Science Classroom Teacher Resources
Kinetic Theory
- This “Collision Theory Worksheet” ( doc ) includes answers.
- A “Phase Change Worksheet” ( pdf ) with answers.
- Review vocabulary with this “Thermodynamics Worksheet” ( pdf ) .
- Have students do the “Kinetic Theory” ( doc ) with answers ( doc ) .
- Demonstrate the “electron sea model of metals” concept with this “ Modeling Metals with Marbles ” activity.
- Demonstrate kinetic theory with Flinn Scientific’s “Sudsy Kinetics” ( pdf ) demonstration.
- Do this “Observing Latent Heat With a Portable Hand Warmer” ( pdf ) demonstration.
- This follow-up lab to the NOVA program “Descent Into Ice” ( pdf ) investigates the phase change of water changing into ice.
- The purposed of the “ Temperature Changes Everything ” lab is to determine the effect of temperature on particles. It includes a student worksheet ( pdf ).
- This lab uses toilet bowl freshener and moth balls to demonstrate “ Sublimation .”
- The “ Kinetic Molecular Theory of Popcorn ” is an edible lab.
- Try this “Boiling Point” ( doc ) lab.
- Do the “How Much Energy Is in a Nut?” lab ( doc ) .
- Or try the “Heat and the Calorie” lab ( doc ).
- Do this “Melting and Freezing” lab ( doc ).
- Try “The Sublimation of Air Freshener” lab ( doc ) .
- Or try the “Water Expands When It Freezes” lab ( doc ) .
- Abigail Freiberger provided this “Kinetics of Chemical Reaction” ( doc ) lab that is designed for an AP Chemistry class.
- Try this “Kinetic Theory Inquiry” ( doc ) lab.
- Do Shelly Rudnick-Peterson’s “Absolute Zero” ( doc ) lab.
- Describes states of matter and shows microscopic views: http://www.chem.purdue.edu/gchelp/atoms/states.html
- A temperature conversion calculator: http://www.onlineconversion.com/temperature.htm
- A Java applet for estimation of heat of vaporization: http://www.pirika.com/chem/TCPEE/Hv/ourHv.htm
- Applets to demonstrate phase changes and vapor pressure: http://www.chm.davidson.edu/vce/PhaseChanges/VaporPressure.html
- Graphic shows phase changes in water, copper, and nitrogen with changes in temperature: http://www.miamisci.org/af/sln/phases/watersolid.html
- All about plasmas: http://fusedweb.pppl.gov/CPEP/Chart_Pages/5.Plasma4StateMatter.html
- Tutorial on vapor pressure and evaporation: http://hyperphysics.phy-astr.gsu.edu/hbase/kinetic/vappre.html
- A vapor pressure estimation applet: http://www.pirika.com/chem/TCPEE/VP/ourVP.htm
- A “Virtual Laboratory” that includes an experiment on phase changes in liquid crystals: http://plc.cwru.edu/tutorial/enhanced/lab/lab.htm
- A virtual lab with several experiments on “Thermodynamic Equilibrium”: http://jersey.uoregon.edu/vlab/Thermodynamics/index.html
- A vapor pressure simulation: http://www.chem.iastate.edu/group/Greenbowe/sections/projectfolder. . .
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Unit 8: Gases and kinetic molecular theory
About this unit, ideal gas equation.
- The ideal gas law (PV = nRT) (Opens a modal)
- Worked example: Using the ideal gas law to calculate number of moles (Opens a modal)
- Worked example: Using the ideal gas law to calculate a change in volume (Opens a modal)
- Gas mixtures and partial pressures (Opens a modal)
- Dalton's law of partial pressure (Opens a modal)
- Worked example: Calculating partial pressures (Opens a modal)
- Worked example: Vapor pressure and the ideal gas law (Opens a modal)
- Ideal gas law 4 questions Practice
- Calculations using the ideal gas equation 4 questions Practice
Kinetic molecular theory
- The kinetic molecular theory of gases (Opens a modal)
- Kinetic molecular theory and the gas laws (Opens a modal)
- The Maxwell–Boltzmann distribution (Opens a modal)
- Kinetic molecular theory 4 questions Practice
Non-ideal gas behavior
- Introduction to real gases (Opens a modal)
- Real gases: Deviations from ideal behavior (Opens a modal)
- The van der Waals equation (Opens a modal)
- Non-ideal behavior of gases (Opens a modal)
- Deviation from ideal gas law 4 questions Practice
- Chapter 9: Gases
Kinetic Molecular Theory Practice Questions
Chemistry end of chapter exercises.
