Do Now: Find new seats zacharia 9 ian 10 joy 11 Shajra 12 de'andre 13
melanie 1 andretta 2 jennifer 3 elias 4 mariah 5 casandra 6 shaquom 7 augustin 8 zacharia 9 ian 10 joy 11 Shajra 12 de'andre 13 hector 14 julianna 15 isabella 16 jacob 17 arianna 18 gabrielle 19 Jose 20 Nailah 21 syndey 22 emily 23 Se'jean 24 angelica 25 daniel 26 jairo 27 christina 28 kayla 29 Do Now: Find New Seats egar 1 alexandra 2 damien 3 kiara 4 lorena 5
denzell 6 olivia 7 emma 8 jordan 9 elijah 10 yasheema 11 joshua 12 mina 13 christopher 14 kevin 15 bruno 16 joseph 17 seth 18 johanan 19 lindsey 20 itzel 21 Jessica 22 jonathan 23 vernon 24 parker 25 megan 26 sara 27 nazjai 28 WELCOME BACK! WELCOME BACK! Bellringer:
Read the first page of the notes packet and fill in the particle diagrams based on the reading Remember about gravity Homework: Make sure you finish and turn in types of reactions lab by tomorrow This unit All about phases, their properties and phase changes
Are there different types of solids? What happens when things go from slg? How much energy is needed in order to go through those changes Todays objective Describe the properties of solids
Design a lab to determine the type of solid for an unknown Solids High, Medium, or Low attraction between each particle?
How do they move? Liquids High Medium or Low attraction How do they move?
Proof that liquid molecules are attracted to each other: Gas High Medium or Low attraction? How do they move? Solids! We are going to focus on Different types of solids.
Focus: You are going to design a lab to determine what type of solid two different solids are Read along with your neighbor and fill in the venn diagram on the next page Maybe split it: 2 types per neighbor? Things all Solids have in common goes in the center Overlap is for things in common Do Now Pick up a copy of the lab
RETURN ANY EXTRA COPIES OF THE NOTES THAT YOU MAY HAVE TAKEN Make sure the following are described in the venn diagram: Melting point (very high, high, variable, low) Solubility Conductivity (if so, under what conditions) How the particles are arranged Types of solids lab 2 different solids You have:
Distilled water (may have CO2 Dissolved in it) This would make it slightly conductiveneed to account for that Conductivity testers cups stirring rods other miscellaneous lab equip (NOT BUNSEN BURNERS) Procedure Get it approved before beginning
It would be unfortunate to get all the way done and then find an error with the procedure and need to do it all over Something to think about: When CO2 dissolves into water, it makes the water conductivegoing to need to account for that Do now Take out your Types of Solids Lab Refresh your memory
IonicMolecular NetworkMetallic Sol. Cond. M.p. Make sure you get your procedure approved and finish the lab (and turn it in) Absent? Then you need to play a little catch up
Read the notes about the types of solids and fill in the 4 box ven diagram on the next page Use this information to figure out how you could test these 2 unknown solids to determine what type of solid they are Homework: Finish the lab Do now Bellringer Quiz: Pick up, do independently and turn in
Also turn in Types of Solids lab Homework Phases and phase change diagrams Heat of phase changes
(front and back of 1st page) And now Read page 4 and fill in the graphic organizer on page 5 and 6 A nice simulator Phase Changes: Label the phase changes (1-6), identify each side as either exothermic or endothermic, fill in the phase change diagrams and particle diagrams for each phase. Gas (particle diagram) Liquid Solid _____thermic + or -H 1.___________ 2.___________ 3.___________ 4.___________ 5.___________ 6.___________ Time Temp. (K) Sublimation and Deposition
1) Label the phases present at each line segment above using (s), (l), and (g).
