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GTCC CHEM 131
Exam 3 Review
| Question | Answer |
|---|---|
| Chemical Reaction is what kind of change | Chemical Change |
| Law of Conservation of Mass | Reactants and Products number of atoms must equal no matter lost or gained in a chemical reaction |
| What balances Chemical Equations | Coefficients |
| Do you add or multiply Coefficients by Subscripts | Multiply |
| What must we never change | Subscripts |
| What happens when you have an odd number as a coefficient | change the odd number to an even number by multiplying the the whole equation by 2 |
| If the coefficients have a common factor what must you do | Simplify |
| What does the triangle over the reaction represent | Heat |
| What does aq next to an element or compound mean | aqueous solution |
| What does s next to an element or compound mean | Solid |
| What does L next to an element or compound mean | Liquid |
| What does G next to an element or compound mean | Gas |
| What are the 6 types of Reactions | Combination Single Replacement Double Replacement Decomposition Oxidation and Reduction Combustion |
| Describe Combination | Metal and Nonmetal react to form compounds Formula determined by ionic charge |
| Always__________ the types of reactions | Balance |
| Li+ Br2---- LiBr is an example of what kind of reaction | Combination |
| What are the Diatomic Elements | H2, N2,O2, F2,Cl2, Br2, I2 |
| Describe Decomposition | A--B+C Compound, Element + Element Compound , Compound, Element Compound, Compound, Compound |
| Describe Combustion | Reaction of Carbon and Hydrogen and Oxygen and always resulting in Carbon Dioxide and Water CO2 and H20 |
| Describe Single Replacement | A+BC-- AC + B One Element replaces another to form Products Also Deals with ionic Charges to make the Products |
| Describe Double Replacement | Combine Cation with Anion of Second Substance then Combine Anion with Cation of Second Substance Uses Ionic Charges to form Products in the chemical formula |
| AgNO3+NaCl----- AgCl +NaNO3 is an example of what reaction | Double Replacement |
| Describe Oxidation and Reduction Reaction | Oxidation is Loss OIL Reduction is Gain RIG What is oxidized or reduced in a chemical equation |
| What charge does Oxidation have | Positive |
| What charge does Reduction have | Negative |
| Oxidation has a Gain/ Loss of Oxygen | Gain |
| Reduction has a Gain/ Loss Oxygen | Loss |
| Oxidation has a Gain/ Loss of Hydrogen | Loss |
| Reduction has a Gain/ Loss of Hydrogen | Gain |
| Zn+Cu2+----- Zn2+Cu What is this an example of | Oxidation and Reduction Reaction |
| Zn+Cu2+----- Zn2+Cu What is Oxidized in this Chemical Equation | Zn is being Oxidized Going from 0 to 2 |
| Zn+Cu2+----- Zn2+Cu What is Reduced in this Chemical Equation | Cu is being reduced Going from 2 to 0 |
| When Predicting the Products in a formula what do you use to make the Products | Ionic Charges |
| After we write the product from ionic charges what do we do after that | Balance |
| The Mole is what | Unit of Measurement |
| The Mole can be in what units of Measurement | Gram, Liter, Kilometer |
| SI Unit the Mole is what | 6.022x10 to the 23rd power Particles |
| 6.022x10 to the 23rd can be said what number | Avogadros Number |
| Mole can convert atomic mass units amu to what | Grams |
| Moles can be described as what | The number of particles |
| What are the Mole Conversions | Mole-Mole-1 step Mole to Gram-2step Gram to Gram-3step |
| How do we find Molar Mass like NaOH | Mass of one mole of a substance Adding up all the masses of the elements to get the total molar mass Na-22.99 O-16.0 H-1.01 |
| In Molar Mass what are the units of measurement with the Solution | g/mol |
| 1 mole is equal to what atoms of the element | 6.022x10 to the 23rd power |
| Round to the nearest____________ place when dealing with Molar Mass | Tenths 0.1g 1 use at least 3 sig figs in calculations |
| Limiting Reactant | Limits the amount of product formed |
| What makes the Percent Yield | Actual Yield and Theoretical yield divided and multiplied 100 |
| Theoretical Yield | amount of product 100 percent we would expect if all reactants are converted to desired products |
| Actual Yield | When reactions end we measure and collect the mass of the products |
