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| 9060890553 | What are the distinct characteristics of matter? | It has mass and it occupies space. | 0 | |
| 9060890554 | Describe the shape and volume of a solid. | Definite shape and definite volume. | 1 | |
| 9060890555 | How do the particles move in a solid? | The particles in a solid are packed tightly together and only vibrate gently around fixed positions. | 2 | |
| 9060890556 | Describe the shape and volume of a liquid. | Have no shape of their own but take the shape of their container. A liquid has a definite volume. | 3 | |
| 9060890557 | How do the particles move in a liquid? | The particles in a liquid are free to move. | 4 | |
| 9060890558 | Describe the shape and volume of gases. | Have neither a definite shape nor a definite volume. | 5 | |
| 9060890559 | How do the particles move in a Gas? | The particles in a Gas spread apart filling all the space of the container available to them. | 6 | |
| 9060890560 | Solids fall broadly into how many categories? | Two | 7 | |
| 9060890561 | What are the categories that solids broadly fall into? | Crystalline And a amorphous | 8 | |
| 9060890562 | Define crystalline. | Where a regular, ordered, repeatable 3-D Structure of particles is found. | 9 | |
| 9060890563 | Define amorphous. | Where the arrangement of particles is not regular or ordered. | 10 | |
| 9060890564 | Describe the movement of particles in the solids as crystalline or amorphous. | In both cases, the particles in the solid have very little energy and move very little in relation to one another. They are sometimes described as 'vibrating around fixed positions.' | 11 | |
| 9060890565 | Describe the movement of particles in liquids. | Particles in liquids are constantly moving and colliding with one another, have significantly greater energy and move a lot in relation to one another. | 12 | |
| 9060890566 | Since solids and liquids tend to have their particles very close together. Their volumes are often very similar. What does this mean? | They have strong forces of attraction. | 13 | |
| 9060890567 | ***Since, in a Gas, the particles possess enough energy to overcome any intermolecular forces and hence move around completely freely and with large spaces between them, a liquid represents particles in an intermediate state between the extremely ordered and low energy state of a solid, and the extremely disordered and high energy state of a Gas.*** | 14 | ||
| 9060890568 | All the properties of solids and liquids such as viscosity, surface tension, hardness etc., are dependent upon what? | 1. How the particles that make up the solid or liquid are arranged 2. The extent of the attractions between those particles | 15 | |
| 9060890569 | Define viscosity. | Thickness- resistance to motion | 16 | |
| 9060890570 | Gases are made up of particles that have what kind of energy? | (Relatively) large amounts | 17 | |
| 9060890571 | A Gas has no definite ___________________ and will expand to ______________? | Shape or volume; fill as much space as possible | 18 | |
| 9060890572 | As a result of the large amount of empty space in a volume of gas, gases are ____________________? | Easily compressed | 19 | |
| 9060890573 | A pressure is what? | Exerted when the gas particles collide with the walls of any container it is held in. | 20 | |
| 9060890574 | ***1.00 atm= 760. mmHg= 760. Torr*** ON EQUATION TABLE | 21 | ||
| 9060890575 | Convert 657 mmHg to atm | 0.864 atm | 22 | |
| 9060890576 | Convert 830 torr to atmospheres | 1.09 atm | 23 | |
| 9060890577 | What is the basis for many properties of gases? | The Kinetic molecular theory | 24 | |
| 9060890578 | What are the five postulates of the Kinetic molecular theory? | 1. Gases are composed of tiny particles (atoms or molecules) whose size is negligible compared to the average distance between them; the total volume that the gas fills is almost all empty space; the observation that gases are compressible. 2. The gas particles move randomly, in straight lines, in all directions and at various speeds. 3. The forces of attraction or repulsion between two gas particles are negligible, except when they collide. 4. When particles collide with one another, the collisions are elastic. The collisions with the walls of the container create the gas pressure. Elastic collisions do not spontaneously convert to the liquid. 5. The average kinetic energy of a molecule is proportional to the Kelvin temperature and as a result, all calculations involving gases should be carried out with temperatures converted to K. | 25 | |
