Final Exam Study Guide: Gases, Solutions, Kinetics & Equilibrium
School
Monroe Township High School**We aren't endorsed by this school
Course
CHEM PHYSICAL C
Subject
Chemistry
Date
Dec 10, 2024
Pages
10
Uploaded by ProfessorWhale2930
Name: Block:Final Exam Study Guide Directions: The following concepts should be included in the preparation for your final exam. At the end of the conceptual outline, you will find general practice problems to continue preparation. Good luck and study hard! Conceptual Outline Gases 1.Conversions and relationships a.For example: i.Know how to convert between various units of pressure. ii.How do you convert from degrees Celsius to degrees Kelvin? iii.How do you convert from grams to moles? 2.The definition and main parts of the kinetic molecular theory. 3.Be able to analyze pictures of gas molecules/be able to draw pictures of gas molecules to determine the pressure, volume, temperature, kinetic energy, etc. 4.Know the variables that affect a gas. a.Volume, temperature, moles and pressure b.What does STP stand for? c.How many liters are in one mole of a substance at STP? 5.Be able to sketch the graphs about how the various units relate to each other (i.e. graph the relationship between pressure and volume, temperature and volume, etc.) 6.Know all of the gas laws –you will need to know how to explain why your answer makes sense and how to solve for an answer algebraically. 7.Know how to calculate the partial pressures of a gas due to the different particles in a gas. 8.Explain what diffusion and effusion is and how they are different and be able to calculate the rate of effusion/diffusion. Solutions, Solids, and Liquids 1.How does the Kinetic-Molecular theory also describe the properties of liquids and its changes of state? 2.Describe the process by which liquids can change states of matter. 3.Does the ability of a liquid to diffuse change when transitions to a gas and/or solid? Explain your reasoning. 4.What are the 4 types of crystals seen in solids? Briefly describe the properties and an example of each. 5.Explain the relationship between equilibrium and changes of state. 6.Be able to interpret a phase diagram. Understand each axis, where the triple point and critical point are on any phase diagram 7.Be able to interpret and construct a heating curve 8.Distinguish between heterogeneous and heterogeneous mixtures. 9.Explain factors that affect the rate at which a solute dissolve in a solvent.
10.Explain solution equilibrium and distinguish between a saturated, supersaturated, and unsaturated solution both by description and through a solubility curve. 11.“Like dissolves like” in terms of polar and nonpolar substances.12.Compare the effects of temperature and pressure on solubility. 13.Be able to calculate…Molarity, Molality, Dilutions, Mole Fraction14.Distinguish between four colligative properties and explain why they are classified as colligative properties 15.Be able to calculate…a.Boiling-point elevation b.Osmotic pressure c.Freezing-point depression d.Vapor Pressure Lowering Kinetics 1.Describe the rate of reactant with respect to each chemical in a reaction, including analyzing its [X] vs. time graph. 2.Write the rate law and finding the value of the rate constant using initial rates data to describe how concentration of reactants affect a reaction’s rate.3.Determine the order (0, 1st, and 2nd orders only) of a reactant by analyzing the [X] vs. time, ln[X] vs time, and 1/[X] vs. time graphs. 4.Explain how the concentration of a reactant affects (or does not affect for 1st order reactions) its half-life. 5.Calculate the reaction’s half-life. 6.List factors that affect how fast a reaction occurs using collision theory. 7.Explain how changing the temperature or adding a catalyst/inhibitor affects the rate of reaction, using potential energy graph. Equilibrium 1.Describe the reaction mixture of a system at equilibrium qualitatively, graphically, and quantitatively. 2.Given concentrations of substances in a system, explain whether the reaction will shift (to the left or right) using Le Châtelier’s Principle and comparing Q vs. Keq.3.Determine the concentrations of substances at equilibrium using an ICE Chart. 4.Write and find the value for the equilibrium expression when the balanced equation is changed or when equations are combined. Types of Acids and Bases 1.Identify strong acids and strong bases. 2.Recall the behavior of indicators (i.e. universal indicator, litmus, phenolphthalein, and cabbage juice) to determine whether a solution is acidic or basic. 3.Define an acid or base using the Arrhenius or Bronsted-Lowry definitions. 4.Identify the acids, bases, conjugate acids, and conjugate bases in Bronsted-Lowry acid-base reaction 5.Calculate the pH, pOH, [H+], and [OH−] of a solution and determine whether it’s acidic or basic. 6.Identify whether a substance is an acid or base or neither. 7.Write the dissociation equations for monoprotic or polyprotic acid.
