AP chemistry
|Concepts |Details |
|Empirical Formula & |Definition |
|Molecular Formula | |
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| |How is empirical formula calculated? |
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| |How is molecular formula calculated? |
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|Ionic vs Covalent |Formula differences? |
|compounds | |
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| |Chemical differences? |
| |Boiling points |
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| |Melting points |
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| |Conductivity |
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| |How does number of ions affect conductivity? |
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|Density |Definition: |
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| |Changes with changes in ___________________ |
|Lattice Energy in |Definition: |
|ionic compounds | |
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| |Coulombs Law: |
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| |Relationships: |
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|Bond Energy in |Compare single – double – triple bond strength. |
|Covalent Compounds | |
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| |How does this relate to bond length? |
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| |How can (H be calculated for a reaction using bond energies? |
|Molarity | |
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| |What is Molarity? |
| |What will the final concentration KNO3 when 400 mL of 1.8 M Ba(NO3)2 solution reacts with 300 mL of a 1.2 M K2SO4 solution? |
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|Gases |What variable affects: |
| |Molecular speed |
| |Density |
| |Effusion |
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| |What is partial pressure? |
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| |STP? When should it be used? |
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| |What is your go to equation for gases? |
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|Electron |Write a sample electron configuration for the following: |
|Configurations |A noble gas |
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| |A transition metal |
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| |A chemically unreactive element |
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| |An element with 1 valence electron in the p block |
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| |An element with an electron in an excited state. |
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| |A halogen |
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| |Two unpaired electrons |
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| |How are valence electrons identified in an electron configuration? |
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|Periodic Trends |All periodic trends are best explained by atomic radius, quantum levels, the effective nuclear charge of the nucleus and the shielding of the|
| |core electrons. |
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| |Use these principles to explain: |
| |The difference between 1st ionization energy for Potassium and Rubidium |
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| |The difference between 1st and 2nd ionization energy in sodium. |
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| |The difference in electron affinity between Bromine and Iodine. |
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| |When looking at sequential ionization energies for Aluminum (1st, 2nd, 3rd, etc.) Where would you expect to see a large increase? Why? |
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|Molecular Shapes |Molecular shapes are relevant for ______________ bonded molecules. |
| |Examples: |
| |Lewis Dot structures are key to determining molecular shapes. |
| |After a Lewis dot structure is determined, the shape of the molecule can be determined. |
| |Polarity can also be determined by: |
| Look at VSEPR Shapes handout |
|Practice – For each of |CH4 |
|the following molecules | |
|determine | |
|Lewis Dot structure |BF3 |
|Shape | |
|Polarity |TeF6 |
|Hybridization | |
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| |KrF4 |
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| |SO2 |
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| |IF3 |
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| |SeF6 |
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| |AsF5 |
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| |KrF2 |
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| |NH3 |
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|Multiple bonds |Sigma bond |
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| |Pi bond |
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| |Single |
| |Double |
| |Triple |
|Intermolecular Forces |Ionic Bonds |
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| |Hydrogen bonding |
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| |Dipole dipole attractions |
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| |London dispersion |
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|Physical properties due |Rank the intermolecular forces in terms of strength. |
|to intermolecular | |
|Forces |How do IMF’s affect the boiling point of a liquid? |
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| |How do IMF’s affect the melting point of a liquid? |
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| |How do IMF’s affect the vapor pressure of a liquid? |
