RT 1 atm P 802 mm g 1.06 atm 760 mm g V 618 cm L L 1000 cm 3 T 75 C K n (1.06 atm)(0.618 L) ( L atm mol 1 K 1 )(348 K) mol gas n O2 20% of mol O 2 Number of O 2 molecules mol O x 1023 molecules 1 mol O 2 molecules 68. We are looking for the subscripts for C x y O z For every g of the compound, we have 48.6 g C 1 mol C g C 4.05 mol C 8.18 g 1 mol g 43.2 g O 1 mol O g O 8.12 mol 2.70 mol O 4.05 : 8.12 : : 3 : 1 3 : 6 : 2 The empirical formula is C 3 6 O 2, which has a molar mass of g/mol [3(12.01) + 6(1.008) + 2(16.00)] If we assume 1.00 L, we can solve for n n PV (1.00 atm)(1.00 L) RT ( L atm mol 1 K 1 )(150 o C + 273) 2.13 g molar mass 74.0 g/mol mol Thus, the molecular formula is C 3 6 O 2 Two possible Lewis structures include mol O O C C C O C C O C and

16 Gases ml 1 L 1000 ml PV nrt 2.00 mol Cl 1 L 1 mol 2 2 mol Cl mol 2 gas V nrt/p [(0.100 mol)( L atm/mol K)(298 K)]/(1.00 atm) 2.45 L The balloon will not pop since it can expand to 3.00 L and the hydrogen gas expands to a volume of 2.45 L at 1.00 atm and 25 o C. 70. a. PV nrt V n RT constant V 1 RT P n 1 P V 2 n 2 V 1 V 2 n 1 n 2 b. An increase in number of moles of gas increases the number of collisions with the container (if volume stays constant), which would increase the pressure (since pressure is due to collisions of gas particles with the walls of the container). In order for the pressure to remain constant, the volume must increase so that the distance the particles must travel increases and thus the collision rate overall stays the same (thus the pressure stays the same). Since temperature is a measure of the average kinetic energy of the particles, and changing the temperature would thus change the speed of the particles, the temperature must remain constant for this argument to hold. c g e 2.50 mol e 20.0 g Ar mol Ar V e 2.50 mol V Ar mol V e V Ar The container with e is 4.99 times as large as the container with Ar.

### 7. 1.00 atm = 760 torr = 760 mm Hg = 101.325 kpa = 14.70 psi. = 0.446 atm. = 0.993 atm. = 107 kpa 760 torr 1 atm 760 mm Hg = 790.

CHATER 3. The atmosphere is a homogeneous mixture (a solution) of gases.. Solids and liquids have essentially fixed volumes and are not able to be compressed easily. have volumes that depend on their conditions,

### Gas Laws. The kinetic theory of matter states that particles which make up all types of matter are in constant motion.

Name Period Gas Laws Kinetic energy is the energy of motion of molecules. Gas state of matter made up of tiny particles (atoms or molecules). Each atom or molecule is very far from other atoms or molecules.

### CHAPTER 12. Gases and the Kinetic-Molecular Theory

CHAPTER 12 Gases and the Kinetic-Molecular Theory 1 Gases vs. Liquids & Solids Gases Weak interactions between molecules Molecules move rapidly Fast diffusion rates Low densities Easy to compress Liquids

### 2. If pressure is constant, the relationship between temperature and volume is a. direct b. Inverse

Name Unit 11 Review: Gas Laws and Intermolecular Forces Date Block 1. If temperature is constant, the relationship between pressure and volume is a. direct b. inverse 2. If pressure is constant, the relationship

### Gas particles move in straight line paths. As they collide, they create a force, pressure.

#28 notes Unit 4: Gases Ch. Gases I. Pressure and Manometers Gas particles move in straight line paths. As they collide, they create a force, pressure. Pressure = Force / Area Standard Atmospheric Pressure

### Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten. Chapter 10 Gases

Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 10 Gases A Gas Has neither a definite volume nor shape. Uniformly fills any container.

### F321 MOLES. Example If 1 atom has a mass of 1.241 x 10-23 g 1 mole of atoms will have a mass of 1.241 x 10-23 g x 6.02 x 10 23 = 7.

Moles 1 MOLES The mole the standard unit of amount of a substance (mol) the number of particles in a mole is known as Avogadro s constant (N A ) Avogadro s constant has a value of 6.02 x 10 23 mol -1.

