Unit 9 Phases of Matter: Cold is but a State of Mind

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1 Key Understandings: 1. Know the difference between an open, closed and isolated systems. 2. Know the difference between heat and temperature. 3. Know that pressure as well as temperature is the determining factors for the phase/state of matter. 4. Know how to define and use the terms/symbols for: a. Specific Heat Capacity (CP) b. Heat of Fusion (HFUS) c. Heat of Vaporization (HVAP) 5. Known how the energy (kinetic and potential) of the particles of a substance changes when heated, cooled or undergoing changes in phase. 6. Know the characteristics and differences of an ideal versus a real gas. 7. Know and know when to apply eitheir the Ideal Gas law (PV=nRT), the Combined Gas law (P1V1/T1 = P2V2/T2), Avogadro s law (n1/v1 = n2/v2) or Dalton s law of Partial Pressure (PT = P1 + P2 + P3 + ) to experimental data. 8. Know how to use the Combined Gas law (P1V1/T1 = P2V2/T2) to drive component equations when one type of variable is held constant. 11 Unit 9: Day 4 Sheet: Gasses; Kinetic Molecular Theory of Gasses; Diffusion vs. Effusion; deal Gases; Real vs. ideal Gasses; Temp in Gas Laws; Standard Pressure; Gas Laws; -U: 6, 7 -A: 3, 6, 7 HW: 9.G & 9.H Unit 9 Phases of Matter: Cold is but a State of Mind and Abilities: 1. Be able to state the key postulates of the KMT. Note: This is a tentative schedule and subject to change based upon student feedback. 12 Unit 9: Day 5 Sheet: Temp in Gas Laws; The Gas Constant, R, in Various Units; Standard Pressure; Gas Laws; Dalton s Law of Partial Pressure -U: 7, 8 -A: 3, 6, 7 HW: 9.I, 9. J 6 Unit 9: Day 1 Sheet: KMT and the Phases of Matter; 3 Things about Energy; Heat vs. Temperature; Temperature; Importance of ; Phase Diagrams, -U: 1, 2, 3, 4, 5 -A: 1, 2, 3, 4 HW: 9.A, 9.B, 9.C 13 Unit 9: Day 6 -Alternative Calculations Lab -DUE END OF PERIOD. NO EXCEPTIONS. -U: 2, 4, 7, 8 -A: 3, 4, 5, 6, 7 Due: Unit 9 NB Check J, No Vocab This Unit 2. Be able to use a phase diagram to determine the phase, boiling point, melting point and the triple point of a material at a given temperature and pressure. 3. Be able to convert from C to K. 4. Be able to complete calorimetric calculations of: q = m CP T, q = m HFUS, q = m HVAP, and qlost = (-qgain), including phase changes, using laboratory data. 5. Be able to interpret and draw heating and cooling curves (noting both significance of plateaus and the physical states of each segment). 6. Be able to convert between equivalent units of pressure (torr, mmhg, atm, kpa) using dimensional analysis. 7. Be able to apply the Ideal Gas law (PV=nRT), the Combined Gas law (P1V1/T1 = P2V2/T2), Avogadro s law (n1/v1 = n2/v2) and Dalton s law of Partial Pressure (PT = P1 + P2 + P3 + ) given experimental data. 7 Unit 9: Day 2 Sheet: Calorimetry -U: 1, 2, 3, 4, 5 -A: 1, 2, 3, 4 HW: 9.D Unit 9: Day 7 -Unit Test 14 No Vocab due to Mr. Butryn s Schedule Hint Hint. The perfect study guide is here. Do you understand these key points? Can you do these things? 8 Unit 9: Day 3 Sheet: Calorimetry; Heat and Cooling Curves. -U: 2, 4, 5 -A: 3, 4, 5 HW: 9.E & 9.F Unit 10: Day 1 -Unit Test 15 No Vocab due to Mr. Butryn s Schedule Absolute Temperature Absolute Zero Condensation Critical Point Heat Kelvin Kinetic Energy Kinetic Molecular Theory Day 1 Vocab This is a temperature reading made relative to absolute zero. We use the unit of Kelvins for these readings. This is the lowest temperature possible of 0 K. Remember that temperature is the measurement molecular movement; you can guess that they stop moving entirely at absolute zero. In reality, bonds still vibrate a little bit, but for the most part you don't see much happening. When a vapor reforms a liquid. This is what happens on your bathroom mirror when you take a shower. The end point of the liquid-vapor line in a phase diagram. Past the critical point, you get something called a "supercritical liquid", which has weird properties. The form of energy that moves spontaneously from a warmer object to a less warm one. Heat flows where it is hot to where it is not A unit used to measure temperature. One Kelvin is equal in size to one degree Celsius. To convert between degrees Celsius and Kelvins, simply add to the temperature in degrees Celsius to get Kelvins. Energy of motion or the energy an object has because of its mass and velocity; the kinetic energy of a moving body is measured in joules. Objects