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| |What is (Hvap of a chemical? How will this be affected by IMF’s? |
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|Solutions |Mole Fraction |
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| |Solubility – what does “like dissolves like” mean |
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| |Compare the boiling point of a solution to the boiling point of a pure solvent. Name the principle. |
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| |Compare the freezing point of a solution to the freezing point of a pure solvent. Name the principle. |
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| |Compare the vapor pressure of a solution to the vapor pressure of a pure solvent. |
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| |Van’t Hoff factor (i) How many particles are in the following |
| |C6H12O6 |
| |NaCl |
| |AlCl3 |
| |C2H5OH |
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| |How does this affect freezing point, boiling point and vapor pressure of a solution? |
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|Kinetics |Kinetics involves the study of: |
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| |Reaction rate is determined by (____/(____ |
| |What is the generic form for rate law? |
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| |Rate = |
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| |Rate law must be determined_______________. |
| |For the following orders of reactions, indicate what doubling the concentration does to the reaction rate. |
| |0 order reactant |
| |1st order reactant |
| |2nd order reactant |
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| |Differential rate law: |
| |[pic] |
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| |Integrated Rate Law: |
| |Draw the graphs of straight lines for 0, 1st and 2nd order reactants, write the equations to go with each graph. |
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|Reaction Mechanism |What is a reaction mechanism? |
| |How can you tell if a chemical is a catalyst? |
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| |How can you tell if a chemical is an intermediate? |
| |What are the two criteria that must be met to determine if a reaction mechanism acceptable? |
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| |How is a catalyst identified? |
| |How in an intermediate identified? |
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| |The proposed mechanism for the reaction in this question is shown below: |
| |Step 1: 2NO (g)--> N2O2 (g) (fast) |
| |Step 2: N2O2 (g) + H2 (g) --> H2O2 (g) + N2 (g) (slow) |
| |Step 3: H2 (g) + H2O2 (g) --> 2H2O (fast) |
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| |A) Write the balanced equation for this reaction. |
| |B) Identify the rate-determining step. |
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| |C) Write a rate law that is most consistent with this mechanism |
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| |What is activation energy? |
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| |Draw an energy profile for an exothermic rxn |
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| |Draw an energy profile for an endothermic rxn. |
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| |Show how a catalyst changes activation energy on each graph. |
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|Equilibrium |Kc – |
| |Kp – |
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| |Properties of equilibrium- |
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| |What goes in the equilibrium expression? |
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| |What does the equilibrium expression tell you? |
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| |At a particular temperature K = 3.75 for the reaction: |
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| |SO2(g) + NO2(g)(( SO3(g) + NO(g) |
| |All four gases had an initial concentration of 0.800 M, calculate the equilibrium concentrations of the gases. |
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| |At a particular temperature, 12.0 mol of SO3 is placed into a 3.0-L rigid container, and the SO3 dissociates by the reaction: |
| |2SO3 (g) (( 2SO2 (g) + O2 (g) |
| |At equilibrium, 3.0 mol of SO2 is present. Calculate K for this reaction |
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|LeChatelier’s Principle |Definintion: |
| |How do the following affect equilibrium? |
| |aq or gas added/removed? |
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| |Solid added/removed? |
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| |Unreactive gas added/ removed? |
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| |The volume of a container is increased/decreased? |
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| |Temperature is increased for an endothermic reaction? Exothermic reaction? How is K changed? |
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| |Temperature is decreased for an endothermic reaction? Exothermic reaction? How is K changed? |
|Acids and Bases |Strong Acids: |
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| |Strong bases: |
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| |Examples of weak acids: |
| |Examples of weak bases: |
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| |How is pH calculated? |
| |pOH? |
| |[H+] From pH |
| |[OH-] from pOH |
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| |What is Kw? |
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| |Is the [H+] concentration 0 for a base? |
| |Why or why not? |
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| |Strong acids _______________________. |