Acid/Base Solutions and Strength of Acids/Bases 1.Describe a strong acid or strong base solution. 2.Describe a weak acid or weak base solution using its Kaor Kb. 3.Find the Kbof a conjugate base given the Ka of a weak acid and vice versa. 4.Describe an acidic or basic salt dissolved in solution. 5.Describe a solution with a weak acid and its conjugate base 6.Describe with pH and concentration of all species in a particulate drawing. 7.Compare the strength of acids by comparing Kaor Kbvalues. 8.Determine whether a salt is acidic or basic using Ka and Kbvalues. 9.Compare the strength of acids by looking at its molecular structure. Acid-Base Titrations 1.Describe the solution at each point of a titration experiment (i.e. WA, WB, polyprotic acid). 2.Calculate the amount of titrant needed to reach the halfway and equivalence points and the pH at those points. 3.Calculate the concentration of an unknown acid in a titration experiment Organic Chemistry 1.Describe how carbons and hydrogens bond to form organic compounds. 2.Name and write the structural formulas for branched and unbranched alkanes, alkenes, and alkynes. 3.Name and write the structural formulas for substituted alkanes, alkenes, and alkynes. 4.Identify the degree of saturation of a hydrocarbon given the molecular formula. 5.List and identify common oxygen-containing functional groups (alcohol/ether, aldehyde/ketone, carboxylic acid/ester) 6.Write the formulas of an organic compound with an oxygen-containing functional group given the name.
Practice Problems Gases 1.Gas in a container has a pressure of 450 kPa at 200 K and a volume of 65 L, when the conditions are changed to STP, what is the volume? 2.There are 50g of Carbon dioxide produced as a result of the combustion of pentane (C5H12), what is the starting volume of pentane if the temperature is 26 °C, and the pressure is 820 Torr? 3.The starting initial temperature of a gas is 22 °C, occupying a volume of 500mL, what is the volume as a results of a 25 degree increase in temperature? 4.As the amount (mass) of gas is added to a container with a fixed volume, the pressure in the container will ___________. This is a _______________ relationship. 5.As the volume of the container decreases (constant mass, constant temp.), the pressure _______________. This a _______________ relationship. 6.As the pressure of the container decreases (constant mass, constant temp.), the volume _______________. This a _______________ relationship. 7.As the temperature of a closed bottle increases, the pressure inside the bottle _____________. This is a _______________ relationship. 8.Pressure results from the _________________ of particles with the ___________ of the container. 9.If you have the same massof gas, but reduce the volume, what happens to the pressure? ____________________________________________________________s 10.Using Boyle’s law for pressure, what happens to a volumeof gas with an increasein pressure? _____________________________________________________________ 11.In a closed container, what would happen to the pressureif the container were heated?__________________________________________________________ 12.Describes Charles law for the effect of volumeas it is heated or cooled? 13._________________________________________________________________ 14.Does kinetic energy increase or decrease with an increase in heat? ___________________ 15.Cooling a substance (slows/accelerates) the particles and (decreases/increases) the kinetic energy. 16.If you apply heat to a solid, the particles vibrate (faster/slower) 17.Going directly from solid to gas is called ___________________ 18.Temperature at which a solid turns to a liquid: _______________________point 19.The temperature at which molecular activity stops: _______________________