that are not moving have no kinetic energy. Theory that assumes that all matter consists of continuously moving molecules of negligible size. Normal boiling point Normal melting point Phase Phase Boundary Phase Diagram Phase Equilibrium Potential Energy Pressure Sublimation System Temperature Triple point: Vaporization The boiling point of a substance at 1.00 atm. The melting point of a substance at 1.00 atm. A physically distinctive form of matter, such as a solid, liquid, gas or plasma. AKA the state of matter. The line on a phase diagram that indicated that more than one phase is present under the conditions of temperature and pressure indicated and a phase change is possible due to any shift in these conditions. A chart showing how phase depends on the equilibrium between pressures and temperatures. Coexistence of phases in thermodynamic equilibrium with one another in a system consisting of two or more phases. Stored energy due to its composition or position; the stored energy of an object may only be measured when it is released. Force exerted by molecular collision per unit area. When a solid can change directly into a gas. Dry ice does this The part of the universe being studied, while the surroundings are the rest of the universe that interacts with the system. The average kinetic energy of a system. A scale of particle motion from 0 to something when measuring temperature in Kelvins. The temperature and pressure at which all three states of a substance can exist in equilibrium. When you boil a liquid.

2 Calorimetry Specific Heat Capacity Heat of Fusion Heat of Vaporization Avogadro's Law Boyle's Law Charles's Law Dalton's Law of Partial Pressures Diffusion Day 2 Vocab The study of heat flow. The amount of heat required to increase the temperature of one gram of a substance by one degree dependent on phase. Symbol is (CP) Day 3 Vocab The energy required to transition one g of a substance between the solid to the liquid state at a constant temperature and pressure. The energy required to transition one g of a substance between the liquid to the gas state at a constant temperature and pressure. Day 4 Vocab If you've got two gases under the same conditions of temperature, pressure, and volume, they've got the same number of particles (atoms or molecules). This law only works for ideal gases, none of which actually exist. The volume of a gas at constant temperature varies inversely with pressure. In other words, if you put big pressure on something, it gets small. The volume of a gas at constant pressure is directly proportional to the temperature. In other words, if you heat something up, it gets big. The total pressure in a mixture of gases is equal to the sums of the partial pressures of all the gases put together. When particles move from areas of high concentration to areas of low concentration. For example, if you open a bottle of ammonia on one end of the room, the concentration of ammonia molecules in the air is very high on that side of the room. As a result, they tend to migrate across the room, which explains why you can smell it after a little while. Be careful not to mix this up with effusion Effusion Ideal gas: Partial Pressure Real gas: Standard Temperature Pressure: Gas Constant and When a gas moves through an opening into a chamber that contains no or less pressure. Effusion is much faster than diffusion because there are no other gas molecules to get in the way. A gas in which the particles are infinitely small, have a kinetic energy directly proportional to the temperature, travel in random straight lines, and don't attract or repel each other. Needless to say, there's no such thing as an ideal gas in the real world. However, we use ideal gases anyway because they make the math work out well for equations that describe how gases behave. The pressure of one gas in a mixture. For example, if you had a 50:50 mix of helium and hydrogen gases and the total pressure was 2 atm, the partial pressure of hydrogen would be 1 atm. A gas in which the particles are small but occupy space, have an individual kinetic energy, travel unpredictable, and are affected by IMF s. Do not cover at this level as we would need to consider the impact of their individual volume, distance between particles and resulting affect of IMF s.fun right? One atmosphere and K. Usually denoted as STP. Day 5 Vocab Constant derived from the ideal gas equation, PV = nrt whose value varies based on the units associated with it. Unit 9 Formula Reference q = m Cp ΔT q = m P1 V1 HFUS = P2 V2 V1 = q = m T1 T2 HVAP n1 V2 n2 P V = n R T PT = P1 + Pn + 9.A Calorimetry: Basics Instructions: Provide a response for each question that is well thought out, satisfies the prompt, is clearly explained, and LEGIBLE. 