2) What is the boiling point of this substance? ________ 3) What is the melting point of this substance? ________ c.Heat of phase change In previous units we have calculated the amount of energy needed to change the temperature of water using the formula: q=mCT (remember that catchy song?). During a phase change, however, there is no change in temperature so this formula cannot be used to solve for the heat needed for a phase change. Instead, there are different formulas used for phase changes; q=mHf and q=mHv. Hf is the heat of fusion, the amount of energy required to melt or freeze a gram of water (334 J/g). Hv is the heat of vaporization of water; the amount of energy required to boil or condense water (2260 J/g).. m is the mass of water involved in the phase change. How much energy is required to melt 50.0g of water at 0oC?
q = m Hf Why Hf? q = 50.0 g x 334J/g q=16700 J Practice Problems _____1) Which of the following phase changes requires heat of fusion to accomplish? a) H2O (s) H2O (g) b) H2O (g) H2O (l) c) H2O (l) H2O (g)d) H2O (s) H2O (l) _____2) Which of the following phase changes is endothermic? a) H2O (s) H2O (l) b) H2O (g) H2O (l) c) H2O (l) H2O (s) d) H2O (g) H2O (s) Calculate the number of joules required to (show correct numerical setup):
a)melt 20.0 g of H2O (s) at 0oC b)boil 30.0 g of H2O (l) at 100oC c)freeze g of H2O (l) at 0oC d)boil 50.0 g of H2O (g) at 100oC Ice cubes at 12.0oCare placed in a saucepan and heated at a constant rate over a stove to 115.0oC.
Sketch a phase change diagram for the phase changes that occur between oC and 115.0oC.Label the temperatures at which the phase changes occur.Then label each line segment with a letter (A, B, C, D, E, etc.). Label where P.E. increases/stays same Do the same for K.E. Do Now: Pick up a copy of the lab Read over the procedure to the lab Questions? _____1) Which of the following phase changes requires heat of fusion to accomplish? a) H2O (s) H2O (g) b) H2O (g) H2O (l)c) H2O (l) H2O (g) d) H2O (s) H2O (l) _____2) Which of the following phase changes is endothermic? a) H2O (s) H2O (l) b) H2O (g) H2O (l)c) H2O (l) H2O (s) d) H2O (g) H2O (s) Calculate the number of joules required to (show correct numerical setup): a)melt 20.0 g of H2O (s) at 0oC b)boil 30.0 g of H2O (l) at 100oC c)freeze g of H2O (l) at 0oC d)boil 50.0 g of H2O (g) at 100oC Ice cubes at 12.0oCare placed in a saucepan and heated at a constant rate over a stove to 115.0oC.
Sketch a phase change diagram for the phase changes that occur between oC and 115.0oC.Label the temperatures at which the phase changes occur.Then label each line segment with a letter (A, B, C, D, E, etc.). Safety Goggles Be careful of HOT WATER Dont drop the thermometers
Do not poke a whole in the bottom of the calorimeters! Dont eat the ice Big Idea Starting with hot water and Ice
Going to calculate how much energy was lost by the water (q=mCT) That energy was used to melt the ice Calculate the Hf based on that q/(g of ice melted) Follow the procedure! Do Now Take out The Heat of Fusion Lab from yesterday and begin working on it Plan on the Test being on Thursday Quiz on THIS FRIDAY (covering phase changes) This periods agenda Finish the lab
Finish the H.W., front and back of the first page Start reading the 4. Gases and Pressure Do now Turn in Heat of Fusion Lab
Turn in first page (front and back) from homework packet Read over topic 4: Gases and Pressure (a+b) Start brainstorming on how you could visualize each of these concepts Kinetic molecular theory (KMT) for gases and ideal gas laws
Before we can discuss what an Ideal gas is, we must first discuss what is true for all gases, ideal and real. The following is true for all gases: Gas particles have no definite volume Gas particles have no definite shape Gases are highly compressible Gases take the volume and shape of the container Gas molecules are relatively far apart from one another Gases form homogeneous mixtures with each other Real gases will act like Ideal gases at low pressure and high temperature. Smaller gases (H2 and He) also behave more ideally than larger gases (CO2, CH4). The concept of the Ideal gas is to explain the behavior of real gases. There is a list of things that we assume about gases to be true to explain their behavior. For example, we assume that ideal gas particles have no attraction for each other, which is why the take on the volume of their container. Real gas particles do have some attraction to each other. The reason we make these assumptions is because they are mostly true, and in doing so we can calculate a lot of information about gases. The following are the Ideal Gas Laws: Gas molecules are so small that the combined size is insignificant compared to the volume occupied by the gas. Gas molecules move in straight line motion until they collide with the container wall or another gas molecule Any collisions between gas molecules are elastic with NO energy lost from the collisions. No attractive or repulsive forces exist between gas molecules. The Average velocity (speed with direction) of the gas is directly proportional to the KELVIN temperature (the higher the temperature, the faster they move). b. Avagadros hypothesis