Solutions, Liquids and Solids 1.Most substances are _________dense in the solid phase rather than the liquid phase 2.Particles escape to the vapor phase when ____________ energy is high forcing the __________________ forces to weaken. 3.________________ crystals are made of metallic cations surround by electrons. 4.Of the covalent solids the particles in covalent _____________ solids are more organized. 5.Amorphous solids have the ____________ amount of particle arrangement. 6.A phase change is dependent on both ______________ and ________________ 7.A substance with a high vapor pressure at a low temperature would be described as having a _________________ boiling point. 8.A system is at __________________ when opposing changes occur at equal rates. 9.In a liquid- vapor system an increase in temperature would favor ___________________ 10.In a liquid vapor system an increase in pressure would favor ____________________ 11.In a liquid vapor system if more liquid is added the system would move towards the ___________________ 12.The heat of vaporization of water is considered to be high because of the __________________forces. 13.The molar heat of fusion of water is 6.009 kJ/mole, how much energy is needed to melt 50grams of ice? 14.A energy source can supply 1000kJ of energy, how many grams of water can the source vaporize? (the molar heat of vaporization of water is 40.79kJ/mole) 15.The following points are found on a phase diagram describe each point; the triple point, the critical point, normal boiling point, and critical temperature. 16.The ________________ is the substance dissolved in a solution, and the __________________ is the substance that does not change phase when forming a solution. 17.A ________________ is a specific type of homogenous mixture 18.A mixture that separates into distinct phases over time is a ________________________ 19.A _____________ is mixture that can be identified using the Tyndall effect. 20.A solubility curve demonstrates the amount of ______________ dissolved in a given amount of ______________ at specific __________________. 21.__________________ solutions occur when the maximum amount of solute has dissolved in a given amount of solvent at a specified temperature. 22.___________________ solutions occur when more solute can dissolve in a given amount of solvent at a specified temperature. 23.___________________ solutions is an unstable mixture that occurs when more solute has dissolved that typically possible. 24.Solid solutes solubility ___________________ with temperature
25.Gas solutes solubility _____________________ with temperature 26.In order for a substance to dissolve the __________ _____________ attractions must overcome the solute-solute attractions. 27.Colligative properties are physical properties that change as a result of a change in _______________________ 28.The four colligative properties are 29.Molarity is described as moles of solute divided by ____________________________ 30.Molality is describe as moles of solute dived by _______________________________ 31.A precipitate is the ________________ product in a double replacement reaction. 32.Predict the products including states of matter when aqueous barium chloride reacts with a sulfuric acid solution. 33.Calculate the molarity of a solution made with 60g of sodium hydroxide dissolved in 450mL of water. 34.How many grams of calcium hydroxide are needed to make 300g of a 0.25m solution? 35.Iron (III) chloride can be produced by reacting Fe2O3 with hydrochloric acid solution. How many milliliters of 6.0M HCl are needed to react with excess Fe2O3to produce 16.5g of FeCl3
Kinetics and Equilibrium 1.Consider the equilibrium: 2 NO (g) + O2(g) ⇌2 NO2(g). a.White the equilibrium expression and calculate its value at this temperature if at 100 C, the equilibrium concentrations for this system are: [NO] = 0.50 M [O2] = 0.20 M [NO2] = 0.10 M 2.Consider the equilibrium: 2 SO2(g) + O2(g) ⇌2 SO3(g). a.What changes can be made so the equilibrium system can be shifted to the right? i.[ Add | Remove ] SO2ii.[ Add | Remove ] O2iii.[ Add | Remove ] SO3iv.[ Add | Remove ] Volume b.When the temperature is raised, the equilibrium system shifts to the left. Is this reaction endothermic or exothermic? 3.Which of the labeled distances in the image below corresponds to the activation energy for the reaction of X to Y? 4.Which point/points remain unchanged if a catalyst is added to the reaction? 5.Consider the following reaction: 2 NO (g) + O2(g) →2 NO2(g) The following kinetics data were collected: a)Find the rate law for this reaction. b)Find the value of the rate constant, k. Include units Trial [NO] [O2] Rate 1 0.10 M 0.10 M 5.0 M/s 2 0.20 M 0.10 M 10.0 M/s 3 0.40 M 0.20 M 20.0 M/s