1. In a closed system what basic fact must always hold true for the energy content of the overall system? 2. What is the difference between heat and temperature, including units and symbol? 3. What property and two conditions determine the phase of a sample of matter is? 9.B Calorimetry: Temperature Conversions and Calculations Instructions: ON A SEPARATE SHEET, convert C to K or vice versa.. Remember, Sig Figs, NW = NC, Boxed Answers and N 3 (this includes C K K C C C K K Instructions: ON A SEPARATE SHEET, calculate the change in temperature ( ΔT ) from the following data. Remember, Sig Figs, NW = NC, Boxed Answers and N C to 12.4 C C to C C to 49.0 C C to C

3 9.C Calorimetry: Phase Diagrams Instructions: Answer the question 1 9 in relation to the following phase diagram. Remember N 3 1. Which letter denotes the solid phase? 2. Which letter denotes the liquid phase? 3. Which letter denotes the gas phase? 4. Which letter denotes the triple point? In your own words, what is the definition of a triple point? 5. What is the melting point at 1 atm of pressure? 6. What is the boiling point at 1 atm of pressure? 7. Above what temperature is it impossible to liquefy this substance, no matter what the pressure? 8. At what temperature and pressure do all three phases coexist? 9. At a constant temperature, what would you do to cause this substance to change from the liquid phase to the solid phase? Instructions: Refer to the phase diagram below when answering the questions NOTE: Normal refers to 1.0 atm and remember N What are the values for temperature and pressure at STP? T=, P= 11. What is the normal freezing point of this substance? normal boiling point of this substance? normal melting point of this substance? 12. What is the phase (s, l, g) of a substance at 2.0 atm and 100 C? 13. What is the phase (s, l, g) of a substance at 0.75 atm and 100 C? 14. What is the phase (s, l, g) of a substance at 0.5 atm and 100 C? 15. What is the phase (s, l, g) of a substance at 1.5 atm and 50 C? 16. What is the phase (s, l, g) of a substance at 1.5 atm and 200 C? 17. What is the phase (s, l, g) of a substance at 1.5 atm and 800 C? 18. What is the condition of the triple point of this substance? T=, P= 19. A sample was at an initial pressure of 1.25 atm and a temperature of C and was lowered to a pressure of 0.25 atm, what phase transition(s) would occur? 20. A sample was at an initial pressure of 0.5 atm and a temperature of C was lowered to a temperature of C, what phase transition(s) would occur? 21. If this substance was at a pressure of 2.0 atm, at what temperature would it melt? boil? 22. If this substance was at a pressure of 0.75 atm, at what temperature would it melt? boil? 23. At what temperature do the gas and liquid phases become indistinguishable from each other? 24. At what pressure would it be possible to find this substance in the gas, liquid, and solid phase? 25. If I had a quantity of this substance at a pressure of 1.00 atm and a temperature of C, what phase change(s) would occur if I increased the temperature to C? At what temperature(s) would they occur? (NOTE: multiple answers needed for this question) 9.D Calorimetry: Calometric Calculations Instructions: ON A SEPARATE SHEET OF PAPER, identify the values and symbols of all variables present within the following data. Be sure to denote the unknown variable, what you need to solve for, as = x and/or y. Variables to denote in each include Ti, Tf, ΔT, Cp, m, and q. 1. A sample of mercury is heated from 25.5 C to 52.5 C. In the process, 3050J of heat are absorbed. What mass of mercury was in the sample? The specific heat of mercury is J/g C. 3. A cube of gold with a mass of g is heated from 30.0 C to some higher temperature with the absorption of 921 J of heat. The specific heat of gold is J/g C. What is the final temperature of the gold? 2. A block of aluminum with a mass of 140g is cooled from 98.4 C to 62.2 C with a release of 1137J of heat. From this data, calculate the specific heat of aluminum. 4. A total of 226 J of heat are absorbed as 58.3 g of lead is heated from 12.0 C to 42.0 C. From this data, what is the specific heat of lead?