### The Gas Laws. Our Atmosphere. Pressure = Units of Pressure. Barometer. Chapter 10

Our Atmosphere The Gas Laws 99% N 2 and O 2 78% N 2 80 70 Nitrogen Chapter 10 21% O 2 1% CO 2 and the Noble Gases 60 50 40 Oxygen 30 20 10 0 Gas Carbon dioxide and Noble Gases Pressure Pressure = Force

### AS1 MOLES. oxygen molecules have the formula O 2 the relative mass will be 2 x 16 = 32 so the molar mass will be 32g mol -1

Moles 1 MOLES The mole the standard unit of amount of a substance the number of particles in a mole is known as Avogadro s constant (L) Avogadro s constant has a value of 6.023 x 10 23 mol -1. Example

### Sample Exercise 10.1 Converting Pressure Units

Sample Exercise 10.1 Converting Pressure Units (a) Convert 0.357 atm to torr. (b) Convert 6.6 10 2 torr to atmospheres. (c) Convert 147.2 kpa to torr. Solution Analyze In each case we are given the pressure

### Lecture Notes: Gas Laws and Kinetic Molecular Theory (KMT).

CHEM110 Week 9 Notes (Gas Laws) Page 1 of 7 Lecture Notes: Gas Laws and Kinetic Molecular Theory (KMT). Gases Are mostly empty space Occupy containers uniformly and completely Expand infinitely Diffuse

### CHEMISTRY. Matter and Change. Section 13.1 Section 13.2 Section 13.3. The Gas Laws The Ideal Gas Law Gas Stoichiometry

CHEMISTRY Matter and Change 13 Table Of Contents Chapter 13: Gases Section 13.1 Section 13.2 Section 13.3 The Gas Laws The Ideal Gas Law Gas Stoichiometry State the relationships among pressure, temperature,

### Gases. States of Matter. Molecular Arrangement Solid Small Small Ordered Liquid Unity Unity Local Order Gas High Large Chaotic (random)

Gases States of Matter States of Matter Kinetic E (motion) Potential E(interaction) Distance Between (size) Molecular Arrangement Solid Small Small Ordered Liquid Unity Unity Local Order Gas High Large

### Kinetic Molecular Theory

Kinetic Molecular Theory Particle volume - The volume of an individual gas particle is small compaired to that of its container. Therefore, gas particles are considered to have mass, but no volume. There

### Gas Laws. vacuum. 760 mm. air pressure. mercury

Gas Laws Some chemical reactions take place in the gas phase and others produce products that are gases. We need a way to measure the quantity of compounds in a given volume of gas and relate that to moles.

### Overview of Physical Properties of Gases. Gas Pressure

Overview of Physical Properties of Gases! volume changes with pressure! volume changes with temperature! completely miscible! low density gases: < 2 g/l liquids and solids: 1000 g/l Gas Pressure force

### Chapter 4 The Properties of Gases

Chapter 4 The Properties of Gases Significant Figure Convention At least one extra significant figure is displayed in all intermediate calculations. The final answer is expressed with the correct number

### The Gas Laws. The effect of adding gas. 4 things. Pressure and the number of molecules are directly related. Page 1

The Gas Laws Describe HOW gases behave. Can be predicted by the theory. The Kinetic Theory Amount of change can be calculated with mathematical equations. The effect of adding gas. When we blow up a balloon

### Kinetic Theory of Gases. 6.1 Properties of Gases 6.2 Gas Pressure. Properties That Describe a Gas. Gas Pressure. Learning Check.

Chapter 6 Gases Kinetic Theory of Gases 6.1 Properties of Gases 6.2 Gas Pressure A gas consists of small particles that move rapidly in straight lines. have essentially no attractive (or repulsive) forces.