| 9060890579 | ***These assumptions do have limitations. For example, gases can be liquified if cooled enough. This means "real" gas particles do attract one another to some extent; otherwise the particles would never stick to one another and therefore never condense to form a liquid.*** | 26 | ||
| 9060890582 | What does Boyle's Law state? | At constant temperature, pressure is inversely proportional to volume. This means that as the pressure increase the volume decreases and vice versa. |  | 27 |
| 9060890583 | What is the relationships with Boyle's Law? | Pressure and volume |  | 28 |
| 9060890584 | For Boyle's Law, if the volume is increased, the gas particles ______________? | Collide with the walls of the container less often and the pressure is reduced. | 29 | |
| 9060890586 | What is the equation for Boyle's Law? | P1V1=P2V2 | 30 | |
| 9060890587 | What is a real-world example of Boyle's Law? | Squeeze ballon | 31 | |
| 9060890588 | If a 1.23L sample of a Gas at 53.0 torr is put under pressure up to a value of 240. Torr at a constant temperature, what is the new volume? | 0.272L | 32 | |
| 9060890589 | The pressure on a 411mL sample of gas is decreased from 812mmHg to 790mmHg. What will the new volume of the gas be? | 422mL | 33 | |
| 9060890590 | What does Charles' Law state? | At constant pressure, volume is directly proportional to temperature. | 34 | |
| 9060890591 | What are the relationships with Charles' Law? | Volume and temperature | 35 | |
| 9060890592 | For Charles' Law, what does the constant equal? | V/T |  | 36 |
| 9060890593 | For Charles' Law, if the temperature is increased the gas particles ______________ kinetic energy, ________________? | Gain; move around move and occupy more space | 37 | |
| 9060890594 | What is the equation for Charles' Law? | V1/T1=V2/T2 | 38 | |
| 9060890595 | An 11.0L sample of a Gas is collected at 276K and then cooled by 14K. The pressure is held constant at 1.20atm. Calculate the new volume of the gas. | 10.4L | 39 | |
| 9060890596 | A Gas has volume of 0.572L at 35.0C and 1.00atm pressure. What is the temperature inside a container where this gas has a volume of 0.535L at 1.00atm? | 288K | 40 | |
| 9060890597 | What is the relationship between Avogadro's Law? | Volume and moles | 41 | |
| 9060890598 | For Avogadro's Law, what does a constant equal? | V/n | 42 | |
| 9060890599 | What is the equation for Avogadro's Law? | V1/n1=V2/n2 | 43 | |
| 9060890600 | What does Avogadro's Law state? | At constant temperature and pressure, volume is directly proportional to the number of moles of gas present. This means that the volume of a gas increases with increasing number of moles, and vice versa. |  | 44 |
| 9060890601 | A 13.1L sample of 0. 502 moles of 02 is held under conditions of 1.00atm and 25C. If all of the O2 is then converted to ozone (O3) what will be the volume of ozone? | 8.74L | 45 | |
| 9060890602 | If 2.11g of neon gas occupies a volume of 12.0L at 28.0C. What volume will 6.58g of neon occupy under the same conditions? | 37.3L | 46 | |
| 9060890603 | What is the relationship between Gay-Lussac's Law? | Pressure and temperature |  | 47 |
| 9060890604 | For Gay-Lussac's Law, what is the constant? | P/T | 48 | |
| 9060890605 | What is the equation for Gay-Lussac's Law? | P1/T1=P2/T2 | 49 | |
| 9060890606 | What does Gay-Lussac's Law state? | At constant volume, pressure is directly proportional to temperature. This means that temperature increases with increasing pressure, and vice versa. | 50 | |
| 9060890607 | A Gas at 25C In a closed container has its pressure raised from 150. atm To 160. atm. What is the final temperature of the gas? | 318K | 51 | |
| 9060890608 | A Gas exerts a pressure of 900mmHg at 20C. What temperature would be required to lower the pressure to 1.00atm? | 247K | 52 | |