| Excess Reactant | is what is left over |
| Limiting Reactant | is what is used up 1st |
| Which one do you calculate Theoretical Yield or Actual Yield | Theoretical |
| Which value is given Theoretical Yield or Actual Yield | Actual |
| How do you find Percent Yield | Percent Yield= Actual / theoretical X100 |
| What are the 4 questions you need to do a LR Problem | What is LR > Balance equation if not already How much product do you make in Moles When RXN is complete how many moles of N remain: Always 0 When Rxn is complete hwo many moles of H2( other reactant) remain ( moleof LR - to mol of what remain) |
| Whatever isn't the LR, is the______ | Excess Reactant |
| Percent Yield is a what step process | 3 step process Grams to Grams > Theoretical Yield Given Actual Yield Divide and multiply by 100 Actual / Theoretical |
| To get an energy change in a reaction, reactions must_____ | Collide |
| To get an energy change in a reaction, reactions must______ | Collide with sufficient energy to overcome activation energy Break Bonds |
| Activation energy | the amount of energy to break bonds of the reactants |
| If the energy is less what happens to the energy | bounces apart but not breaks or reacts |
| Define Enthalpy | Heat |
| What are the two types of reactions | Endothermic Exothermic |
| Describe Endothermic | Positive energy of products> Energy of reactants greater than Heat absorbed |
| Describe Exothermic | Negative energy , energy of product < Energy of reactants Heat released on Product Side |
| How do you find Heat | Use Grams-mol / mole/KJ |
| Charges for Exothermic | Releasing energy |
| What is the exact number in KJ we can use in a Heat equation | 483.6 KJ |
| What changes reaction rates | Concentration Temperature Catalyst |
| Changes in reaction dealing with concentration | Concentration increases and Reaction rate increases Increasing the number of collisions |
| Changes in reaction dealing with Temperature | Higher temperature increases reaction rate increasing kinetic energy of molecules |
| Changes in reaction dealing with catalysts | Lower energy / higher reaction rate Not consumed in a reaction or in a balanced equation |
| What are the states of matter | Solid , Liquid ,Gas |
| Describe Solid | Volume is definite , Shape is definite |
| How are the particles for a Solid | Tightly packed |
| Describe Liquid | Volume is Definite , Shape takes the shape of the container |
| How are the particles for a Liquid | Closely packed |
| Describe Gas | Volume Indefinite , Shape no definite shape |
| Kinetic Molecular Theory of Gas Rule 1 | Contains small particles ( Atoms, Molecules) move randomly and at high speeds |
| Kinetic Molecular Theory of Gas Rule 2 | Gases don't attract or repel each other |
| Kinetic Molecular Theory of Gas Rule 3 | Actual Volume of gas particles small compared to volume of container |
| Kinetic Molecular Theory of Gas Rule 4 | Gas particles are in constant motion |
| Kinetic Molecular Theory of Gas Rule 5 | Speed of gas particles increase as temperature increases |
| Physical Properties of Gas | Pressure , Volume, Temperature (Always in Kelvins), amount of Moles if not you have to convert it to Kelvins |
| Formula for converting to Kelvins if in Celsius or Fahrenheit | K=C+273 F=Cx1.8+32 |
| Pressure is the force exerted _____ | Per unit area P=F/A Pressure=Force/ Area |
| Force is the exertion by gas particles on_____ | Walls of container |
| Boyle's Law | P and V P1V1=P2V2 |
| What is the constant of Boyle's Law | n, T Moles and Temp. |
| With Boyle's Law the volume is half but the Pressure ____ | Doubles |
| If the Volume is in ml How do you convert it to L | 1L=1000mL 1mL+ 0.001 |
| Boyle's deals with what real life application | Breathing |
| During Inhalation what happens with Boyle's Law | Lungs Expand Pressure Decrease as Volume Increases |
| During Exhalation what happens with Boyle's Law | Lung Volume decreases Pressure Increases as Volume Decreases in lungs --- to the outside |
| Air always goes from what concentration gradient | High to low |
| Charles Law | V, T V1/T1= V2/T2 |
| With Charles Law what happens if the temp doubles , the Volume ____ | Doubles |
| Charles law is Proportional which means to solve you have to ____ | Cross Multiply and divide |