4 9.D Calorimetry: Calometric Calculations Instructions: ON A SEPARATE SHEET OF PAPER, preform the following calorimetric calculations. Remember, Sig Figs, NW = NC, Boxed Answers and N 3 (this includes 5. A sample of mercury is heated from 25.5 C to 52.5 C. In the process, 3050J of heat are absorbed. What mass of mercury was in the sample? The specific heat of mercury is J/g C. 6. A block of aluminum with a mass of 140g is cooled from 98.4 C to 62.2 C with a release of 1137J of heat. From this data, calculate the specific heat of aluminum. 7. A total of 226 J of heat are absorbed as 58.3 g of lead is heated from 12.0 C to 42.0 C. From this data, what is the specific heat of lead? 8. What is the change in heat energy when 132 g of copper at 32.2 C is raised to 45.0 C? The specific heat of copper is J/g C. 9. What is the change in heat energy when 75.0 g of water at 9.8 C is raised to 22.4 C and the specific heat of liquid water is 4.18 J/g C? 10. What is the change in heat energy when 125 g of water at 10.0 C is raised to 90.0 C 9.E Calorimetry: Heating and Cooling Curves Instructions: Answer the question 1 2 using this heating curve for water. 1. Identify the sections where the following phases are found: a. gas b. solid c. liquid d. solid and liquid e. liquid and gas 11. What is the change in heat energy when g of aluminum metal at C is cooled to 82.0 C? The specific heat of aluminum is J /g C. 12. What is the mass of a sample of iron if that sample lost 2300J of heat energy when it cooled from 80 C to 30 C? The specific heat of iron is J /g C. 13. What is the specific heat of metal if its mass is g and it requires J of heat energy to raise its temperature from 27.4 C to 67.3 C? 14. If a 38g sample of water releases 621 J of heat energy and cools to 4.0 C. What was the initial temperature of the water? 15. If 41grams of water at 24 C absorbs 2208 J of heat energy, what will be the final temperature of the water? 16. How much heat energy is absorbed by 10 g of silver if it increases in temperature from 10 C to 310 C? The specific heat of silver is J/g C. 17. What is the change in temperature in a 128 g sample of water if it absorbs 2808J of heat energy at a temperature of 3.21 C? 2. Identify by letter (A-E) in which section the following are found: a. Freezing (if cooling) b. Particles farthest apart c. Boiling d. Particle motion is most restricted e. Heat of fusion f. All areas where energy change is potential only g. Heat of vaporization h. All areas where particles move past each other. i. Least kinetic energy j. All areas where kinetic energy is changing k most potential energy l. All areas where phase changes occur m. All areas in which the heat is making the particles move faster n. All areas in which the heat is breaking the attractions or bonds between particles o. All areas in which the particles are not changing their speed Heat Removed Instructions: Given the following BP and MP information, sketch and label heating and cooling curves for the substances under the following changes in temperature AND phase. BPAg = 2162 C MPAg = 962 C BPPb = 1749 C MPPb = 328 C BPCu = 2927 C MPCu = 1085 C BPN = -196 C MPN = C 3. Water going from 24 C to 123 C. 6. Water going from 10 C to steam at100 C 9. Water going from 130 C to -30 C. 4. Water going from -24 C to 110 C. 7. Pb going from 900 C to -90 C. 10. Ice going from 0 C to water at 10 C. 5. Silver going from 1300 C to 50 C. 8. Cu going from 150 C to 1200 C. 11. Water at 0 C going to -50 C.