### Exploring Gas Laws. Chapter 12. Solutions for Practice Problems. Student Textbook page 477

Chapter 12 Exploring Gas Laws Solutions for Practice Problems Student Textbook page 477 1. Problem At 19 C and 100 kpa, 0.021 mol of oxygen gas, O 2(g), occupy a volume of 0.50 L. What is the molar volume

### Exam 4 Practice Problems false false

Exam 4 Practice Problems 1 1. Which of the following statements is false? a. Condensed states have much higher densities than gases. b. Molecules are very far apart in gases and closer together in liquids

### Abbreviations Conversions Standard Conditions Boyle s Law

Gas Law Problems Abbreviations Conversions atm - atmosphere K = C + 273 mmhg - millimeters of mercury 1 cm 3 (cubic centimeter) = 1 ml (milliliter) torr - another name for mmhg 1 dm 3 (cubic decimeter)

### EXPERIMENT 15: Ideal Gas Law: Molecular Weight of a Vapor

EXPERIMENT 15: Ideal Gas Law: Molecular Weight of a Vapor Purpose: In this experiment you will use the ideal gas law to calculate the molecular weight of a volatile liquid compound by measuring the mass,

### General Properties of Gases. Properties of Gases. K is for Kelvin. C is for degrees Celsius. F is for degrees Fahrenheit PROPERTIES OF GASES GAS LAWS

PROPERTIES OF GASES or GAS LAWS 1 General Properties of Gases There is a lot of empty space in a gas. Gases can be expanded infinitely. Gases fill containers uniformly and completely. Gases diffuse and

### Physics Courseware Physics I Ideal Gases

Physics Courseware Physics I Ideal Gases Problem 1.- How much mass of helium is contained in a 0.0 L cylinder at a pressure of.0 atm and a temperature of.0 C? [The atomic mass of helium is 4 amu] PV (

### Temperature. Number of moles. Constant Terms. Pressure. Answers Additional Questions 12.1

Answers Additional Questions 12.1 1. A gas collected over water has a total pressure equal to the pressure of the dry gas plus the pressure of the water vapor. If the partial pressure of water at 25.0

### An increase in temperature causes an increase in pressure due to more collisions.

SESSION 7: KINETIC THEORY OF GASES Key Concepts In this session we will focus on summarising what you need to know about: Kinetic molecular theory Pressure, volume and temperature relationships Properties

### MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

Chapter 10 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) A gas at a pressure of 10.0 Pa exerts a force of N on an area of 5.5 m2. A) 1.8 B) 0.55

### Gases and Kinetic-Molecular Theory: Chapter 12. Chapter Outline. Chapter Outline

Gases and Kinetic-Molecular heory: Chapter Chapter Outline Comparison of Solids, Liquids, and Gases Composition of the Atmosphere and Some Common Properties of Gases Pressure Boyle s Law: he Volume-Pressure

### Force. Pressure = ; Area. Force = Mass times Acceleration;

Force Pressure = ; Area Force = Mass times Acceleration; If mass = kg, and acceleration = m/s 2, Force = kg.m/s 2 = Newton (N) If Area = m 2, Pressure = (kg.m/s 2 )/m 2 = N/m 2 = Pascal; (1 Pa = 1 N/m

### CHAPTER 12 GASES AND THEIR BEHAVIOR

Chapter 12 Gases and Their Behavior Page 1 CHAPTER 12 GASES AND THEIR BEHAVIOR 12-1. Which of the following represents the largest gas pressure? (a) 1.0 atm (b) 1.0 mm Hg (c) 1.0 Pa (d) 1.0 KPa 12-2. Nitrogen

### Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten. Chapter 10 Gases.

Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 10 The things we will cover in this chapter: How differ from solids and liquids Pressure,

### Gases. Macroscopic Properties. Petrucci, Harwood and Herring: Chapter 6

Gases Petrucci, Harwood and Herring: Chapter 6 CHEM 1000A 3.0 Gases 1 We will be looking at Macroscopic and Microscopic properties: Macroscopic Properties of bulk gases Observable Pressure, volume, mass,

### Substances that are liquids or solids under ordinary conditions may also exist as gases. These are often referred to as vapors. Properties of Gases

Common Student Misconceptions Students need to be told to always use Kelvin temperatures in gas problems. Students should always use units (and unit factor analysis) in gas-law problems to keep track of

### CHEMISTRY GAS LAW S WORKSHEET

Boyle s Law Charles Law Guy-Lassac's Law Combined Gas Law For a given mass of gas at constant temperature, the volume of a gas varies inversely with pressure PV = k The volume of a fixed mass of gas is

### Honors Chemistry. Chapter 11: Gas Law Worksheet Answer Key Date / / Period

Honors Chemistry Name Chapter 11: Gas Law Worksheet Answer Key Date / / Period Complete the following calculation by list the given information, rewriting the formula to solve for the unknown, and plugging