Simply put, Avogadros Hypothesis states that equal volumes of ALL gases, at the same temperature and pressure, have the same number of molecules. If you were to double the number of molecules, you would double the volume. Poster Project (14 minutes)
Illustrations are excellent for visualizing some abstract concepts. You will use your creativity to create a visual for one of these concepts It can be a literal representation, an example from real life or a metaphor. Example: The atom is mostly empty space Draw an atom with mostly empty space A club named Atom, which is almost completely empty Poster Project (14 minutes)
Be prepared to explain your illustrations to the class Poster presentations Quickly Sketch your favorites into your notes packet Do Now (Test Thursday) Take out Homework Packet and put everything else away Homework check time! Finished? Read: Pressure, vapor pressure and boiling points through Using the reference tables Try some of the practice c. Pressure, vapor pressure and boiling point
Pressure is defined as a force exerted on an area. You may be familiar with the term psi, which stands for pounds per square inch. This is what you see on your gas gauge when you check the pressure in your tires of your car or bicycle and measures how much force is being exerted on every square inch of your tires surface. The force itself is a result of the gas particles colliding with the surface of the container. There are other units to measure pressure and in chemistry we will either use atmospheres (1 atmosphere of pressure is the amount of force exerted by the atmosphere above use, about 14.7 psi), or kilopascal named after a French mathematician and physicist (1 atmosphere = kPa). Pressure Pressure simulator Web File Particles in the liquid phase, in a closed container, may evaporate (go into the gas phase while below the boiling point) and exert a pressure. We call this vapor pressure, as it is the pressure caused by the vapor and it does not depend on how much liquid is in the container. Vapor Pressure i.Normal boiling point Particles in the liquid phase, in a closed container, may evaporate (go into the gas phase while below the boiling point) and exert a pressure. We call this vapor pressure, as it is the pressure caused by the vapor and it does not depend on how much liquid is in the container. A substance will boil when it is heated to the point that its vapor pressure is equal to that of its environment. The normal boiling point is the temperature at which the vapor pressure is equal to standard pressure. Standard pressure has been defined as 1 atmosphere (101.3 kPa) and can be found in your reference tables under the Table A titled Standard Temperature and Pressure. i.Normal boiling point If you change the pressure of the system a liquid is in, you also change its boiling point. This is how you can get LP (liquid propane) gas tanks for your grill. Propane, at standard temperature, will be in its gas phase. In order to store it in its more condensed liquid phase, the pressure needs to be increased. This is why they are stored in pressurized tanks. When you open the tank, you let some of the propane out, which is then exposed to a much lower pressure in the grill, becomes a gas which is then ignited to cook some hot dogs, hamburgers, chicken, maybe some cornwhatever your little heart desires! Its really up to you. Dont believe me? Let me show you! Normal Boiling Point Pressure cookers also make use of the impact of pressure on boiling points. A pressure cooker doesnt allow for gas to escape as youre cooking your meal. This causes the pressure inside to build up, which increases the temperature at which the water will boil. This higher temperature allows the food to cook faster! Pressure Cooker Using the reference tables
Reference Table H is titles Vapor Pressure of Four Liquids and can be used to determine the boiling points of these liquids at different temperatures. Remember, the boiling point is the temperature at which the vapor pressure equals the pressure of the system. Using R.T. H What are the normal boiling points for:
Propanone:____________ Ethanol:_____________ H2O:________________ Ethanoic Acid:_____________ What would the boiling point of water be at a pressure of 200 kPa?__________ What would the vapor pressure be for propanone at 50 degrees celcius?____________ Which of these 4 liquids has the strongest attractive force?_________________________ Do Now (Test Thursday) Turn in Heat of Fusion Lab