5 9.F Calorimetry: The Full Picture Instructions: ON A SEPARATE SHEET OF PAPER, (1) Sketch the heating or cooling curves (BE SURE TO LABEL!!!) associated with each of the following temperature changes and: (2) Calculate the amount of heat energy lost or gained during each temperature change given the information below right. Remember, Sig Figs, NW = NC, Boxed Answers and N 3 (this includes g of H2O changing in temperature from C to 85.0 C g of H2O changing in temperature from C to C g of H2O(g) changing in temperature from C to C g of Au changing in temperature from 100. C to 1234 C g of O2 changing in temperature from C to C g of H2O changing in temperature from C to C g of H2O changing in temperature from C to H2O(s) at 0.00 C g of He changing in temperature from C to C 9.G Gases: KMT Instructions: Provide a response for each question that is well thought out, satisfies the prompt, is clearly explained, and LEGIBLE. 1. What theory explains the behavior of gases with respect to conditions such as temperature and pressure? 2. Complete the followign statements in relation to the KMT. a. Gases consist of large numbers of tiny particles that are far apart relative to their size. This means that b.collisions between gas particles and between particles and container walls are elastic collisions. This means that c. Gas particles are in constant, rapid, random motion. This can be inferred because d. There are no forces of attraction or repulsion between gas particles. This means that e.the average kinetic energy of gas particles depends on the temperature of the gas. This means that 3. gasses conforms to all postulates of the KMT. 4. In order to fully describe a gas, measurable quantities must be stated. a. Define PRESSURE: units: 1 atm ( atmosphere ) = mm Hg ( millimeters mercury ) = torr = kpa ( kilopascals ) measured with a b. Define TEMPERATURE: units: degrees Celsius ( ) or Kelvin ( ) how to convert from C to K? c. Define VOLUME: units: 1 Liter (L) = ml = cm 3 = dm 3 d. Define QUANTITY: units: Convert from grams to moles using abbreviated. 5. STP stands for. The conditions at STP are exactly atm of pressure and a temperature of exactly and any gas at STP will occupy a volume of L. Latent Heats of Fusion, Vaporization and Specific Heats Substance Specific Heat J _ g C Melting Point ( C) Heat of Fusion (J/g) Boiling Point ( C) Heat of Vaporization (J/g) Helium Nitrogen Oxygen Ethyl Alcohol Water (s) = 2.11 (l) = (g) = 2.08 Aluminum Silver Gold H Gases: Variables of Gas Laws Instructions: ON A SEPARATE SHEET OF PAPER, preform the following temperature and pressure conversions. Remember, Sig Figs, NW = NC, Boxed Answers and N 3 (this includes atm to mm Hg kpa to atm x 10 4 torr to mm Hg mm Hg to kpa 7. 93,500 Pa to atm atm to kpa mm Hg to atm torr to atm C to Kelvin C to Kelvin K to C C to Kelvin K to C C to Kelvin Kelvin to C

6 Instructions: ON A SEPARATE SHEET OF PAPER, identify the values and symbols of all variables present within the following data. Be sure to denote the unknown variable, what you need to solve for, as = x. Variables to denote in include but are not limited to include n1, V1, P1, T1, n2, V2, P2, and T2. Remember, temperature for Gas Laws must be reported in K. No Work must be shown. 16. If 2.00 mol of gas occupies 4.50L at STP. How much of the same gas will occupy 3.00L at STP? 22. The pressure of neon changes from 786 mm Hg to 1811 mm Hg. If the initial temperature 87 o C, what is the new temperature (in K)? 17. A gas has an initial volume of 15 L. If the temperature increases from 330 K to 450 K, find the new volume. 18. A gas exerts 1.2 atm of pressure. If the temperature is raised from 225 K to 325 K, find the new pressure. 19. Suppose 5.00 L of a gas is known to contain mol. If the amount of gas is increased to 1.80 mol, what new volume will result (at an unchanged temperature and pressure)? 20. A sample of oxygen takes up 34 dm 3 of space when it is under 500 kpa of pressure. When the pressure is changed to 340 kpa, find the new volume. 