VIBRATIONS AND WAVES - Simon Technology
NameDateClass11StoichiometrySection 11.1What is stoichiometry?In your textbook, read about stoichiometry and the balanced equation.For each statement below, write true or false.1. The study of the quantitative relationships between the amounts of reactantsused and the amounts of products formed by a chemical reaction is calledstoichiometry.2. Stoichiometry is based on the law of conservation of mass.3. In any chemical reaction, the mass of the products is less than the mass of thereactants.4. The coefficients in a chemical equation represent not only the number ofindividual particles but also the number of moles of particles.5. The mass of each reactant and product is related to its coefficient in thebalanced chemical equation for the reaction by its molar mass.Complete the table below, using information represented in the chemical equation for thecombustion of methanol, an alcohol.methanol oxygen carbon dioxide water2CH3OH(l) 3O2 (g) 2CO2(g) 4H2O(g)SubstanceMolar Mass (g/mol)6. Methanol32.057. Oxygen gas32.008. Carbon dioxide44.019. Water18.02Number of MoleculesNumber ofMoles (mol)Mass (g)10. What are the reactants?11. What are the products?12. What is the total mass of the reactants?13. What is the total mass of the products?14. How do the total masses of the reactants and products compare?Chemistry: Matter and Change1Study Guide
NameDateClass1311Section 11.1 continuedIn your textbook, read about mole ratios.Answer the questions about the following chemical reaction.sodium iron(III) oxide sodium oxide iron6Na(s) Fe2O3(s) 3Na2O(s) 2Fe(s)15. What is a mole ratio?16. How is a mole ratio written?17. Predict the number of mole ratios for this reaction.18. What are the mole ratios for this reaction?19. What is the mole ratio relating sodium to iron?20. What is the mole ratio relating iron to sodium?21. Which mole ratio has the largest value?Chemistry: Matter and Change2Study Guide
NameDateClass1311Section 11.2Stoichiometric CalculationsIn your textbook, read about mole-to-mole conversion.Read the following passage and then solve the problems. In the equation that follows each problem,write in the space provided the mole ratio that can be used to solve the problem. Complete theequation by writing the correct value on the line provided.The reaction of sodium peroxide and water produces sodium hydroxide and oxygengas. The following balanced chemical equation represents the reaction.2Na2O2(s) 2H2O(l) 4NaOH(s) O2(g)1. How many moles of sodium hydroxide are produced when 1.00 mol sodium peroxide reacts withwater?1.00 mol Na2O2 mol NaOH2. How many moles of oxygen gas are produced when 0.500 mol Na 2O2 reacts with water?0.500 mol Na2O2 mol O23. How many moles of sodium peroxide are needed to produce 1.00 mol sodium hydroxide?1.00 mol NaOH mol Na2O24. How many moles of water are required to produce 2.15 mol oxygen gas in this reaction?2.15 mol O2 mol H2O5. How many moles of water are needed for 0.100 mol of sodium peroxide to react completely in thisreaction?0.100 mol Na2O2 mol H2O6. How many moles of oxygen are produced if the reaction produces 0.600 mol sodium hydroxide?0.600 mol NaOH Chemistry: Matter and Change mol O23Study Guide
NameDateClass1311Section 11.2 continuedIn your textbook, read about mole-to-mass and mass-to-mass conversions.Solving a mass-to-mass problem requires the four steps listed below. The equations in the boxesshow how the four steps are used to solve an example problem. After you have studied the example,solve the problems below, using the four steps.Example problem: How many grams of carbon dioxide are produced when 20.0 g acetylene (C 2H2) is burned?Solution2C2H2(g) 5O2(g) 4CO2(g) 2H2O(g)20.0 g C2 H 2 ﾴ1 mol C 2 H 226.04 g C2 H 2 0.768 mol C 2 H 20.768 mol C2 H 2 4 mol CO 22 mol C 2 H 2 1.54 mol CO 21.54 mol CO 2 44.01 g CO 21 mol CO 2 67.8 g CO 2Step 1 Write a balanced chemical equation for the reaction.Step 2 Determine the number of moles of the known substance, usingmass-to-mole conversion.Step 3 Determine the number of moles of the unknown substance, usingmole-to-mole conversion.Step 4 Determine the mass of the unknown substance, using mole-to-massconversion.Chemistry: Matter and Change4Study Guide
