What type of reaction is taking place? They typically start with a scenario: a lab setup, a chemical reaction, etc. (eii) Using the balanced equation for the redox reaction and your answer to part (c), calculate the value of the enthalpy change of the reaction in kJ/molRXN. Write the net ionic equation. (ei) Write the electron configuration for a Zn atom in the ground state (eii) From which sublevel are electrons removed when a Zn atom in the ground state is oxidized? (d) Calculate the number of moles of precipitate that is produced in the experiment (e) Calculate the mass percent of I- in the tablet (f) In another trial, the student dissolves a tablet in 55.0 mL of water instead of 50.0 mL of water. The course covers everything from quantum mechanics and atomic structure to properties of states of matter to acid-base titrations. After equilibrium has been reestablished, is the number of moles of Ba2+ present in the solution greater than, less than, or equal to the number of moles of Ba2+ present in the original solution before it was diluted? (ai) For the chemical reaction that occurs when the precipitate forms, write a balanced net ionic equation for the reaction and (ii) explain why the reaction is best represented by a net-ionic equation (b) Explain the purpose of drying and weighing the filter paper with the precipitate three times. (b)Using the data in the table above, write the balanced equation for the thermodynamically favorable reaction that will produce Br2 when the teacher combines two of the reagents. Hi, I'm Wes Winter! Circle the formula of the molecule that has the longest bond length. Write a balanced net ionic equation for the following reaction: Complete the equation and then write a net ionic equation: Write a balanced chemical equation and use the necessary symbols from Table 11.1 to describe the reaction completely: 2Fe(s) + 6HCl(aq) --> 2FeCl3 (aq) + 3H2(g). Justify your choice in terms of atomic structure. The reaction of a fixed amount of H2 and I2 is studied H2SO4(aq) + 2NaOH(s) --> Na2SO4(aq) + 2H2O(l). ⚛️ Unit 1: Atomic Structure and Properties (7-9%) ? milwaukee, wi 53211. Would the final pressure be less than, greater than, or equal to 1.04 atm? After the LiCl dissolves completely, the maximum temperature reached by the solution is 35.6C. Academia.edu is a platform for academics to share research papers. Write "no reaction" if a reaction does not occur: Pieces of sodium and magnesium are dropped into separate water-filled test tubes (A and B). The AP Chemistry exam covers a ton of content. 1. (ei) Calculate the magnitude of the heat energy in joules that is released during the reaction. In order to transwer for electrons with a smaller mask, Na and Ca are investigated as potential anodes. Justify in terms of polarity and structure. (f) The pH of the soft drink is 3.37 after the addition of the KC6H7O2. The system is allowed to reach equilibrium. (bii) Justify in terms of the equation for the overall cell reaction (ci) Will the cell potential be higher, lower, or the same as the cell potential at the lower elevation? (c) The student hypothesizes that increasing the temperature will increase the amount of N2O3 in the equilibrium mixture. (c) Determine the number of moles of Na2CO3 in the original 50.0 mL of solution. Your explanation should clearly reference the types and relative strengths of the IMFs present in each substance. The AP Chem FRQs are 50% of the exam and include 3 long questions, which are worth 10 points, and 4 short questions, each worth 4 points. (c) Using the balanced equation for the oxidation-reduction reaction and the information in the table above, determine which reactant is the limiting reactant. I'm a streamer, intern, and content creator for Fiveable and production manager of the Homeroom podcast! (d) Calculate the pressure in the container before equilibrium is established. (ai) Based on the spectrum, write the ground-state electron configuration of the element. (aii) How many grams of carbon disulfide are needed to react completely with the Cl2? (eii) Calculate the value of delta Go for the reaction. Justify your answer. A 1.0g anode of which of these metals would transfer more electrons, assuming that the anode is totally consumed during the lifetime of a cell? Would this error increase, decrease, or have no effect on the calculated acid concentration for the second trial? Justify. To ensure the best experience, please update your browser. Explain why in terms of periodic properties and Coulomb's law. Write a balanced, net-ionic reaction for the reaction between HNO3 and the chemical species in the sample that is responsible for the pH remaining at 4.7, Chemical Reactions, Applications of Thermodynamics, Stoichiometry, Intermolecular Forces, Electrochemistry, (a) Given that the metal M is in excess, calculate the number of moles of I2 that reacted (b) Calculate the molar mass of the unknown metal M (c) Propose an experimental test the student could perform that could be used to support the hypothesis. Justify, (a) For trial 1, calculate the initial pressure, in atm, in the vessel at 625K. (gi) Will the substitution of AgNO3 for Pb(NO3)2 result in the precipitation of the I- ion from solution? Justify your answer. Calculate [KC6H7O2] in the stock solution. Fiveable’s Guide to the 2020 AP Exam Updates, Molecular and Ionic Structure and Properties, Best AP Chem Quizlet Decks for Every Unit, New Online AP Chemistry Study Guide – 2020 Changes. Do you agree