Kinetic-Molecular theory of Matter/Ch10, Gases/Ch11 Column notes: Answer all parts of each question IN YOUR OWN WORDS. Use the text, figures and captions as resources. Section 10-1: The Kinetic-Molecular Theory of Matter 1) How does the word kinetic apply to particles of matter? 2) Briefly describe the postulates of the Kinetic Molecular Theory (KMT). 3) What is the relationship between temperature and average kinetic energy? 4) What is the mathematical relationship between average kinetic energy and velocity of particles? Therefore, what is the relationship between temperature and velocity? 5) Using the KE equation, explain why balloons filled with helium (molar mass 4g/mol) deflate faster than those filled with air (molar mass 29g/mol) 6) What is an ideal gas? Do any actually exist? Why do we care about them? 7) Describe the properties of gases and how each can be explained by the KMT? 8) Which postulates of KMT do real gases not follow? What types of gases are most like ideal gases? What types of gases are most like real gases? 11-1 Gases and Pressure 9) What causes pressure? How is it defined (include units)? Why does the pressure on your feet change if you are on tip toes? 10) What gas characteristics does pressure depend on? 11) What causes atmospheric pressure? What is the value for this pressure at sea
level (including units)? Write the equivalent pressures in atmospheres, pascals, millimeters of mercury, torr, kilopascals, and pounds per square inch. 12) What is standard temperature and pressure? Why do scientists want these variables standardized for gas measurements? 13) Describe how a barometer measures atmospheric pressure. 14) Describe how a manometer measures the pressure inside a closed container. 15) The pressure of oxygen on Mount Everest is 47.88 mmhg on a given day(your lungs need about 100 mmhg oxygen for you to survive). Using conversion factors, calculate this mountain pressure in units of atmospheres, pascals, torr, kilopascals, and pounds per square inch. (see sample problem A) 16) What is Daltons law of Partial Pressure? How is it related to the KMT? 17) Calculate the partial pressure, in mmhg, exerted by the 4 main gases in air at 760mmHg if the abundance of nitrogen is 78.08%, oxygen 20.95%, argon 0.934%, carbon dioxide 0.035%. Show work. 18) Based on Figure 5 on p366, when gases are generated in a chemical reaction, why is it convenient to collect them by water displacement? Why do you have to correct the total atmospheric pressure in order to determine the accurate pressure of the gas from the reaction?
19) After reading the Chemistry in Action article, answer the following questions: a) Explain how increased water pressure can cause nitrogen narcosis in scuba divers (an intoxicating feeling) b) Explain how Henry s Law can cause decompression sickness ( the bends ) if a diver comes up too quickly. 11-2 The Gas Laws 20) What are the 4 variables of gases? 21) What two variables are related in Boyle s Law? What is the equation used for this relationship? Are the 2 variables directly or inversely related and explain how you know this? What 2 variables must be kept constant? 22) How is Boyles Law related to the KMT? 23) Do the practice problem on p370. Show work. 24) What two variables are related in Charles Law? What is the equation used for this relationship? Are the 2 variables directly or inversely related and explain how you know this? What 2 variables must be kept constant? 25) What units of temperature must be used for this calculation? How do you convert from one unit to the other?
26) How is Charles Law related to the KMT? 27) Do practice problem 1 on p372. Show work. 28) What two variables are related in Gay- Lussac s Law? What is the equation used for this relationship? Are the 2 variables directly or inversely related? What 2 variables must be kept constant? 29) What does Combined mean in the Combined Gas Law. Demonstrate how each of the 3 previous gas laws can be obtained from the Combined Gas Law. 30) If 5 out of 6 of the Combined Gas Law variables are known, the 6 th can be solved for. Do Practice Problem 1 on p375. 11-3 Gas Volumes and the Ideal Gas Law 31) What does Avogadro s Law tell us about the number of gas molecules and the volume they occupy? What 2 variables must be kept constant? 32) How can coefficients of a balanced equation involving gases be used to determine the ratio of the volumes. 33) How many molecules are contained in 22.4 liters of a gas at STP? What is this volume called? 34) How does mass of a molecule affect its volume? 35) Do Practice Problems 1 and 2 on p381. 36) How can Avogadro s relationship between volume and moles be used to do stoichiometry calculations. 37) Do Practice Problem 2 on p382.
38) How does the ideal gas law relate the 4 gas variables? Do any of them need to be kept constant for this relationship to work? 39) What does R represent in the Ideal Gas Law? How were the number and its units derived from the other 4 quantities? 40) Why are there 4 different numbers for the gas constant R? How do you decide which one to use for a particular problem? Which units will you usually use for volume, pressure, temperature and amount? 41) Do Section Review problem 5 on p385. Make sure to check units and convert those which will not fit with R units. 11-4 Diffusion and Effusion 42) Compare and contrast Diffusion and Effusion. 43) How is Kinetic Energy related to the mass of a molecule? To the velocity of a molecule? 44) What postulate in the KMT is used to derive Grahams Law of Effusion. What is the equation for this Law? 45) Calculate the molar mass of a gas that effuses at 1.6 times faster than carbon dioxide. (hint: set the ratio as 1.6 1 and identify which of these will be the larger molecule and which will be the smaller one). Use sample problem to guide you.