|Calculating the pH of |pH is calculate by using _________________ |
|strong acids | |
| |For the following acids, calculate pH |
| |.004 M HCl |
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| |.05 HNO3 |
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| |1.0 x 10-8 M HBr |
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| |Strong bases _______________________. |
|Calculating the pH of |pH is calculate by using _________________ |
|strong bases | |
| |For the following bases, calculate pH |
| |.015 M NaOH |
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| |.05 Ca(OH)2 |
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| |1.0 x 10-8 M KOH |
| |Weak acids do not _______________________ |
| |What is the acid dissociation constant? What does it tell you about an acid? |
| |What is the pH of a 0.15 M solution of HC2H3O2? Ka=1.8 x 10-5 |
|Calculating the pH of | |
|weak acids | |
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| |What concentration of HCN would you need to create a pH of 4.25? (Ka = 6.2 x 10-10) |
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| |How do weak bases form hydroxide? |
| |What is the base dissociation constant? What does it tell you about a base? |
| |What is the pH of a 0.75 M solution of NH3? Kb=1.8 x 10-5 |
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| |Kb, the base dissociation constant, for a base is 9.4 x 10-4 at room temperature. At this temperature, what is the approximate percent |
|Calculating the pH of |dissociation of the base in a 1.0 M solution? |
|weak bases | |
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| |A weak acids conjugate base will produce a basic salt. |
| |A weak bases conjugate acid will produce an acidic salt. |
| |__________________ is used to find Ka or Kb. |
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| |Identify the following salts as acidic, or neutral. For each salt, calculate the pH of the solution. |
| |.600 M NH4Cl Kb for NH3 = 1.8 x 10-5 |
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|Acid/Base properties of | |
|salts | |
| |1.2 M KNO3 |
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| |.98 M NaC2H3O2 Ka for HC2H3O2 =1.8 x 10-5 |
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| |What is a buffer? |
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| |Give two examples of acidic buffer systems. |
|Buffer solutions | |
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| |Give two examples of basic buffer systems. |
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| |What is the pH of an aqueous solution containing 0.20M acetic acid and 0.10M sodium acetate? |
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| |Ksp – |
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| |Molar solubility – |
|Solubility Product | |
|(Ksp) |What information does Ksp give you? |
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| |What information does molar solubility give you? |
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| |Given Ksp ___________________ can be found |
| |Given molar solubility _______________can be found |
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| |Several reactions are carried out using AgBr, a cream colored silver salt for which the value of the solubility-product constant, |
| |Ksp, is 5.0 x 10-13 at 298K. |
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| |Write the expression for the solubility–product constant, Ksp, of AgBr. |
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| |Calculate the value of [Ag+] in 50.0 mL of a saturated solution of AgBr at 298K. |
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| |A 50.0 mL sample of distilled water is added to the solution described in the bullet above, which is in a beaker with some solid AgBr at |
| |the bottom. The solution is stirred and equilibrium is reestablished. Some solid AgBr remains in the beaker. Is the value of [Ag+] |
| |greater than, less than or equal to the value you calculated in the part above? Justify your answer. |
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| |Calculate the minimum volume of distilled water, in liters, necessary to completely dissolve a 5.0 g sample of AgBr(s) at 298 K. (The |
| |molar mass of AgBr is 188g/mol.) |
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| |A student mixes 10.0 mL of 1.5 x 10-4 M AgNO3 with 2.0 mL of 5.0 s 10-4 M NaBr and stirs the resulting mixture. What will the student |
| |observe? Justify your answer with calculations. |
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| |The color of another salt of silver, AgI(s), is yellow. A student adds a solution of NaI to a test tube containing a small amount of |
| |solid, cream colored AgBr. After stirring the contents of the test tube, the student observes that the solid in the test tube changes |
| |color from cream to yellow. |
| |Write a chemical equation for the reaction that occurred in the test tube |
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| |Which salt has a great Ksp: AgBr or AgI. Justify your answer. |
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|Thermo- |Enthalpy (include units)– |
|dynamics | |
| |How can it be measured? |
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| |Specific heat – |
| |What is the relationship between specific heat and change in temperature? |
| |(H + means |
| |(H – means |
| |(Hf- |
| |What is the (Hf of elements? |
| |How can the standard enthalpies of formation be used to solve for (Hrxn? |
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| |(Hcomb- |
| |Find the (H for the reaction below, given the following reactions and subsequent (H values: |