| 9060890609 | ***REVIEW GRAPHS IN NOTES OF BOYLE'S AND CHARLE'S LAW*** | 53 | ||
| 9060890610 | How proportional is Boyle's Law? | Inversely proportional between volume and pressure | 54 | |
| 9060890611 | How proportional is Charles' Law? | Directly proportional between temperature and volume | 55 | |
| 9060890612 | What happens to all random motion? | It ceases. | 56 | |
| 9060890613 | What happens when all random motion ceases? | It cannot be attained. |  | 57 |
| 9060890614 | What is the equation for general and combined gas equations? | P1V1/n1T1=P2V2/n2T2 | 58 | |
| 9060890615 | If the number of moles of a Gas in an experiment is constant (frequently the case), what is the equation? | P1V1/T1=P2V2/T2 | 59 | |
| 9060890616 | The combination of Laws above leads to the formulation of the ________________? | Ideal gas law |  | 60 |
| 9060890617 | What is the equation for the ideal gas law? | PV=nRT | 61 | |
| 9060890618 | For the ideal gas law, describe the particles. | They do not attract one another (they act independently) | 62 | |
| 9060890619 | What is the universal gas constant (R)? | 0.0821 L atm K^-1 mol^-1 | 63 | |
| 9060890620 | What does n equal in the PV=nRT equation? | mass/molar mass= g/g/mol= mol | 64 | |
| 9060890621 | ***What is the equation you must have memorized for pressure?*** | P=densityRT/molar mass | 65 | |
| 9060890622 | Assuming ideal behavior, how many moles of helium gas are in a sample that has a volume of 8.12L at a temperature of 0.00C and a pressure of 1.20 atm? | 0.435mol | 66 | |
| 9060890623 | A sample of aluminum chloride weighing 0.100g was vaporized at 350.C and 1.00atm pressure to produce 19.2mL of vapor. Calculate a value for the molar mass of aluminum chloride. | 267g/mol | 67 | |
| 9060890624 | What does Dalton's Law state? | In a mixture of ideal gases the total pressure exerted by the mixture is equal to the sum of the individual partial pressures of each Gas. | 68 | |
| 9060890625 | What is the equation for Dalton's Law? | Ptotal= P1+P2+P3 etc. |  | 69 |
| 9060890626 | Calculate the number of moles of hydrogen present, in a 0.641L mixture of hydrogen and water vapor, at 21C, that has a total pressure of 750. Torr, given that the vapor pressure of water at this temperature is 20.0 torr. | 0.0255mol | 70 | |
| 9060890627 | 3.00L of Carbon monoxide gas at a pressure of 199. kPa, And 1.00L of carbon dioxide gas at a pressure of 300. kPa are injected into a 1.25L container. Assuming no reaction between the two gases, what is the total pressure in this container? | 717.6kPa | 71 | |
| 9060890628 | At ______________________ gas particles come close enough to one another to make the two postulates of the Kinetic molecular theory invalid. | High pressures and low temperatures | 72 | |
| 9060890629 | ***High pressures and low temperatures experience ________________ and are _________________?*** | ***Induced dipoles; polarizable (see picture on Dingle Notes)*** | 73 | |
| 9060890630 | Engineers/scientists can't use PV=nRT at high pressure to predict __________________? Answers would be __________________? | Properties of gases; incorrect |  | 74 |
| 9060890631 | What is the assumption that gases are composed of tiny particles? | Whose size is negligible. | 75 | |
| 9060890632 | ***When the gas is pressurized into a small space that gas particles size becomes _________________?*** | More significant compared to the total volume. | 76 | |
| 9060890633 | ***The Assumption that the forces of attraction or repulsion between two particles in a Gas are very weak or negligible begins to fail. — Low temperature means less energy, so the particles are attracted to one another more*** — What does this mean? | Temporary induced dipoles! | 77 | |
| 9060890634 | Under these conditions (high P and low T), gases are said to behave non-ideally or like 'real' gases. This has two consequences which are? | 1. The real gas situation necessitates the need to correct the volume by subtracting a factor. 2. The observed pressure is less than in an ideal gas. | 78 | |
| 9060890635 | In Van Der Waals equation, what does the a stand for? | Relatively strong inter particle attractions for one another would have corresponding relatively large values (intermolecular forces) | 79 | |