21. The pressure of some N2 drops from 315 kpa to 220 kpa. If the initial volume is 1.4 L, find the new volume. 23. When the temperature of a gas changes, its volume decreases from L to 7.92 L. If the final temperature is measured to be K, what was the initial temperature (in K)? 24. If 22.5 L of nitrogen at 748 mm Hg are compressed to 725 mm Hg at constant temperature. What is the new volume? 25. A gas with a volume of 4.0L at a pressure of 205kPa is allowed to expand to a volume of 12.0L. What is the pressure in the container if the temperature remains constant? 26. What pressure is required to compress liters of air at 1.00 atmosphere into a cylinder whose volume is 26.0 liters? 27. A 40.0 L tank of ammonia has a pressure of 12.7 kpa. Calculate the volume of the ammonia if its pressure is changed to 8.4 kpa while its temperature remains constant. 9.I Gases: A,B,C and D of Gas Laws Instructions: ON A SEPARATE SHEET OF PAPER, preform the following basic gas law calculations. Remember, Sig Figs, NW = NC, Boxed Answers and N 3 (this includes 1. If 2.00 mol of gas occupies 4.50L at STP. How much of the same gas will occupy 3.00L at STP? 2. A gas has an initial volume of 15 L. If the temperature increases from 330 K to 450 K, find the new volume. 3. A gas exerts 1.2 atm of pressure. If the temperature is raised from 225 K to 325 K, find the new pressure. 4. Suppose 5.00 L of a gas is known to contain mol. If the amount of gas is increased to 1.80 mol, what new volume will result (at an unchanged temperature and pressure)? 5. A canister contains 425 kpa of carbon dioxide, 750 kpa of nitrogen, and 525 kpa of oxygen. What is the total pressure of the container? 6. A sample of oxygen takes up 34 dm 3 of space when it is under 500 kpa of pressure. When the pressure is changed to 340 kpa, find the new volume. 7. The pressure of some N2 drops from 315 kpa to 220 kpa. If the initial volume is 1.4 L, find the new volume. 8. The pressure of neon changes from 786 mm Hg to 1811 mm Hg. If the initial temperature 87 o C, what is the new temperature (in K)? 12. A gas with a volume of 4.0L at a pressure of 205kPa is allowed to expand to a volume of 12.0L. What is the pressure in the container if the temperature remains constant? 13. What pressure is required to compress liters of air at 1.00 atmosphere into a cylinder whose volume is 26.0 liters? 14. A 40.0 L tank of ammonia has a pressure of 12.7 kpa. Calculate the volume of the ammonia if its pressure is changed to 8.4 kpa while its temperature remains constant. 15. A container containing 5.00 L of a gas is collected at K and then allowed to expand to 20.0 L. What must the new temperature be in order to maintain the same pressure? 16. A gas occupies ml at a temperature of 27.0 C. What is the volume at K? 17. If 15.0 liters of neon at 25.0 C is allowed to expand to 45.0 liters, what must the new temperature be to maintain constant pressure? 18. The pressure of a gas changes from kpa to 50.0 kpa. The volume changes from 45 L to 40 L. If the initial temperature is K, what is the final temperature in K? 9. When the temperature of a gas changes, its volume decreases from L to 7.92 L. If the final temperature is measured to be K, what was the initial temperature (in K)? 10. If 22.5 L of nitrogen at 748 mm Hg are compressed to 725 mm Hg at constant temperature. What is the new volume? 11. A tank containing ammonia and argon has a total pressure equal to 1.8 atm. The pressure of the ammonia is 1.2 atm. What is the pressure of the argon gas? 19. A sample of nitrogen goes from 21L to 14 L and its pressure increases from 100. kpa to 150. kpa. The final temperature is 300. K. What was the initial temperature in Kelvins? 20. A sample of argon goes from 500 K to 350 K and its pressure changes from 280 kpa to 380 kpa. If the initial volume is 18 dm 3, what is the final volume? 21. A sample of neon experiences a pressure drop from 75 kpa to 53 kpa. The temperature increases from K to K. If the initial volume is 12 L, what is the final volume?