| Always remember what in every calculation | Sig Figs |
| Gay Lussac's Law | P ,T P1/T1= P2/T2 |
| With Gay Lusacc's Law what happens if the pressure doubles, what happens to the temp______ | Doubles |
| psi is another unit for____ | atm |
| 1atm=____ | 760mmHG |
| Gay Lussac's Law also has what Pressure associated with it | Vapor Pressure |
| Vapor Pressure | any pressure , vapor exists over that liquid |
| To boil a liquid the VP must be______ | Equal to the external Pressure |
| If External Pressure is higher than what else would be increased | VP, BP( Boiling Point) Ex: Autoclave |
| If External Pressure is lower, than what else would be decreased | VP, BP (Boiling Point) Ex: Boiling water in Denver |
| Combined Gas Law | Combines all the law Boyle's, Charles, Gay Lusacc's P1V1/T1= P2V2/T2 ( Peas and Veggies on the Table) |
| What is the constant for Charles Law | n, p |
| What is the constant for Gay Lussac's Law | n, v |
| What is the constant for the Combined Gas law | n |
| Avogadro's Law | V, N V1/N1=V2/N2 |
| What is the constant for Avogadro's Law | p, t |
| Avogadro's Law has what standard___ | Temp , and Pressure |
| What is the Standard Temp | 273K |
| Temperature must always be in what units______ | Kelvins |
| What is the Standard Pressure | 1.0 atm |
| Any 1 mole of gas has what volume | 22.4L |
| Ideal Gas Law | Combined Gas Law and Avogadro's Law PV=NRT with STP T:273K, P: 1.0 atm |
| What does R stand for | 0.0821 Lxatm/molxK- Not a formula just units to cancel out |
| Moles= Mass/ Molar Mass | Convert to Kelvin first if need to , then find the moles in PV=NRT, After divide it by the amount of grams you have that result use to find the element on the periodic table |
| To find an element on the periodic table then search what columns | Halogens and Noble Gases and Even Diatomic's |
| Diatomic's | always come in 2's if the element isn't a halogen or a noble gas then divide result by 2 to find the diatomic's mass number |
| What are the Diatomic's | H2, N2, O2, F2, CL2 |
| What are the Noble Gases | Far Right on the Periodic Table He, Ne, Ar, Kr, Xe, Rn |
| Halogens are where on the periodic table | one column to the left of the Noble Gases |
| Gases and Stoichiometry use what formula | PV=NRT |
| If the problem has moles and Liters missing find the moles first by what conversion | moles to moles |
| After you find moles then find the Liter in what formula | PV=NRT |
| Dalton's Law of Partial Pressure | Total P= Pa+Pb+Pc Add them together |
| If you have some of the elements pressure but not the last one but have the total P you can what to find the difference of the one missing element 's p | Subtract |
| What are the two types of Ozone Layer | Stratospheric (O3) Ground Level |
| Does Stratospheric Ozone Layer helps or harms the environment | Helps to block harmful UV rays Destroyed by CFC- Chloroflurocarbon -Catalyzes 03+O=O2 |
| Does Ground Level Ozone Layer is it harmful or helpful | Harmful- Main Component of smog Formed by a rxn NOX +_VOC + Heat (Sunlight) |
| Ground Level Ozone Layers come from what | Vehicles and Electric utilities |
| Carbon Dioxide is what kind of source | Natural |
| The Natural Source for Carbon Dioxide comes from what examples | Volcano eruptions, forest fires , cellular respiration |
| Anthropogenic is what kind of example of Carbon Dioxide | Combustion of fossil fuels CxHy+02-CO2+H20 |
| The Carbon Dioxide in the environment is called | Atmospheric Carbon Dioxide |
| If you have an increase in Atmospheric Carbon Dioxide what effect does it have | Greenhouse Effect |
| How does the Greenhouse effect work | Thermal Energy from plants re-radiated / Temperature Increases and Impacts the environment |
| Gases expand to fill what ______ | it's container |
| Tire Pressure gets low in the fall what do you do to your tires Add more Air, Release Air, Nothing | Add Air in the Tires |
| In the summer when it is Hot the temperature increases what should you do to alleviate your pressure in your tires | Let some air out |
| What Law makes this possible: Helium in a hot air balloon | Charles Law T, V, |
| What law makes this possible: Equalizing of pressure out of a balloon | Avogadro's Law V, n(Moles) |
Created by:
aphastings