with the student’s claim? Draw in the species needed to accurately represent the major ionic species remaining in the solution after the reaction has been completed. Which is more resistant to changes in pH when a strong acid or a strong base is added, the buffer made by the first or second student? The AP Chemistry exam will take place on May 14th, at 2PM Eastern Time. It looks like your browser needs an update. *AP® and Advanced Placement® are registered trademarks of the College Board, which was not involved in the production of, and does not endorse, this product. (b) Calculate the wavelength, in meters, of electromagnetic radiation needed to remove an electron from the valence shell of an atom of the element. Your email address will not be published. By the time you've learned all of this, it's more than... Table of Contents ❓ Why Quizlet? Justify your answer. For butanoic acid the value of pKa is 4.83. (a) The reaction is first order. What would be observed? Explain why the representation of HF molecules in Figure 1 is more accurate than the representation in figure 2. We’ve compiled a sortable list of all AP Chemistry past prompts! CaCl2(aq) + H2SO4(aq) + CaSO4(s) + 2HCl(aq). (c) In the box below, complete a particle representation diagram that includes four water molecules with proper orientation around the Ca2+ ion. 4.1 Using Molecular Scenes to Depict an Ionic Compound in Aqueous Solution 148 4.2 Determining Amount (mol) of Ions in Solution 149 4.3 Calculating the Molarity of a Solution 150 4.4 Calculating Mass of Solute in a Given Volume of Solution 151 4.5 Determining Amount (mol) of Ions in a Solution 151 4.6 Preparing a Dilute Solution … The container is sealed and heated to 325K, at which temperature all of the CS2 has vaporized. (e) The equipment shown above is provided so that the student can determine the value of the molar heat of solution for urea. Justify your answer (d) The half-life of the reaction in trial 4 is less than the half life in trial 1. Unit 4: Chemical Reactions (7-9%) ? Write sentences that completely describe each of the chemical reactions shown in this skeleton equation: Gaseous ammonia and oxygen react in the presence of a platinum catalyst to produce nitrogen monoxide gas and water vapor, Aqeous solutions of sulfuric acid and barium chloride are mixed to produce a precipitate of barium sulfate and aqueous hydrochloric acid. (b) The reaction is known to be first order with respect to bleach. Include the net ionic equation for the reaction that occurs when the student adds the NaOH to the HNO2 (cii) Determine the volume, in mL, of 0.100M NaOH the student should add to 100 mL of 0.100M HNO2 to make a buffer solution with a pH of 3.40, justify your answer (d) A second student makes a buffer by dissolving 0.100 mol of NaNO2 in 100 mL of 1.00M HNO2. In a 0.0350M HF solution, the percent ionization of HF is 13.0 percent. Answer by drawing a circle around one of the choices below (ii) Justify your selection in terms of delta Go (e) The HCO3- ion has 3 C-O bonds. Give one reason for this stronger interaction and justify using Coulomb's Law (d) Write the balanced equation for the half-reaction for the oxidation of Fe2+ to Fe3+ (e) The student titrates a 10.0 mL sample of the Fe2+ solution. Predict whether the experimentally determined mass percent of I- will be greater than, less than, or equal to the amount calculated in part (e). Circle the one proposed modification to correct the problem and explain (c) In another experiment, a student wishes to study the oxidation of red food coloring with bleach. At this temperature the initial partial pressures of N2 and O2 are 6.01 atm and 1.61 atm respectively. (b) Determine the value of Ka for propanoic acid at 25 degrees Celsius. Explain why, in terms of activation energy. In the box below, draw a complete Lewis electron-dot diagram for a molecule of ClF3. There is vigorous bubbling in Tube A but not in Tube B. (c) Consider two possible mechanisms for the decomposition reaction. (a) Calculate the number of grams of Mg(OH)2 that is dissolved in 100mL of a saturated solution of Mg(OH)2 at 25C (b) The energy required to separate the ions in the Mg(OH)2 crystal lattice into individual Mg2+ and OH- ions, as represented in the table below, is known as the lattice energy of Mg(OH)2. (fii) Explain how the student could use the measured value in part (f)(i) to calculate the initial concentration of CO32−(aq). Calculate the magnitude of the heat absorbed by the solution during the dissolution process, assuming that the specific heat capacity of the colution is 4.18 J/gC, include units (aii) Determine the value of delta Hsoln for LiCl in kJ/molrxn (b) Write the complete electron configuration for the Na+ ion in the ground state (c) Using principles of atomic structure, explain why the Na+ ion is larger than the Li+ ion (d) Which salt, LiCl or NaCl has the greater lattice enthalpy? Prepare for the new 2020 AP Chemistry exam format with weekly lesson plans, study materials, and FRQ practice! If you walk into the exam room knowing what the exam will look like, not only can it help ease some nerves and anxiety, but it can also even help you learn content better. If they are not equal, write both (di) Identify all types of Intermolecular Forces present in HCl (ii) What can be inferred about the relative strengths of the intermolecular forces in CCl4 and HCl? Since the AP Chemistry Exam was changed drastically in 2014, there are only 6 years of available