Using the postulates of the kinetic molecular theory, explain why a gas uniformly fills a container of any shape.
Can the speed of a given molecule in a gas double at constant temperature? Explain your answer.
Yes. At any given instant, there are a range of values of molecular speeds in a sample of gas. Any single molecule can speed up or slow down as it collides with other molecules. The average velocity of all the molecules is constant at constant temperature.
Describe what happens to the average kinetic energy of ideal gas molecules when the conditions are changed as follows:
(a) The pressure of the gas is increased by reducing the volume at constant temperature.
(b) The pressure of the gas is increased by increasing the temperature at constant volume.
(c) The average velocity of the molecules is increased by a factor of 2.
The distribution of molecular velocities in a sample of helium is shown in [link] . If the sample is cooled, will the distribution of velocities look more like that of H 2 or of H 2 O? Explain your answer.
H 2 O. Cooling slows the velocities of the He atoms, causing them to behave as though they were heavier.
What is the ratio of the average kinetic energy of a SO 2 molecule to that of an O 2 molecule in a mixture of two gases? What is the ratio of the root mean square speeds, u rms , of the two gases?
A 1-L sample of CO initially at STP is heated to 546 K, and its volume is increased to 2 L.
(a) What effect do these changes have on the number of collisions of the molecules of the gas per unit area of the container wall?
(b) What is the effect on the average kinetic energy of the molecules?
(c) What is the effect on the root mean square speed of the molecules?
(a) The number of collisions per unit area of the container wall is constant. (b) The average kinetic energy doubles. (c) The root mean square speed increases to $\sqrt{2}$ times its initial value; $u_{rms}$ is proportional to $\sqrt{KE_{avg}}$
The root mean square speed of H 2 molecules at 25 °C is about 1.6 km/s. What is the root mean square speed of a N 2 molecule at 25 °C?
Answer the following questions:
(a) Is the pressure of the gas in the hot-air balloon shown at the opening of this chapter greater than, less than, or equal to that of the atmosphere outside the balloon?
(b) Is the density of the gas in the hot-air balloon shown at the opening of this chapter greater than, less than, or equal to that of the atmosphere outside the balloon?
(c) At a pressure of 1 atm and a temperature of 20 °C, dry air has a density of 1.2256 g/L. What is the (average) molar mass of dry air?
(d) The average temperature of the gas in a hot-air balloon is $1.30×10^2$ °F. Calculate its density, assuming the molar mass equals that of dry air.
(e) The lifting capacity of a hot-air balloon is equal to the difference in the mass of the cool air displaced by the balloon and the mass of the gas in the balloon. What is the difference in the mass of 1.00 L of the cool air in part (c) and the hot air in part (d)?
(f) An average balloon has a diameter of 60 feet and a volume of $1.1×10^5\;ft^3$. What is the lifting power of such a balloon? If the weight of the balloon and its rigging is 500 pounds, what is its capacity for carrying passengers and cargo?
(g) A balloon carries 40.0 gallons of liquid propane (density 0.5005 g/L). What volume of CO 2 and H 2 O gas is produced by the combustion of this propane?
(h) A balloon flight can last about 90 minutes. If all of the fuel is burned during this time, what is the approximate rate of heat loss (in kJ/min) from the hot air in the bag during the flight?
(a) equal; (b) less than; (c) 29.48 g mol −1 ; (d) 1.0966 g L −1 ; (e) 0.129 g/L; (f) $4.01×10^5$ g; net lifting capacity = 384 lb; (g) 270 L; (h) 39.1 kJ min −1
Show that the ratio of the rate of diffusion of Gas 1 to the rate of diffusion of Gas 2,$\frac{R_1}{R_2}$ is the same at 0 °C and 100 °C.
InertiaLearning
Kinetic theory of gases - topic 3.2.