### The Mole. Chapter 10. Dimensional Analysis. The Mole. How much mass is in one atom of carbon-12? Molar Mass of Atoms 3/1/2015

The Mole Chapter 10 1 Objectives Use the mole and molar mass to make conversions among moles, mass, and number of particles Determine the percent composition of the components of a compound Calculate empirical

### ESSAY. Write your answer in the space provided or on a separate sheet of paper.

Test 1 General Chemistry CH116 Summer, 2012 University of Massachusetts, Boston Name ESSAY. Write your answer in the space provided or on a separate sheet of paper. 1) Sodium hydride reacts with excess

### Use each of the terms below to complete the passage. Each term may be used more than once.

Gases Section 13.1 The Gas Laws In your textbook, read about the basic concepts of the three gas laws. Use each of the terms below to complete the passage. Each term may be used more than once. pressure

### 4. Aluminum chloride is 20.2% aluminum by mass. Calculate the mass of aluminum in a 35.0 gram sample of aluminum chloride.

1. Calculate the molecular mass of table sugar sucrose (C 12 H 22 O 11 ). A. 342.30 amu C. 320.05 amu B. 160.03 amu D. 171.15 amu 2. How many oxygen atoms are in 34.5 g of NaNO 3? A. 2.34 10 23 atoms C.

### Chapter 13 Gases. An Introduction to Chemistry by Mark Bishop

Chapter 13 Gases An Introduction to Chemistry by Mark Bishop Chapter Map Gas Gas Model Gases are composed of tiny, widely-spaced particles. For a typical gas, the average distance between particles is

### Boyles Law. At constant temperature the volume occupied by a fixed amount of gas is inversely proportional to the pressure on the gas 1 P = P

Boyles Law At constant temperature the volume occupied by a fixed amount of gas is inversely proportional to the pressure on the gas 1 or k 1 Boyles Law Example ressure olume Initial 2.00 atm 100 cm 3

### 1. Which graph shows the pressure-temperature relationship expected for an ideal gas? 1) 3)

1. Which graph shows the pressure-temperature relationship expected for an ideal gas? 2. Under which conditions does a real gas behave most like an ideal gas? 1) at low temperatures and high pressures

### Type: Double Date: Kinetic Energy of an Ideal Gas II. Homework: Read 14.3, Do Concept Q. # (15), Do Problems # (28, 29, 31, 37)

Type: Double Date: Objective: Kinetic Energy of an Ideal Gas I Kinetic Energy of an Ideal Gas II Homework: Read 14.3, Do Concept Q. # (15), Do Problems # (8, 9, 31, 37) AP Physics Mr. Mirro Kinetic Energy

### CHAPTER 25 IDEAL GAS LAWS

EXERCISE 139, Page 303 CHAPTER 5 IDEAL GAS LAWS 1. The pressure of a mass of gas is increased from 150 kpa to 750 kpa at constant temperature. Determine the final volume of the gas, if its initial volume

### Version 001 HW04-Ideal Gas Laws, Gas Mixtures and KMT sparks (52100) 1

Version 001 HW04-Ideal Gas Laws, Gas Mixtures and KMT sparks (52100) 1 This print-out should have 15 questions. Multiple-choice questions may continue on the next column or page find all choices before

### 10. Gases. P= g h Pressure. Pressure is defined as the force across a unit area. Force N

0. Gases 0. ressure ressure is defined as the force across a unit area. Force N ascal, a Area m In chemistry, the SI unit for pressure, the ascal (a), is typically too small to be of practical use. Typically

### Chapter 13 Gases. Review Skills

Chapter 13 Gases t s Monday morning, and Lilia is walking out of the chemistry building, thinking about the introductory lecture on gases that her instructor just presented. Dr. Scanlon challenged the

### 5. Which temperature is equal to +20 K? 1) 253ºC 2) 293ºC 3) 253 C 4) 293 C

1. The average kinetic energy of water molecules increases when 1) H 2 O(s) changes to H 2 O( ) at 0ºC 3) H 2 O( ) at 10ºC changes to H 2 O( ) at 20ºC 2) H 2 O( ) changes to H 2 O(s) at 0ºC 4) H 2 O( )

### Temperature Measure of KE At the same temperature, heavier molecules have less speed Absolute Zero -273 o C 0 K

Temperature Measure of KE At the same temperature, heavier molecules have less speed Absolute Zero -273 o C 0 K Kinetic Molecular Theory of Gases 1. Large number of atoms/molecules in random motion 2.