| |2CO2(g) + H2O(g) --> C 2H2(g) + 5/2O2(g) |
| |C2H2(g) + 2H2(g) --> C2H6(g) (H =-94.5 kJ |
| |H2O(g) --> H2(g) + 1/2O2 (g) (H =71.2 kJ |
| |C2H6(g) + 7/2O2(g) --> 2CO2(g) + 3H2O(g) (H =-283 kJ |
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| |Entropy (include units)- |
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| |(S + means |
| |(S – means |
| |When looking at a chemical reaction what do you look at to determine if entropy is increasing or decreasing? |
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| |Free Energy (include units)- |
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| |(G + means |
| |(G – means |
| |(G 0 means |
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| |Gibbs Free energy equation and Chart |
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| |Because (G = 0 means the system is at equilibrium, |
| |______________________ can be used to fine the equilibrium constant. |
| |[pic] |
| |A student performs an experiment to determine the molar enthalpy of a solution of urea, H2NCONH2. The student places 91.95 grams of |
| |water at 25(C into a coffee-cup calorimeter and immerses a thermometer into the water. After 50 s, the students adds 5.13 grams of solid|
| |urea, also at 25(, to the water and measures the temperatures of the solution as the urea dissolves. A plot of the temperature data is |
| |shown in the graph above.. |
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| |Determine the change in temperature of thesolution that results from the |
| |Dissolution of the urea. |
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| |According to the data, is the dissolution of urea in water an endothermic process or an Exothermic process? Justify your answer. |
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| |Assume that the specific heat capacity of the calorimeter is negligible and that the specific heat capacity of the solution of urea and |
| |water is 4.2 J/g(C throughout the experiment. |
| |Calculate the heat of dissolution of the urea in joules. |
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| |Calculate the molar enthalpy of the solution, (H(soln, of urea in kJ/mol. |
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| |Using the information in the table below, calculate the value of the molar entropy of solution, (S(soln, of urea at 298 K. Include units|
| |with your answer. |
| |(H(soln urea |
| |14.0 kJ/mol |
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| |(G(soln urea |
| |-6.9 kJ/mol |
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| |The student repeats the experiment and this time obtains a result for (H(soln of urea that is 11 percent below the accepted value. |
| |Calculate the value of (H(soln that the student obtained in the second trial. |
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| |The student performs a third trial of the experiment but this time adds urea that has been taken directly from a refrigerator at 5(C. |
| |What effect, if any, would using the cold urea instead of urea at 25(C have on the experimentally obtained value of (H(soln? Justify |
| |your answer. |
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| |Electrochemistry |
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| |Oxidation – Reduction |
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| |What is Oxidation? |
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| |What is Reduction? |
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| |What are the steps for balancing half reactions? |
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| |What are standard reduction potentials? |
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| |If substance is likely to be reduced, what does that mean about it’s potential as an oxidizing agent? Where are these chemicals found on|
| |the standard reduction potential chart? |
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| |If a substance is likely to be oxidized, what does that mean about it’s potential to be a reducing agent? Where are these |
| |chemicals found on the standard reduction potential chart? |
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| |Galvanic Cell |
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| |Draw a basic galvanic cell, with all parts labeled. Show electron flow. |
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| |How is cell potential found? |
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| |What is the relationship between (G( and E(cell? |
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| |How does changing concentration from 1.0 Molar standard state affect the Cell potential? |
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| |The diagram below shows the experimental setup for a typical electrochemical cell that contains two standard half-cells. The |
| |cell operates according to the reaction represented by the following equation. |
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| |[pic] |
| |Identify M and M2+ in the diagram and specify the initial concentration for M2+ in solution. |
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| |Indicate which of the metal electrodes is the cathode. Write the balances equation for the reaction that occurs in the |
| |half-cell containing the cathode. |
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| |What would be the effect on the cell voltage if the concentration of Zn2+ was reduced to 0.100 M in the half cell containing |
| |the Zn electrode? |
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| |Describe what would happen to the cell voltage if the salt bridge was removed. Explain. |
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