NameDateClass13117. In some mole-to-mass conversions, the number of moles of the known substanceis given. In those conversions, which step of the above solution is not necessary?8. In a blast furnace, iron and carbon monoxide are produced from the reaction of iron(III) oxide(Fe2O3) and carbon. How many grams of iron are formed when 150 g iron(III) oxide reacts with anexcess of carbon?9. Solid sulfur tetrafluoride (SF4) and water react to form sulfur dioxide and an aqueous solution ofhydrogen fluoride. How many grams of water are necessary for 20.0 g sulfur tetrafluoride to reactcompletely?Chemistry: Matter and Change5Study Guide
NameDateClass1311Section 11.3Limiting ReactantsIn your textbook, read about why reactions stop and how to determine the limitingreactant.Study the diagram showing a chemical reaction and the chemical equation that represents thereaction. Then complete the table. Show your calculations for questions 25–27 in the space belowthe table.O2 2NO 2NO2The molar masses of O2, NO, and NO2 are 32.00 g/mol, 30.01 g/mol, and 46.01 g/mol, respectively.Amount of O2Amount of NOAmount of NO2Limiting ReactantAmount and Nameof Excess Reactant1 molecule2 molecules2 moleculesnonenone4 molecules4 molecules4 moleculesNO2 molecules O22 molecules8 molecules1.2.3.1.00 mol2.00 mol4.5.6.4.00 mol4.00 mol7.8.9.5.00 mol7.00 mol10.11.12.1.00 mol4.00 mol13.14.15.0.500 mol0.200 mol16.17.18.32.00 g60.02 g19.20.21.16.00 g80.00 g22.23.24.10.00 g20.00 g25.26.27.Chemistry: Matter and Change6Study Guide
NameDateClass1311Section 11.4Percent YieldIn your textbook, read about the yields of products.Study the diagram and the example problem.Example Problem: The following chemical equation represents the production of gallium oxide, asubstance used in the manufacturing of some semiconductor devices.4Ga(s) 3O2(g) 2Ga2O3(s)In one experiment, the reaction yielded 7.42 g of the oxide from a 7.00-g sample of gallium. Determinethe percent yield of this reaction. The molar masses of Ga and Ga 2O3 are 69.72 g/mol and 187.44 g/mol,respectively.Use the information in the diagram and example problem to evaluate each value or expressionbelow. If the value or expression is correct, write correct. If it is incorrect, write the correct value orexpression.1. actual yield: unknown2. mass of reactant: 7.00 g Ga3. number of moles of reactant: 7.00 g Ga 69.72 g Ga1 mol Ga4. number of moles of product: 0.100 mol Ga 5. theoretical yield: 0.0500 mol Ga 2 O 3 6. percent yield:2 mol Ga 2 O 31 mol Ga187.44 g Ga 2 O 31 mol Ga 2 O 39.37 g Ga 2 O 3 1007.42 g Ga 2 O 3Chemistry: Matter and Change7Study Guide
TEACHER GUIDE AND ANSWERSSection 11.2 Stoichiometric CalculationsStudy Guide - Chapter 11 – Stoichiometry1. 4 mol NaOH/2 mol Na2O2, 2.00Section 11.1 What is stoichiometry?2. 1 mol O2/2 mol Na2O2, .2501. true3. 2 mol Na2O2/4 mol NaOH, 0.5002. true4. 2 mol H2O/1 mol O2, 4.303. false5. 2 mol H2O/2 mol Na2O2, 0.1004. true6. 1 mol O2/4 mol NaOH, 0.1505. true7. Step 26. 2, 2, 64.108. Fe2O3(s) 3C(s) 2Fe(s) 3CO(g)7. 3, 3, 96.00150 g Fe 2 O 3 ﾴ1 mol Fe 2 O3 /159.7 g Fe 2 O 3 8. 2, 2, 88.020.939 mol Fe 2 O39. 4, 4, 72.080.939 mol Fe 2 O 3 ﾴ 2 mol Fe/1 mol Fe 2 O 3 1.88 mol Fe1.88 mol Fe 55.85 g Fe/1 mol Fe 105 g Fe10. methanol and oxygen gas11. carbon dioxide and water12. 160.10 g9. SF4(s) 2H2O(l) SO2(g) 4HF(aq)13. 160.10 g20.0 g SF 4 ﾴ1 mol SF4 /108.07 g SF 4 14. They are equal.0.185 mol SF415. A mole ratio is a ratio between the numbers of moles0.185 mol SF 4 ﾴ 2 mol H 2 O/1 mol SF 4 of any two substances in a balanced chemicalequation.0.370 mol H 2 O16. A mole ratio is written for two substances in abalanced chemical equation as a fraction by placingthe number of moles of one substance in thenumerator and the number of moles of anothersubstance in the denominator.17. 1218.1 mol Fe2O3/6 mol Na3 mol Na2O/6 mol Na2 mol Fe/6 mol Na6 mol Na/1 mol Fe2O33 mol Na2O/1 mol Fe2O32 mol Fe/1 mol Fe2O36 mol Na/3 mol Na2O1 mol Fe2O3/3 mol Na2O2 mol Fe/3 mol Na2O6 mol Na/2 mol Fe1 mol Fe2O3/2 mol Fe3 mol Na2O/2 mol Fe19. 6 mol Na/2 mol Fe20. 2 mol Fe/6 mol Na21. 6 mol Na/1 mol Fe2O3Chemistry: Matter and Change8Teacher Guide and Answers