### 1.23 Gas Calculations

1.23 Gas Calculations Gas calculations at A-level are done in two different ways although both link the volumes of a gas to the amount in moles of the gas. The same amount in moles of any gas will have

### Guide to Chapter 9. Gases Answers in green and red.

Guide to Chapter 9. Gases Answers in green and red. We will spend three lecture days on this chapter. Day 1. Pressure, barometers, STP, manometers, Charles Law, Boyles Law, Aogadro's Law, Combined Gas

### Chemistry 13: States of Matter

Chemistry 13: States of Matter Name: Period: Date: Chemistry Content Standard: Gases and Their Properties The kinetic molecular theory describes the motion of atoms and molecules and explains the properties

### Gas Density. Lift GOODYEAR. Goodyear blimp filled with He gas BADYEAR. Weight. Badyear blimp filled with Cl 2 gas

Gas Density Lift GOODYEAR Goodyear blimp filled with He gas BADYEAR Weight Badyear blimp filled with Cl 2 gas At STP( 1.00 atm, 273 K) 1.00 mole gas = 22.4 L Gas density: d = mass/volume = molar mass/molar

### IB Chemistry. DP Chemistry Review

DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount

### Name Class Date. In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question.

Assessment Chapter Test A Chapter: States of Matter In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. The kinetic-molecular

### Wed Sep 12, 2007 THE GASEOUS STATE

Chapter 5: Gases Gas Stoichiometry Partial Pressure Kinetic Theory Effusion and Diffusion Wed Sep 12, 2007 Exam #1 - Friday, Sep 14 Attendance is mandatory! Practice exam today in recitation Week 3 CHEM

### The Gas, Liquid, and Solid Phase

The Gas, Liquid, and Solid Phase When are interparticle forces important? Ron Robertson Kinetic Theory A. Principles Matter is composed of particles in constant, random, motion Particles collide elastically

### CHEM 120 Online Chapter 7

CHEM 120 Online Chapter 7 Date: 1. Which of the following statements is not a part of kinetic molecular theory? A) Matter is composed of particles that are in constant motion. B) Particle velocity increases

### Type: Single Date: Kinetic Theory of Gases. Homework: Read (14.1), Do CONCEPT Q. # (1), Do PROBLEMS # (2, 3, 5) Ch. 14

Type: Single Date: Objective: Kinetic Theory of Gases Homework: Read (14.1), Do CONCEPT Q. # (1), Do PROBLEMS # (2, 3, 5) Ch. 14 AP Physics Mr. Mirro Kinetic Theory of Gases Date Unlike the condensed phases

### Chapter 8: Gases and Gas Laws.

133 Chapter 8: Gases and Gas Laws. The first substances to be produced and studied in high purity were gases. Gases are more difficult to handle and manipulate than solids and liquids, since any minor

### Molar Mass of Butane

Cautions Butane is toxic and flammable. No OPEN Flames should be used in this experiment. Purpose The purpose of this experiment is to determine the molar mass of butane using Dalton s Law of Partial Pressures

### Gas Laws. E k = ½ (mass)(speed) 2. v101613_10am

Gas Laws v101613_10am Objective: In this lab you will become familiar with the Ideal Gas Law and Dalton s Law of Partial Pressures. You will be able to use the information collected along with stoichiometry

### A. Kinetic Molecular Theory (KMT) = the idea that particles of matter are always in motion and that this motion has consequences.

I. MOLECULES IN MOTION: A. Kinetic Molecular Theory (KMT) = the idea that particles of matter are always in motion and that this motion has consequences. 1) theory developed in the late 19 th century to

### 6 Evaluation of the Gas Law Constant

6 Evaluation of the Gas Law Constant Name: Date: Section: Objectives Measure the value of the gas constant R Use Dalton s Law to calculate the partial pressure of hydrogen in a closed container Learn to

### Bloom s Taxonomy. Study Habits and Study Resources: Pause. Expectations: Develop a working knowledge of the topics.

Dr. C. Weldon Mathews Chem 1 Office: 004 Evans Lab Telephone: 9-1574 email: mathews.6@osu.edu web: www.chemistry.ohio-state.edu/~mathews/ Office hours: TR 1:30 - :00 pm TR 4:00-5:00 pm or by appointment