Bite-sized Kinetic Theory of Gases Study Notes for IB Physics HL/SL
Table of Contents
The Avogadro Constant
- The number of particles in a mole is equal to the Avogadro Constant
- A ‘particle’ can mean an atom or a molecule
- The number of particles in a mole is N A
Formula Booklet
If a substance contains N particles, then the number of moles ‘ n ‘ is given by this formula.
- n = number of moles
- N = Number of particles
- N A = Avogadro’s Constant
The atomic mass unit (1u) is defined as 1/12 of the mass of a carbon-12 atom.
- The mass per one neutron is 1 mole
- The mass per one proton is 1 mole
- Molar mass is the sum of all atomic masses of a molecule
Not in Formula Booklet but important
Unified atomic mass unit
- Pressure is the normal force applied per unit area
- The force is applied normal to the area
- If the force is given by with an angle, then find the vertical component of the angle
- P = Pressure
- Unit: Newton per square metre, Nm -2 = pascal, Pa
- Can also be used: atmospere, atm = 1.013 x 10 5 Pa
Ideal Gases
- An ideal gas is a theoretical model of a real gas
- A real gas can be approximated by an ideal gas at low density (low pressure, high temperature)
An Ideal Gas is a theoretical model of a gas. It is defined by the following assumptions:
- The molecules are point particles – with negligible volume
- The molecules obey the laws of mechanics
- An ideal gas can not be liquefied or solidified
- Molecules have a variety of speeds and move randomly
- There are no forces between the molecules except when the molecules collide
- The duration of a collision is negligible compared to the time between collisions
- The collisions of the molecules with each other and with the container walls are elastic
At very low density (low pressure, high temperature) a real gas will generally behave like an ideal gas.
The Pressure-Volume Law
- Pressure is inversely proportional to volume
The Pressure-Volume Law states that at constant temperature and with a fixed quantity of gas, pressure is inversely proportional to volume.
- This relationship is also known as Boyle’s Law
- The curve is isothermal – the temperature at all points on the curve is the same
- The product pV is the same for all points on the curve
The Volume-Temperature Law
- Volume increases uniformly with temperature
The Volume-Temperature Law states that when temperature is expressed in kelvin, then at constant temperature volume increases uniformly with temperature.
- Charle’s Law
The Pressure-Temperature Law
- Pressure increases uniformly with increasing temperature
The Pressure-Temperature Law states that when temperature is expressed in kelvin and volume is constant, then pressure increases uniformly with increasing temperature.
- Gay-Lussac’s Law or Amonton’s Law
The Equation of state of an Ideal Gas
- The Gas constant (R) is a universal constant
The Equation of state of an Ideal Gas relates Volume, Pressure, Temperature, and the number of moles of a gas. .
- R is the universal gas constant
- p = pressure
- T = temperature
- Through the introduction of the universal gas constant one can now calculate for the missing quantities (with the help of the given quantities)
The Boltzmann Equation
- Calculate the Kinetic Energy of a gas
- The Internal Energy of an ideal gas consists only of its kinetic energy
The molecules of a gas move randomly with a range of speeds.
- k b = Boltzmann constant
- T = Temperature
- E K = Kinetic Energy
The Internal Energy of an ideal gas consists only of the random kinetic energy of its molecules
- N = Number of Molecules
- k B = Boltzmann constant
- Remember the basic rules that characterize an ideal gas
Worksheet - Kinetic Molecular Theory of Gases
Worksheet with answers.
Questions and Answers
Worksheet with Answers 2.0
Ppt (pdf) - kinetic molecular theory of gases, power point presentation, subscribe to the inertia newsletter.
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KINETIC THEORY OF MATTER WORKSHEET AND ANSWERS
Subject: Chemistry
Age range: 14-16
Resource type: Worksheet/Activity
Last updated
7 April 2020
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This worksheet will help to assess and challenge the understanding of students in the behaviour of matter in gaseous, liquid and solid states; rate of diffusion in matter, etc.
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Kinetics (Worksheet)
- Last updated
- Save as PDF
- Page ID 11040
- Mark Draganjac
- Arkansas State University
Name: ______________________________
Section: _____________________________
Student ID#:__________________________
Work in groups on these problems. You should try to answer the questions without referring to your textbook. If you get stuck, try asking another group for help.