Acids and Bases 1.Arrhenius acids produce __________ 2.Bronsted Lowry Bases _____________ hydroxide 3.Make a list of characteristics common to acids and common to bases 4.A strong acid is a __________ electrolyte because it ___________ completely in water 5.When naming a binary acid the prefix is _____________ 6.Oxyacid acids with the suffix “ous” produce an anion with the suffix ___________. 7.Identify each of the following as being acidic, basic, or neutral solutions at 25 C a.[H3O+] = 1.0 x 10-7M b.[OH-] = 1.0 x 10-11M c.pH = 3.0 d.pH = 13.0 8.Name each of the following acids or bases a.HBr b.HNO3c.H2SO3d.HClO3e.NaOH f.Ba(OH)29.Write the formula for each of the following acids a.Hydrofluoric Acid b.Phosphoric Acid c.Hypochlorous acid 10.Write the first and second ionization of carbonic acid. 11.A conjugate acid has __________ hydrogen atoms than its bases 12.A conjugate base has ___________hydrogen atoms than its acid 13.The products of neutralization are ___________ and ______________ 14.Write the neutralization reaction between barium hydroxide and phosphoric acid 15.The pH describes the percent ________________ in a solution 16.Indicators are ___________ specific 17.Calculate the [OH-1] of solution with a 0.002M [H3O+] 18.Calculate the pH of a Ca(OH)2with a concentration of 0.15M 19.Find the hydroxide concentration of a solution with a pH of 3.7 20.A titration is uses a solution of a _____________ concentration to find the _________________ of another solution with a specific volume. 21.Describe what a titration curve demonstrates. 22.Determine the concentration of 20.0 mL of carbonic acid are titrated with 17.2mL of 0.14M potassium hydroxide. 23.Suppose that 15.0 mL of 2.50 x 10-2M H2SO4is required to neutralize 10.0 mL of a KOH solution. What is molarity of the KOH solution? 24.The pH of a sample of human blood was measured to be 7.41 at 25 °C. Calculate the pOH, [H+], and [OH-1] of the sample
25.A student has an unknown solution, labeled as A, and must determine if it is a strong acid or base. He starts by using a pH meter to determine the initial pH of solution A. He finds that solution A has a pH of 10.08 and decides to titrate 50.0 mL of solution A against a standard 0.15 M HCl solution. He records the pH of the sample as he titrates in the table below: a.Sketch a titration curve (Volume vs. pH) using the graph paper provided. b.Using the titration curve, find the equivalence point for the titration. Clearly make and label the equivalence point on the titration curve. c.Calculate the molarity of unknown solution A. 26.Consider a 0.20 M HC2H3O2 solution. Find the concentration of all species, the pH and pOH, and the percent ionization. The Kafor HC2H3O2is 1.8 x 10-5Titration of Unknown Solution A Volume of 0.15 M HCl added (mL) pH 0 10.98 5 10.00 10 9.86 15 9.60 20 9.43 25 9.26 30 8.90 35 8.75 40 8.65 45 8.25 50 5.37 55 4.05 60 2.20 65 2.05 70 1.93
Organic Chemistry1.Hydrocarbons are composed of ____________________ and ____________ ____ 2.Alkanes are said to be saturated because the carbon atom is bonded to four ____________________ atoms. 3.An alkene compound has at least one __________________ bond. 4.When naming a branched alkane the alkyl groups are placed in ___________________ order. 5.When naming a branched alkene the ________________ takes precedence when assigning the carbon number. 6.A 4 carbon alkane that has formed a ring would be named ____________________ 7.An alcohol is identified by the ____________ attached to a carbon chain. 8.When fluorine, chlorine, bromine, or iodine is attached to a carbon chain it is considered to be an alkyl ___________________ 9.A carbon double bonded to an oxygen in the middle of a carbon chain is a _______________ 10.An ether forms when two alkyls are connected by a _____________ atom. 11.Aldehydes from when double bond forms between carbon an oxygen at the ____________ of a carbon chain. 12.When carboxylic acid attaches to a(n) _____________ an ester is formed. 13.The identifying element of an amine is ____________________. 14.If a hydroxide attaches to propane the name is ____________________. 15.The prefix of an alkyl halide formed when bromine attaches to an alkane is _____________________. 16.The “al” ending identifies a(n) ________________ group. 17.A pentane has a double bond to oxygen on the third carbon the name is _______________________ 18.A 4 carbon alkane is attached to an oxygen that is attached to a 3 carbon alkane, the name would be _____________________________ 19.__________________________ is the name of a 6-carbon carboxylic acid 20.The name of a molecule made when propanoic acid is attached to a 2-carbon alkane is _________________________. 21.A nitrogen is attached to 2 different 2 carbon molecules it’s name is ________________________________________