### 1.4.6-1.4.8 Gas Laws. Heat and Temperature

1.4.6-1.4.8 Gas Laws Heat and Temperature Often the concepts of heat and temperature are thought to be the same, but they are not. Perhaps the reason the two are incorrectly thought to be the same is because

### 7. Gases, Liquids, and Solids 7.1 Kinetic Molecular Theory of Matter

7. Gases, Liquids, and Solids 7.1 Kinetic Molecular Theory of Matter Kinetic Molecular Theory of Matter The Kinetic Molecular Theory of Matter is a concept that basically states that matter is composed

### Chapter 3 Mass Relationships in Chemical Reactions

Chapter 3 Mass Relationships in Chemical Reactions Student: 1. An atom of bromine has a mass about four times greater than that of an atom of neon. Which choice makes the correct comparison of the relative

### Final Exam Review Questions PHY Final Chapters

Final Exam Review Questions PHY 2425 - Final Chapters Section: 17 1 Topic: Thermal Equilibrium and Temperature Type: Numerical 12 A temperature of 14ºF is equivalent to A) 10ºC B) 7.77ºC C) 25.5ºC D) 26.7ºC

### Molar Mass of Butane

Suggested reading: Chang 10 th edition text pages 175-201 Cautions Butane is toxic and flammable. No OPEN Flames should be used in this experiment. Purpose The purpose of this experiment is to determine

### Problem Solving. Stoichiometry of Gases

Skills Worksheet Problem Solving Stoichiometry of Gases Now that you have worked with relationships among moles, mass, and volumes of gases, you can easily put these to work in stoichiometry calculations.

### Name Date Class CHEMICAL QUANTITIES. SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296)

10 CHEMICAL QUANTITIES SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296) This section defines the mole and explains how the mole is used to measure matter. It also teaches you how to calculate

### Calculating Atoms, Ions, or Molecules Using Moles

TEKS REVIEW 8B Calculating Atoms, Ions, or Molecules Using Moles TEKS 8B READINESS Use the mole concept to calculate the number of atoms, ions, or molecules in a sample TEKS_TXT of material. Vocabulary

### Test 6: Phases of Matter Review Questions

Name: Wednesday, January 16, 2008 Test 6: Phases of Matter Review Questions 1. According to the kinetic theory of gases, which assumption is correct? 1. Gas particles strongly attract each other. 3. The

### CHEM 105 HOUR EXAM III 28-OCT-99. = -163 kj/mole determine H f 0 for Ni(CO) 4 (g) = -260 kj/mole determine H f 0 for Cr(CO) 6 (g)

CHEM 15 HOUR EXAM III 28-OCT-99 NAME (please print) 1. a. given: Ni (s) + 4 CO (g) = Ni(CO) 4 (g) H Rxn = -163 k/mole determine H f for Ni(CO) 4 (g) b. given: Cr (s) + 6 CO (g) = Cr(CO) 6 (g) H Rxn = -26

### 3-1 Copyright Richard M. Felder, Lisa G. Bullard, and Michael D. Dickey (2014)

EQUATIONS OF STATE FOR GASES Questions A gas enters a reactor at a rate of 255 SCMH. What does that mean? An orifice meter mounted in a process gas line indicates a flow rate of 24 ft 3 /min. The gas temperature

### Stoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2.

Stoichiometry 1 The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 01; (4) 02 2 A 44 gram sample of a hydrate was heated until the water of hydration was driven

### (1) The size of a gas particle is negligible as compared to the volume of the container in which the gas is placed.

Gas Laws and Kinetic Molecular Theory The Gas Laws are based on experiments, and they describe how a gas behaves under certain conditions. However, Gas Laws do not attempt to explain the behavior of gases.

### Chapter 5 Gases. August 2, 2009 [PROBLEM SET FROM R. CHANG TEST BANK] Student:

Chapter 5 Gases Student: 1. A pressure that will support a column of Hg to a height of 256 mm would support a column of water to what height? The density of mercury is 13.6 g/cm 3 ; the density of water

### Chemistry 110 Lecture Unit 5 Chapter 11-GASES

Chemistry 110 Lecture Unit 5 Chapter 11-GASES I. PROPERITIES OF GASES A. Gases have an indefinite shape. B. Gases have a low density C. Gases are very compressible D. Gases exert pressure equally in all

### Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test

Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test NAME Section 7.1 The Mole: A Measurement of Matter A. What is a mole? 1. Chemistry is a quantitative science. What does this term mean?