1. Write the rate expression in terms of \(\Delta\)[reactant]/\(\Delta\)t and \(\Delta\)[product]/\(\Delta\)t for the reaction:
\[N_2 + 3H_2 \rightarrow 2NH_3 \nonumber \]
2. Determine
- The order of each reactant,
- The order of the reaction,
- Write the rate law and
- Calculate the rate constant, \(k\), for the following data:
3. The decomposition of \(A_2B_3\) is second order with a \(k = 6.5 \times 10^{-5} M^{-1}s^{-1}\) at 25 o C. If the initial concentration is \(0.50\, M\), what is the concentration after \(3 min\)?
4. The decomposition of \(AB\) is first order with a \(k = 2.3 \times 10^{-7} s^{-1}\) at 45 o C. If the initial concentration is 0.25 M, what is the concentration after 2.3 min?
5 What is the concentration of reactant after 2.5 minutes if the initial concentration was \(0.100\, M\) and \(k = 6.93 \times 10^{-3} s^{-1}\) for a first order reaction?
- What is the half-life?
6. For the first order reaction:
\[SO_2Cl_2 \rightarrow SO_2 + Cl_2 \nonumber \]
How long will it take to reach \(0.31 \times 10^{-3}\, M\) if the initial concentration was \(1.25 \times 10^{-3}\; M\) and \(k = 0.17 hr^{-1}\)?
7. The rate constant is \(k = 1.5 \times 10^{-2} M^{-1}s^{-1}\) for the second order reaction
\[A \rightarrow B \nonumber \]
- If the initial concentration of \(A\) is \(0.10\, M\), what is the concentration of \(A\) after 4 min?
- what is the half-life?
Contributors and Attributions
- Mark Draganjac ( Arkansas State University )
IMAGES
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This "Collision Theory Worksheet" ( doc) includes answers. A "Phase Change Worksheet" ( pdf) with answers. Review vocabulary with this "Thermodynamics Worksheet" ( pdf). Have students do the "Kinetic Theory" ( doc) with answers ( doc). Demonstrate the "electron sea model of metals" concept with this " Modeling Metals with Marbles " activity. Labs
Kinetic Theory of Gases (Worksheet)
Theory: an accepted statement about science that has been tested and peer reviewed many times that explains observations (facts) can be used to make predictions. Kinetic: this word means movement. Kinetic energy is energy that has to do with things moving and is stored in objects. To examine: means to look at or study.
1. The Kinetic Theory of Matter states that all matter is composed of are in a constant state of 2. What is Brownian motion, and why does it happen in terms of kinetic theory? that 3. What is thermal expansion, and why does it happen in terms of kinetic theory? 4. What is diffusion, and why does it happen in terms of kinetic theory? 5.
1. Describe how gases, liquids, and solids compare using the following table. Solids Liquids Period Gases Volume (definite or indefinite) Molecular Motion (high, med, low) Distance Between Molecules (g 2. Read page 420: What is kinetic energy? Describe kinetic molecular theory. 3. Identify each statement as True or False.
The word kinetic comes from a Greek word that means "to move.". The kinetic molecular theory is. State the names of the phases in order of Temperature, Kinetic Energy, density and bond strength between atoms. 3. Kinetic Energy is directly related to temperature. As the temperature increases so does the Kinetic Energy.
Unit 10 Gases and kinetic molecular theory. Unit 11 States of matter and intermolecular forces. Unit 12 Chemical equilibrium. Unit 13 Acids and bases. Unit 14 Buffers, titrations, and solubility equilibria. Unit 15 Thermodynamics. Unit 16 Redox reactions and electrochemistry. Unit 17 Kinetics. Unit 18 Nuclear chemistry.
Kinetic Molecular Theory (KNIT) Worksheet Period: Name: Date: Directions: Answer the following questions completely and concisely. 1. What is kinetic energy? 2. Describe the 3 assumptions of the KNIT (Kinetic Molecular Theory). 3. According the KM T, "collisions between particles are perfectly elastic". What does that mean? oe k E SQ-MC 4.