7 9.J Gases: Ideal Gas Law 1.What are the differnces between an ideal gas and a real gas? 2. REAL GASES BEHAVE NEARLY IDEALLY UNDER CONDITIONS of temperature, pressure, & molar mass. Instructions: Complete the following statements to remind yourself of the requirments of the Ideal Gas law before completing the calualtions that follow. In P V = n R T: "P" stands for, must be in units of "V" stands for, must be in units of "n" stands for, must be in units of "T" stands for, must be in units of "R" stands for the Ideal Gas Constant, has a value that dependent on. Instructions: ON A SEPARATE SHEET OF PAPER, preform the following basic gas law calculations. Remember, Sig Figs, NW = NC, Boxed Answers and N 3 (this includes 3. If 3.7 moles of propane are at a temperature of 28 C and are under kpa of pressure, what volume does the sample occupy? 4. A sample of carbon monoxide at 57 C and under 0.67 atm of pressure takes up 85.3 L of space. What mass of carbon monoxide is present in the sample? 5. At 45 C, 71 g of fluorine gas take up 6843 ml of space. What is the pressure of the gas, in kpa? 6. At 971 mm Hg, 145 g of carbon dioxide have a volume of L. What is the temperature of the sample, in C? 7. At 137 o C and under a pressure of 3.11 atm, a 67.3 g sample of an unknown noble gas occupies L of space. What is the gas? 8. Given 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature? 9. An unknown quantity of gas at a pressure of 1.2 atm, a volume of 31 liters, and a temperature of 87 0 C, how many moles of gas are present? 10. A vessel contains 3.21 moles of gas with a volume of 60.9 liters and at a temperature of K, what is the pressure inside the container? 11. A vessel contains 7.7 moles of gas at a pressure of 0.09 atm and at a temperature of 56 0 C, what is the volume of the container that the gas is inml? 12. A vessel contains 1.37 moles of gas at a temperature of C, and a volume of liters, what is the pressure of the gas in atm? 9.J Gases: Ideal Gas Law 1.What are the differnces between an ideal gas and a real gas? 2. REAL GASES BEHAVE NEARLY IDEALLY UNDER CONDITIONS of temperature, pressure, & molar mass. Instructions: Complete the following statements to remind yourself of the requirments of the Ideal Gas law before completing the calualtions that follow. In P V = n R T: "P" stands for, must be in units of "V" stands for, must be in units of "n" stands for, must be in units of "T" stands for, must be in units of "R" stands for the Ideal Gas Constant, has a value that dependent on. Instructions: ON A SEPARATE SHEET OF PAPER, preform the following basic gas law calculations. Remember, Sig Figs, NW = NC, Boxed Answers and N 3 (this includes 3. If 3.7 moles of propane are at a temperature of 28 C and are under kpa of pressure, what volume does the sample occupy? 4. A sample of carbon monoxide at 57 C and under 0.67 atm of pressure takes up 85.3 L of space. What mass of carbon monoxide is present in the sample? 5. At 45 C, 71 g of fluorine gas take up 6843 ml of space. What is the pressure of the gas, in kpa? 6. At 971 mm Hg, 145 g of carbon dioxide have a volume of L. What is the temperature of the sample, in C? 7. At 137 o C and under a pressure of 3.11 atm, a 67.3 g sample of an unknown noble gas occupies L of space. What is the gas? 8. Given 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature? 9. An unknown quantity of gas at a pressure of 1.2 atm, a volume of 31 liters, and a temperature of 87 0 C, how many moles of gas are present? 10. A vessel contains 3.21 moles of gas with a volume of 60.9 liters and at a temperature of K, what is the pressure inside the container? 11. A vessel contains 7.7 moles of gas at a pressure of 0.09 atm and at a temperature of 56 0 C, what is the volume of the container that the gas is inml? 12. A vessel contains 1.37 moles of gas at a temperature of C, and a volume of liters, what is the pressure of the gas in atm?