| 9060890636 | In Van Der Waals equation, what does the b stand for? | Relatively large gas particles would have correspondingly relatively large values since they take up a larger volume (volume) | 80 | |
| 9060890637 | HCl vs. NH3— where would the attraction be closer? | HCl: 36 g/mol NH3: 17 g/mol Closer to HCl because NH3 is lighter & travels faster | 81 | |
| 9060890638 | N2 vs. O2— Where would the attraction be closer? | N2: 28g O2: 32g Closer to O2 because N2 is lighter and travels faster. | 82 | |
| 9060890639 | The root-mean-square-speed of the velocities of gas particles is _______________? | The square root of the averages of the square of the speeds of all the particles a sample at a particular temperature | 83 | |
| 9060890640 | What is the equation for the root mean square speed? | Urms = _/3RT/M | 84 | |
| 9060890641 | What must the R be in the root mean square speed equation? | 8.314kgm^2/s^2molK | 85 | |
| 9060890642 | What must the molar mass be for the root mean square speed? | In kilograms | 86 | |
| 9060890643 | What can be said about the Urms of a gas in relation to its molar mass and in relation to its temperature? | The higher the molar mass, the Urms should be lower because it is heavier. The higher the temperature, the more kinetic energy. | 87 | |
| 9060890644 | Effusion is _________________? | The process in which a gas escapes from one vessel to another by passing through a very small opening. | 88 | |
| 9060890645 | Diffusion is ________________? | The process by which a homogenous mixture is formed by the random mixing of two different gases. | 89 | |
| 9060890646 | Rate of effusion A/Rate of effusion B equals what? | _/density of B/density of A OR _/Molar mass of B/Molar mass of A | 90 | |
| 9060890647 | For Henry's Law, at higher pressures more gas particles strike the surface of the solution and enter the solution, meaning ___________________? | The concentration of the gas dissolved in the solvent is greater. | 91 | |
| 9060890648 | Henry's Law example: Coke bottles under ____________ pressure, ___________ carbonation CO2 (g) | High; more | 92 | |
| 9060890649 | For Henry's Law, Gas solubility usually ________________ with increase of temperature of the solution. | Decreases | 93 | |
| 9060890650 | Henry's Law example: low temperature equals ____________? | More carbonate. | 94 | |
| 9060890651 | How much faster is H2 than CO? | 3.72 (no units) | 95 | |
| 9060890652 | For Henry's Law, if the answer is greater than one ________________? | Then the first in the problem is lighter, faster than the second element/compound in the problem. | 96 | |
| 9060890653 | For Henry's Law, if the answer is less than one ______________? | Then the first in the problem is heavier, slower than the second element/compound in the problem. | 97 | |
| 9060890654 | For Henry's Law, if the answer is equal than one ______________? | Then the elements/compounds in both of the problem share the same speed and mass. | 98 | |
| 9060890655 | For Henry's Law, what is the direct proportion? | Pressure and solubility. | 99 | |
| 9060890656 | In regards to Henry's Law, what is true of higher pressure in the balanced equation: CO2 + H2O —> H2CO3 | - higher pressure - solubility of a gas increases - CO2 is dissolved in H2O to get carbonic acid | 100 | |
| 9060890657 | In regards to Henry's Law, what is true of lower pressure in the balanced equation: CO2 + H2O —> H2CO3 | - lower pressure - solubility of a gas decreases - CO2 is NOT dissolved in H2O to get carbonic acid | 101 | |
| 9060890658 | For Henry's Law, what is the inverse proportion? | Temperature and solubility. | 102 | |
| 9060890659 | In regards to Henry's Law, what is true of higher temperature in the balanced equation: CO2 + H2O —> H2CO3 | - higher temperature - solubility of a gas decreases - CO2 leaves (rises up and out) | 103 | |
| 9060890660 | In regards to Henry's Law, what is true of lower temperature in the balanced equation: CO2 + H2O —> H2CO3 | - lower temperature - solubility of a gas increases - CO2 remains (stays) | 104 | |
| 9060890661 | Higher altitude equals ________________? | Less pressure, less molecules | 105 | |