Q8. Freon-12 is used as a refrigerant in central home air conditioners. The rate of effusion of Freon-12 to Freon-11 (molar mass = 137.4 g/mol) is 1.07:1. Which formula is correct for Freon-12: CF4 C F 4, CF3Cl C F 3 C l, CF2Cl2 C F 2 C l 2, CFCl3 C F C l 3, or CCl4 C C l 4. Hint: use Graham's Law of Effusion.
Q9. Define vapor pressure. the pressure of the vapor over a liquid at equilibrium (meaning that as many molecules are going into the vapor state as there are gas molecules going back into the liquid state) this is measured in a closed container.
docx, 2.92 MB Kinetic theory worksheet will help and challenge students to learn the particle behaviour in solids, liquids and gases on the application of heat, pressure and concentration. it also treats the change of state of matter. Answers have also been included. Tes paid licence How can I reuse this?
Solution Describe what happens to the average kinetic energy of ideal gas molecules when the conditions are changed as follows: (a) The pressure of the gas is increased by reducing the volume at constant temperature. (b) The pressure of the gas is increased by increasing the temperature at constant volume.
1. The word kinetic comes from a Greek word that means "to move." The kinetic molecular theory is based upon the assumption that particles of matter (atoms or molecules) are in constant random motion. 2. Of the three states of matter, which one has the most kinetic energy? Gas 3.
A real gas can be approximated by an ideal gas at low density (low pressure, high temperature) An Ideal Gas is a theoretical model of a gas. It is defined by the following assumptions: The molecules are point particles - with negligible volume. The molecules obey the laws of mechanics. An ideal gas can not be liquefied or solidified.
solid, liquid and gas. Kinetic theory explains the properties of solid,liquid and gases in terms of the energy possessed by the particles and. the forces that act between the particles. According to Kinetic theory, most significant difference between the gas and liquid is. the distance between the particles. An ideal gas is an imaginary gas that.
Kinetic Molecular Theory Worksheet Use the following terms to fill in the blanks. Some may be uses more than once. Hopefully all will be included but you never know. If you seem to need an additional term (oops!) just do your best Gas Solid Liquid Phase Compress Empty Space Kinetic Energy Bonds Structure Collisions ...
Q14.1.6. In a typical laboratory setting, a reaction is carried out in a ventilated hood with air circulation provided by outside air. A student noticed that a reaction that gave a high yield of a product in the winter gave a low yield of that same product in the summer, even though his technique did not change and the reagents and concentrations used were identical.
a liquid's particles have enough energy to escape the attractive forces of the other particles in the liquid. the pressure of a liquid's vapor is equal to the pressure of the atmosphere, and the liquid becomes a gas. Study with Quizlet and memorize flashcards containing terms like States of matter, Kinetic Theory, All matter is compose of small ...
docx, 54.06 KB. This worksheet will help to assess and challenge the understanding of students in the behaviour of matter in gaseous, liquid and solid states; rate of diffusion in matter, etc. Tes paid licence How can I reuse this? Report this resource to let us know if it violates our terms and conditions. Our customer service team will review ...
Pump gas molecules to a box and see what happens as you change the volume, add or remove heat, and more. Measure the temperature and pressure, and discover how the properties of the gas vary in relation to each other. Examine kinetic energy and speed histograms for light and heavy particles. Explore diffusion and determine how concentration, temperature, mass, and radius affect the rate of ...
1. Write the rate expression in terms of Δ Δ [reactant]/ Δ Δ t and Δ Δ [product]/ Δ Δ t for the reaction: N2 + 3H2 → 2NH3 N 2 + 3 H 2 → 2 N H 3. 2. Determine. The order of each reactant, The order of the reaction, Write the rate law and. Calculate the rate constant, k k, for the following data:
Kinetic Molecular Theory What is Kinetic Energy? Activities (Select 2-3): Exploring KMT: For this activity you will be researching Kinetic Molecular Theory, and creating a project or presentation to teach others. To start, watch The Kinetic Theory of Matter. Then, use Explora and World Book Student to research the KMT. Your project should ...
Quiz Course Try it risk-free for 30 days Instructions: Choose an answer and hit 'next'. You will receive your score and answers at the end. question 1 of 3 Which is not a phase of matter? Solid...