Pick up a copy of the lab Read over the procedures (Next homework due tomorrow) Safety Bunsen burner safety Beaker tongs to handle hot things
Not using it, turn it off! Beaker tongs to handle hot things Be careful when flipping your hot can, dont let the water escape Be careful in general Balloon + water: need about an inch of water Finished the lab? Finish the HWs Do Now Take out the lab from yesterday and your homework packet Reviewing the lab As Temperature increased, volume___________
As Temperature decreased, pressure__________ As the pressure increased, volume___________ Neat demo And now Gases and pressure Practice in the HW packet
H.W. for tonight: Read the rest of the notes packet and attempt the practice Short summary next class and then jumping right into practice Do Now: Take out homework #3 (gases and pressure)
Read topic 5: Gas laws: Pressure, temperature and volume Try the practice problems on the next page Homework Review C A B D 202.6 19.25 ~102 ~25 ~80 ~70 ~45 ~123 ~57 Gas laws: Pressure, temperature and volume
The Gas Laws are relationships between temperature, pressure and volume of a gas.Gas law equations are used to determine what effect changing one of those variables will have on any of the others. There are three gas laws that combine to give us our combined gas law, and they are: Boyles Law: Boyles Law: P1V1=P2V2: As pressure on a gas increases, the volume of the gas decreases. The product of the initial pressure (P1) and volume (V1) will be equal to the product of the final pressure and volume (P2V2) Which experiment? Charles Law Charles Law: V1/T1 = V2/T2: As temperature of the gas increases, the volume of the gas must also increase. The quotient of the initial volume and temperature (V1/T1) is equal to the quotient of the final volume and temperature (V2/T2). TEMPERATURE NEEDS TO BE IN KELVIN Which experiment? Gay-Lussacs Law Gay-Lussacs Law: P1/T1 = P2/T2: As the temperature of a gas increases, so does its pressure. The quotient of the initial pressure and temperature (in kelvin) (P1/T1) is equal to the quotient of the final pressure and temperature (P2/T2). Which experiment? PT Cruiser Cards A neat way to remember how these three factors are related is by what has been trademarked as a PT Cruiser card. Simply take an index card and write across it the lettersP T V. To see how one factor will be affected by changing one of the other two, simply grasp the card with your finger covering the letter for the factor being kept constant, push the variable that is being changed in the direction in which it is changing (up for increasing, down for decreasing) and see how the other variable responds. For example: increasing pressure while temperature is kept the same. You would cover grab the card at the temperature letter, push the P up, and see how the volume would decrease! Pt Cruiser Card PTV Combined Gas Law The three individual gas laws combine to give us the combined gas law, which allows us to examine how all three variables respond to a change in a system without needing to have one of the variables kept constant (seen on the right). You can also get the other three gas laws from this combined formula. If one of the variables is kept constant, it simply drops out of the equation. For example: If temperature was kept the same, T would drop out and you would be left with: P1V1=P2V2. Solving for when something is held constant
A sealed can with an initial pressure of #p1 is heated from #t1 kelvin to #t2 kelvin. What is the new pressure? Solving for when something is held constant
A balloon with an initial pressure of #p1 is heated from #t1 kelvin to #t2 kelvin at a constant pressure. What is the new volume? Practice: (remember temperature needs to be in kelvin).
What volume will 500.mL of a gas occupy if the pressure is changed from 1.00 atmosphere to 2.00 atmosphere at constant temperature? P1 = P2= V1= V2= T1 = T2= A tube of hydrogen gas at a room temperature of 22
A tube of hydrogen gas at a room temperature of 22.4C has a pressure of 88.0 KPa.What was the new temperature of the hydrogen gas when the pressure in the tube is at KPa? (Volume is constant!) P1 = P2= V1= V2= T1 = T2= A gas has a volume of 700. mL at a temperature of 10
A gas has a volume of 700.mL at a temperature of 10.0C at constant pressure.What volume will the gas occupy if the temperature is raised to 50.0C? (Remember: change C to K!!) P1 = P2= V1= V2= T1 = T2= 4. ) A sample of gas occupies a volume of 500. mL at a pressure of 0
4 .) A sample of gas occupies a volume of 500. mL at a pressure of atm and a temperature of 298K.At what temperature will the gas occupy a volume of 250. mL and have a pressure of 2.50 atm? P1 = P2= V1= V2= T1 = T2= Homework: Finish the homework packet
Start studying for the test/quarterly (heavy on the periodic table) Do Now Read the final topic: Gas laws; pV=nRT Honors: Gas laws; pv=nRT