TEACHER GUIDE AND ANSWERSAmount of O2Amount of NOAmount of NO2Amount and Name ofLimiting Reactant Excess Reactant1 molecule2 molecules2 moleculesnonenone4 molecules4 molecules4 moleculesNO2 molecules O22 molecules8 molecules1.00 mol1. 4 molecules2. O23. 4 molecules NO2.00 mol4. 2.00 mol5. none6. none4.00 mol4.00 mol7. 4.00 mol8. NO9. 2.00 mol O25.00 mol7.00 mol10. 7.00 mol11. NO12. 1.50 mol O21.00 mol4.00 mol13. 2.00 mol14. O215. 2.00 mol NO0.500 mol0.200 mol16. 0.200 mol17. NO18. 0.400 mol O232.00 g60.02 g19. 92.02 g20. none21. none16.00 g80.00 g22. 46.01g23. O224. 50.12 g NO10.00 g20.00 g25. 28.76 g26. O227. 1.24 g NO0.370 mol H 2 O ﾴ18.02 g H 2 O/1 mol H 2 O 6.67 g H 2 OSection 11.4 Percent Yield1. 7.42 g Ga2O3balanced equation mole ratio 2 mol NO/1 mol O 210.00 g O 2 ﾴ1 mol O 2 /32.00 g O0.3125 mol O 22. correct23. 7.00 g Ga 1 mol Ga/69.72 g Ga 4. 0.100 mol Ga 2 mol Ga2O3/4 mol Ga20.00 g NO ﾴ1 mol NO/30.01 0.6664 mol NOactual mole ratio 0.6664 mol NO/0.3125 molO 2 2.132 mol NO/1.000 mol O 25. correct6. 7.42 Ga2O3/9.37 g Ga2O3 100Because the actual mole ratio of NO:O2 is larger thanthe balanced equation mole ratio of NO:O2, there isan excess of NO; O2 is the limiting reactant.Mass of NO used 0.3125 mol O 2 ﾴ 2 mol NO/1 mol O 2 0.6250 mol NO0.6250 mol NO ﾴ 30.01 g NO/1 mol NO 18.76 g NOMass of NO 2 produced 0.6250 mol NO 2 ﾴ 46.01 g NO 2 /1 mol NO 28.76 g NO 22Excess NO 20.00 g NO 18.76 g NO 1.24 g NOChemistry: Matter and Change9Teacher Guide and Answers
TEACHER GUIDE AND ANSWERS Study Guide - Chapter 11 – Stoichiometry Section 11.1 What is stoichiometry? 1. true 2. true 3. false 4. true 5. true 6. 2, 2, 64.10 7. 3, 3, 96.00 8. 2, 2, 88.02 9. 4, 4, 72.08 10. methanol and oxygen gas 11. carbon dioxide and water 12. 160.10 g 13. 160.10 g 14. They are equal. 15. A mole ratio is a ratio between .
electromagnetic waves, like radio waves, microwaves, light, and x-rays are examples of transverse waves. Longitudinal waves travel through a medium in a direction parallel to the direction of travel of the wave. Mechanical waves such as sound waves, seismic waves created by earthquakes, and explosions are all examples of longitudinal waves.
Q: What are mechanical waves? A: Waves that require a medium in which to travel. A medium is the _ that waves travel through o Mediums can be solid, liquid, or gas Examples of mechanical waves include sound waves, seismic waves, ocean waves, etc Q: Describe two types of mechanical waves.
College physics Semester 2 Unit 2 What is a wave? How do they act? How are do waves differ? 1/29 Pre-test Waves on a String. Notes: Introduction to Waves . Lab: Waves on a String Activity (PhET) Do: read 12.3 p457 (1,3,5) 1/30 Clicker questions: Waves on a String. Lab: Fourier-Making Waves part 1 (PhET) 2/1 Lab: Fourier-Making Waves part 2 (PhET)
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whereas the water waves move perpendicularly to the boat. 3. Answers may vary. Sample answer: Sound waves and shock waves are examples of longitudinal waves. In these waves, the disturbance travels along the same axis as the motion of the wave. 4. The "wave" is not a true mechanical wave because there is no equilibrium point in the motion.
AA242B: MECHANICAL VIBRATIONS 1/50 AA242B: MECHANICAL VIBRATIONS Undamped Vibrations of n-DOF Systems These slides are based on the recommended textbook: M. G eradin and D. Rixen, \Mechanical Vibrations: Theory and Applications to Structural Dynamics," Second Edition, Wiley, John & Sons, Incorporated, ISBN-13:9780471975465 1/50
Waves and Thermodynamics MASTERING PHSICS 3.4 Electromagnetic Waves Conduct investigations to explain and analyse differences between mechanical and electromagnetic waves. Electromagnetic waves Electromagnetic transverse waves are different from transverse matter waves in that they: Can travel through a vacuum.
electromagnetic waves we can see. We see these waves as the colors of the rainbow. Each color has a different wavelength. Red has the longest wavelength and violet has the shortest wavelength. When all the waves are seen together, they make white light. Visible light waves are the only electromagnetic waves we can see.