| 9060890662 | Lower altitude equals ________________? | Higher pressure, more molecules | 106 | |
| 9060890663 | Ne- 20g/mol Xe- 131g/mol Cl2- 70g/mol HCl- 36g/mol He- 4g/mol What method do you use to solve this? | Lighter=faster Heavier=slower | 107 | |
| 9060890664 | What are the postulates of the Kinetic molecular theory? | 1. High energy - never lose with collisions - collisions cause P 2. ID of gas doesn't matter - small 3. Much empty space - that's why compressible! 4. No attraction/repulsion between particles 5. Average kinetic energy ~ proportional to Kelvin temperature | 108 | |
| 9060890665 | For temporary induced dipoles with London dispersion forces (attractions), what is the OPPOSITE of the Kinetic molecular theory postulates? | 1. Volume - NO empty space - not compressible 2. Pressure - GREAT AMOUNT of attraction/repulsion between particles (High pressure, low temperature) | 109 | |
| 9060890666 | ***If two elements are at the same temperature, using the equation T=KE=1/2mv^2*** | 110 | ||
| 9060890667 | T=KE=1/2mv^2 A: 20=1/2(10)(2) B: 20=1/2(4)(3.16) Which has the highest KE? Which has the highest velocity? | A: heavier, slower B: lighter, faster | 111 | |
| 9060890668 | ***Review Manometer*** | 112 | ||
| 9060890669 | Steps with manometer? | 1. Make sure the height is in MILLIMETERS (mm) 2. Once the height is in mm, convert it to ATM. 3. If the gas pressure is more than the pressure outside, then add the given atmospheric pressure to the height. 4. If the gas pressure is less than the pressure outside, then subtract the height from the given atmospheric pressure. 5. If the tube is closed, the pressure of the gas is equal to the height of the mercury column, therefore, just convert to atmospheres and that is your answer. | 113 | |
| 9060890670 | What does n equal in the PV=nRT equation? | mass/molar mass= g/g/mol= mol | 114 | |
| 9060890671 | ***What is the equation you must have memorized for pressure?*** | P=densityRT/molar mass | 115 | |
| 9060890672 | Assuming ideal behavior, how many moles of helium gas are in a sample that has a volume of 8.12L at a temperature of 0.00C and a pressure of 1.20 atm? | 0.435mol | 116 | |
| 9060890673 | A sample of aluminum chloride weighing 0.100g was vaporized at 350.C and 1.00atm pressure to produce 19.2mL of vapor. Calculate a value for the molar mass of aluminum chloride. | 267g/mol | 117 | |
| 9060890674 | What does Dalton's Law state? | In a mixture of ideal gases the total pressure exerted by the mixture is equal to the sum of the individual partial pressures of each Gas. | 118 | |
| 9060890675 | What is the equation for Dalton's Law? | Ptotal= P1+P2+P3 etc. | 119 | |
| 9060890676 | Calculate the number of moles of hydrogen present, in a 0.641L mixture of hydrogen and water vapor, at 21C, that has a total pressure of 750. Torr, given that the vapor pressure of water at this temperature is 20.0 torr. | 0.0255mol | 120 | |
| 9060890677 | 3.00L of Carbon monoxide gas at a pressure of 199. kPa, And 1.00L of carbon dioxide gas at a pressure of 300. kPa are injected into a 1.25L container. Assuming no reaction between the two gases, what is the total pressure in this container? | 717.6kPa | 121 | |
| 9060890678 | At ______________________ gas particles come close enough to one another to make the two postulates of the Kinetic molecular theory invalid. | High pressures and low temperatures | 122 | |
| 9060890679 | ***High pressures and low temperatures experience ________________ and are _________________?*** | ***Induced dipoles; polarizable (see picture on Dingle Notes)*** | 123 | |
| 9060890680 | Engineers/scientists can't use PV=nRT at high pressure to predict __________________? Answers would be __________________? | Properties of gases; incorrect | 124 | |
| 9060890681 | For halogens, what is fluorine? | Gas and pale green | 125 | |
| 9060890682 | For halogens, what is chlorine? | Gas and yellow/green | 126 | |
| 9060890683 | For halogens, what is bromine? | Liquid and brown/orange | 127 | |
| 9060890684 | For halogens, what is iodine? | Solid and purple/black | 128 | |
| 9060890685 | The heavier the elements get, the _______________. | More polarizable they are which is why they change states. | 129 |