The pressure and volume of a gas are proportional to the number of moles of gas and the Kelvin temperature.The equation can be derived as follows: From the Combined Gas Law, we have PV/T = K, K = nR(n is number of moles, R is a proportionality constant) (increase the number of moles, it affects everything else) R Since one mole of gas exerts a pressure of 1.00 atm and occupies a volume of 22.4 L at 273 K, R (the proportionality constant) can be derived as follows: (1 atm)(22.4 L)/(1 mole)(273 K) = R R = atm-L/mol-K Ideal Gas Law This yields the IDEAL GAS LAW, which can be used to determine the pressure, volume, temperature or number of moles of gas if all of the other conditions are known, and none of the conditions have changed. PV = nRT P= Pressure (atm)V = Volume (L) n = moles R = atm-L/mol-K T = Temp (K) Practice with ideal gas law
What is the pressure exerted by 3.00 moles of gas at a temperature of 300. K in a 4.00 L container? PV = nRT What is the volume of a sample of gas if 5
What is the volume of a sample of gas if 5.00 moles if it exerts a pressure of atm at 200. K? PV = nRT A sample of gas contained in a cylinder of 5
A sample of gas contained in a cylinder of 5.00 L exerts a pressure of 3.00 atm at 300. K.How many moles of gas are trapped in the cylinder? PV = nRT A hydrogen gas thermometer is found to have a volume of 100
A hydrogen gas thermometer is found to have a volume of cm3 when placed in an ice-water bath at 0C. When the same thermometer is immersed in boiling liquid chlorine, the volume of hydrogen at the same pressure is found to be 87.2 cm3. What is the temperature of the boiling point of chlorine? When filling a weather balloon with gas you have to consider that the gas will expand greatly as it rises and the pressure decreases. Lets say you put about 10.0 moles of He gas into a balloon that can inflate to hold L. Currently, the balloon is not full because of the high pressure on the ground. What is the pressure when the balloon rises to a point where the temperature is -10.0C and the balloon has completely filled with the gas. Do Now Turn in any owed work (last day to turn in is Friday of next week) Take out a sheet of paper and something to write with Topics on the test Properties of phases (solid vs liquid vs gas)
Phase diagrams and describing how they behave Types of solids and their properties Conductivity, melting points, solubility, how they are held together Phase changes and heat of phase changes Properties of gases (ideal vs real) Gas law problems Really, re-do the homework, read and re-do the practice in the notes packetas always, no real surprises Combined Gas Law Partner Practice
As we have done in the past; 1st person writes the givens and rearranges the formula to solve for what is missing 2nd person plugs and chugs, then rounds final answer correctly to sig figs and gives units Switch for the next problem 1 sheet of paper per partnership Answers are on the back to ensure you are doing it correctly Cant see what yourre doing wrong? Ask a neighbor, then ask me! A bag of potato chips is packaged at sea level (1
A bag of potato chips is packaged at sea level (1.00 atm) and has a volume of 315 mL.If this bag of chips is transported to Denver (0.775 atm), what will the new volume of the bag be? 2)A Los Angeles class nuclear submarine has an internal volume of eleven million liters at a pressure of atm.If a crewman were to open one of the hatches to the outside ocean while it was underwater (pressure = atm), what be would the new volume of the air inside the submarine? 3). A child has a toy balloon with a volume of 1. 80 liters
3)A child has a toy balloon with a volume of 1.80 liters.The temperature of the balloon when it was filled was 200 C and the pressure was 1.00 atm.If the child were to let go of the balloon and it rose 3 kilometers into the sky where the pressure is atm and the temperature is -100 C, what would the new volume of the balloon be? 4). A commercial airliner has an internal pressure of 1
4)A commercial airliner has an internal pressure of 1.00 atm and temperature of 250 C at takeoff.If the temperature of the airliner drops to 170 C during the flight, what is the new cabin pressure? 5)If divers rise too quickly from a deep dive, they get a condition called the bends which is caused by the expansion of very small nitrogen bubbles in the blood due to decreased pressure.If the initial volume of the bubbles in a divers blood is 15 mL and the initial pressure is atm, what is the volume of the bubbles when the diver has surfaced to 1.00 atm pressure? GET READY FOR JEOPARDY! TEST DAY! Turn in Homework packet Pick up: Quarterly Review
New unit packet HOMEWORK Read/highlight pages 1-4 Monday: Start the first day of the new unit, then review for the quarterly Take out the review from yesterday
Any questions on it? Anything you would like me to go over?