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Chemistry Unit 3 Study Guide

Chemistry Unit 3 Study Guide. You may use this study guide to review for your test; practice your new skills or review old concepts. Each topic has several questions relating to it, this should help with giving you plenty of practice. Boyle’s Law A. What does Boyle’s Law state?.

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Chemistry Unit 3 Study Guide

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  1. ChemistryUnit 3 Study Guide You may use this study guide to review for your test; practice your new skills or review old concepts. Each topic has several questions relating to it, this should help with giving you plenty of practice.

  2. Boyle’s Law A What does Boyle’s Law state? That as the pressure on a gas increases the volume will decrease.

  3. Boyle’s Law B What type of relationship do we see in Boyle’s Law? Indirect relationship; as one variable goes up the other goes down.

  4. Boyle’s Law C Using the Kinetic Theory of Matter explain how Boyle’s Law works. Kinetic Theory states that the particles in a gas are very far apart. Therefore when you compress a gas the particles move closer but do not have contact.

  5. Charles’ Law A What does Charles’ Law state? That as you increase the temperature on a gas the volume will increase also.

  6. Charles’ Law B What type of relationship do we see in Charles’ Law? Direct Relationship, as one variable goes up so does the other.

  7. Charles’ Law C Using the Kinetic Theory of Matter explain how Charles’ Law works. Kinetic Theory states that as the temperature increases the atoms which are in constant motion will move faster and expand. This causes an increase in volume.

  8. Combined Gas Law A What is the combined gas law? It is the combination of Boyle’s and Charles’ Law because it is rare in the real world that only one variable will change at a time.

  9. Combined Gas Law B What is the equation for the combined gas law? P1V1/T1 = P2V2/T2 or PV/T = k

  10. Combined Gas Law C Describe a circumstance in which the combined gas law would be used. Your answer should include a discussion of a temperature change and/or a pressure change and how the volume would change because of that.

  11. States of Matter A What are the three states of matter and how are they different according to the Kinetic Theory of Matter? Solid: very slow moving, close together particles Liquid: faster moving, they move in two dimensions Gas: very fast moving and very far apart, they move in three dimensions

  12. States of Matter B Is there ever a time where we can have more than one state of matter of the same material existing at a time? Yes, anytime it is going through a phase change we have two states existing at the same time.

  13. States of Matter C What do we call all the changes in phase and what phases are they going to? Melting: solid-liquid Boiling: liquid-gas Evaporation: liquid- gas below boiling Condensation: gas- liquid Freezing: liquid- solid Sublimation: solid-gas

  14. Conservation of Mass A What does the Law of Conservation of Mass state? That matter(mass) is neither created nor destroyed it simply changes form. This means that we cannot lose any mass in a chemical reaction.

  15. Conservation of Mass B Conservation of Mass is used as the reason that we balance chemical equations; please explain why. If mass cannot be created or destroyed then the number of atoms on one side of the chemical reaction should match the number on the other side.

  16. Conservation of Mass C When you balance an equation do the elements have to be combined in the same way on both sides of the equation? No, as long as there is the same number of elements of each type.

  17. Phase Diagrams A Using the phase diagram below please explain what is happening at the S-L line. At the S-L line the substance is melting and freezing at various pressures.

  18. Phase Diagrams B What is the pressure when the substance condenses at 50C? 200 mmHg; 400 mmHg; 20 mmHg About 200 mmHg

  19. Phase Diagrams C What is the triple point? It is the point at which all 3 states of matter can exist at the same time.

  20. Kinetic Molecular Theory A What does the kinetic theory state? All gases consist of molecules and that those molecules are in motion. They are very far apart compared to solids and liquids and when they collide with each other it is perfectly elastic. The attractive forces between the gas molecules is very weak and that the temperature of a gas is directly proportional to the average kinetic energy of the gas

  21. Kinetic Molecular Theory B Using the kinetic theory explain why a liquid thermometer reads higher at higher temperatures. The higher the temperature the faster the particles move and the more they collide with the thermometer. As they collide faster they apply pressure to the outside of the thermometer causing the liquid inside to rise higher.

  22. Kinetic Molecular Theory C What do the dotted lines indicate on the graph below? The boiling points for each set of molecules.

  23. Balancing Equations A Balance the following equation: __H2SO4 +__ NaCl→ __Na2SO4 +__ HCl 1; 2; 1; 2

  24. Balancing Equations B Balance the following equation: __KI + __BPO4 → __K3PO4 + __BI3 3; 1; 1; 1

  25. Balancing Equations C Balancing the following equation: __C6H12O6 + __O2 → __CO2 + __H2O 1; 6; 6; 6

  26. Gas Law Equations A A gas has an initial pressure of 1 atm and a volume of 4.6L. Pressure is applied to the gas decreasing the volume to 2.2 L, what is the new pressure? 1atm x 4.6L = 2.2L x ? ? = 2.1 atm

  27. Gas Law Equations B A gas has a temperature of 125 C and a volume of 11.3 L, if the volume is increased to 5.3 L what is the new temperature? 11.3L/ 398 = 5.3L / T 189 K

  28. Gas Law Equations C A gas has a volume of 12.3 mL at STP, what volume will it occupy at 100C and 4 atm? 12.3 ml( 1atm)/ 273 = V(4 atm)/373 4.20 ml

  29. Graphs A What law does the following graph represent? What relationship is it? Indirect relationship; Boyle’s Law

  30. Graphs B What relationship is shown by the graph below, what gas law is it? Direct relationship; Charles’ Law

  31. Graphs C In the graph below, as we move to the right what is happening to the temperature? It is increasing

  32. Mole Calculations A If there is 55 g of CO2 gas, how many moles is that? 55 g / 44 g/mole = 1.25 moles of CO2

  33. Mole Calculations B If we have 3 moles of a gas how many liters does it take up? 3 moles x 22.4 L/mole = 67.2 L

  34. Mole Calculations C If there 1.204 x 1024 molecules of H2 in a beaker, how many L will that take up? 1.204 x 10 24/ 6.02 x 1023 = 2 moles 2 moles x 22.4 L /mole = 44.8 L

  35. Kelvin Scale A How do we convert between C and K? K = C +273

  36. Kelvin Scale B What do we convert to Kelvin when we solve Charles and Combined gas law equations? Because the Kelvin scale is based on absolute zero you can never have a negative value.

  37. Kelvin Scale C What is 551 K in C? 278 C

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