### The gas laws Equations of state The state of any sample of substance is specified by giving the values of the following properties: V the volume the

The gas laws Equations of state The state of any sample of substance is specified by giving the values of the following properties: V the volume the sample occupies p the pressure of the sample T the temperature

### 1. What is the molecular formula of a compound with the empirical formula PO and a gram-molecular mass of 284 grams?

Name: Tuesday, May 20, 2008 1. What is the molecular formula of a compound with the empirical formula PO and a gram-molecular mass of 284 grams? 2 5 1. P2O 5 3. P10O4 2. P5O 2 4. P4O10 2. Which substance

### MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

General Chemistry PHS 1015 Practice Exam 4 Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which of the following statements about pressure

### Metals Topic Test. Part 1: Multiple Choice Choose the best alternative and indicate your response on the answer sheet

Metals Topic Test Part 1: Multiple Choice Choose the best alternative and indicate your response on the answer sheet 1. The chemical equation for the reaction between aluminium and oxygen is: 4Al (s) +

### CHEMISTRY 113 EXAM 4(A)

Summer 2003 1. The molecular geometry of PF 4 + ion is: A. bent B. trigonal planar C. tetrahedral D. octahedral CHEMISTRY 113 EXAM 4(A) 2. The Cl-C-Cl bond angle in CCl 2 O molecule (C is the central atom)

### CHAPTER 8: CHEMICAL COMPOSITION

CHAPTER 8: CHEMICAL COMPOSITION Active Learning: 1-4, 6-8, 12, 18-25; End-of-Chapter Problems: 3-4, 9-82, 84-85, 87-92, 94-104, 107-109, 111, 113, 119, 125-126 8.2 ATOMIC MASSES: COUNTING ATOMS BY WEIGHING

### Chapter 3: Stoichiometry

Chapter 3: Stoichiometry Key Skills: Balance chemical equations Predict the products of simple combination, decomposition, and combustion reactions. Calculate formula weights Convert grams to moles and

### Chem 1A Exam 2 Review Problems

Chem 1A Exam 2 Review Problems 1. At 0.967 atm, the height of mercury in a barometer is 0.735 m. If the mercury were replaced with water, what height of water (in meters) would be supported at this pressure?

### PHYS-2010: General Physics I Course Lecture Notes Section XIII

PHYS-2010: General Physics I Course Lecture Notes Section XIII Dr. Donald G. Luttermoser East Tennessee State University Edition 2.5 Abstract These class notes are designed for use of the instructor and

### AP CHEMISTRY 2009 SCORING GUIDELINES (Form B)

AP CHEMISTRY 2009 SCORING GUIDELINES (Form B) Question 3 (10 points) 2 H 2 O 2 (aq) 2 H 2 O(l) + O 2 (g) The mass of an aqueous solution of H 2 O 2 is 6.951 g. The H 2 O 2 in the solution decomposes completely

### States of Matter CHAPTER 10 REVIEW SECTION 1. Name Date Class. Answer the following questions in the space provided.

CHAPTER 10 REVIEW States of Matter SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Identify whether the descriptions below describe an ideal gas or a real gas. ideal gas

### Chapter 10. Can You... 1. draw the Lewis structure for a given covalently bonded molecule?

Chapter 10 Can You... 1. draw the Lewis structure for a given covalently bonded molecule? e.g. SF 6 and CH 3 Cl 2. identify and count the number of non-bonding and bonding domains within a given covalently

### = 800 kg/m 3 (note that old units cancel out) 4.184 J 1000 g = 4184 J/kg o C

Units and Dimensions Basic properties such as length, mass, time and temperature that can be measured are called dimensions. Any quantity that can be measured has a value and a unit associated with it.

### CHEM 31 Introductory Chemistry EXAM #2 October 16, 2002

CHEM 31 Introductory Chemistry EXAM #2 October 16, 2002 Name: Keye, Onsur SSN: Lab T.A.: INSTRUCTIONS: Read through the entire exam before you begin. Answer all of the questions. For questions involving

### The concept of concentration exists to answer the question: How much of the stuff is there?

Concentrations and Other Units of Measure (Nazaroff & Alvarez-Cohen, Section 1.C.1) The concept of concentration exists to answer the question: How much of the stuff is there? Definition: The concentration