FRQs on this list, but you can find the rest on the CollegeBoard website! (b) Calculate the number of grams of Na2S2O3 needed to prepare 100.00 mL or 0.500 M Na2S2O3. (di) Is the cell potential of the nonstandard cell greater than, less than, or equal to the cell potential of the standard cell? (a) The molecular formulas of diatomic bromine, chlorine, fluorine, and iodine are written below. Account for this difference in terms of the types and strengths of IMFs present in each liquid (c) Using the table of standard enthalpies or formation below, determine whether the combustion of 2.00mol of propene releases more, less, or the same amount of energy that that 2.00 mol of vinyl chloride releases. Include units (c) If 64 atoms of the radioactive isotope are originally present in a sample, what is the expected amount of time that will pass until only one atom of the isotope remains. The student does some research and learns that the molecule has a dipole moment . (a) Determine the oxidation number of Cl in NaOCl. Write a balance chemical equation for the following combination reaction: Write a balanced chemical equation for the single-replacement reaction that takes place in aqueous solution. Required fields are marked *. Justify. (bi) Explain how the higher temperature affects the collision energies between the reactant molecules at 120C. (a) Identify the hybridization of the valence orbitals of the carbon atom in the urea molecule. Which of the following indicators would be the bset choice for determining the end point of the titration? (c) After 20 minutes some CO2 was injected into the container, initially raising the pressure to 1.5atm. Explain this result. (f) A student prepares a solution with equimolar amounts of acetic acid and sodium acetate. Justify your answer in terms of Le Chatelier’s principle. When pale yellow chlorine gas is bubbled through a clear, colorless solution of sodium iodide, the solution turns brown. Explain this observation. Mark the following true or fase and explain: (ci) The pH of a solution prepared by mixing the 50.0mL sample of 0.20M CH3CH2COOH with a 50.0mL sample of 0.20M NaOH is 7.00 (cii) If the pH of a hydrochloric acid solution must be less than the molar concentration of the propanoic acid solution (d) Calculate the molarity of the propanoic acid solution (e) The student is asked to redesign the experiment to determine the concentration of a butanoic acid solution instead of a propanoic acid solution. The net rate of formation of B, the differ- ence of its rates of formation and decomposition, is Net rate of formation of B = kr[A] k[B] dure or a concept of physics; d animated versions of gures are available, these are r When the reaction has reached equilibrium the concentrations of A and B are [A]eq and [B]eq and A … Justify your answer, (a) Calculate the magnitude of the heat energy in kJ absorbed by the water (b) Based on the experimental data, if one mole of C3H7OH is combusted, how much heat, in kJ is released? Justify your answer. Justify your answer. H2C2O4, 90.04 amu 1 mol H 2 C2 O4 2 mol KMnO 4 x = 0.0143 mol KMnO 4 90.04 g H 2 C2 O 4 5 mol H 2 C2 O4 1L 0.0143 mol x = 0.0572 L = 57.2 mL 0.250 mol ... Net ionic equation: Zn2+(aq) + CO32-(aq) → ZnCO3(s) 3 CaCl2(aq) + 2 Na3PO4(aq) → Ca3(PO4)2(s) + 6 NaCl(aq) Ionic equation: 3 Ca2+(aq) + 6 Cl-(aq) … Electrochemistry, Thermodynamic favorability, (ai) Find Eo for the reaction between Cr2O72- and H2O2 at 298K (aii) Find Eo for the reaction between Co2+ and H2O2 at 298K (bi) Which titrant should the student choose, explain your reasoning. Explain your reasoning based on the student's observations (b) As the mass of the Sn electrode decreases, where does the mass go? NaOH is a base, and bases should not be stored next to acids because reactions between these two classes of chemicals generate heat. Practice Exercises 1.1 (a) SF6 contains 1 S and 6 F atoms per molecule (b) (C2H5)2N2H2 contains 4 C, 12 H, and 2 N per molecule (c) Ca3(PO4)2 contains 3 Ca, 2 P, and 8 O atoms per formula unit (d) Co(NO3)26H2O contains 1 Co, 2 N, 12 O, and 12 H per formula unit. (bii) The graph below shows a distribuution for the collision energies of reactant molecules at 120C. Explain. Some calculators have built-in programs that require nothing more than the entry of x, and yt through the keyboard, followed by pressing the "least-square" keys. Mark the position of the half-equivalence point on the curve with an X. (Do not do any numerical calculations.). Assume that the specific heat of the reaction mixture is 3.94 J/gC and that the heat absorbed is negligable. Justify your choice based on formal charges (b) Using the Lewis electron-dot diagrams of fulminic acid and isocyanic acid shown in the boxes above and the table of average bond enthalpies below, determine the value of delta H for the reaction of HCNO to form HNCO. (c) Two possible geometric shapes for the ClF3 molecule are trigonal planar and T-shaped. Find the errors, then rewrite and balance the equation: Write balanced chemical equation for the double-replacement reactions that occur in aqueous solution: ZnS(aq) + H2SO4(aq) --> H2S(g) + ZnSO4(aq), NaOH(aq) + HNO3(aq) --> H2O(l) + NaNO3(aq), 2KF(aq) + Ca(NO3)2(aq) --> CaF2(s) + 2KNO3(aq). Your email address will not be published. How would the student need to modify the original experimental procedure to determine the order of the reaction with respect to the red food coloring? (c) In the filtrate solution, is [K+] greater than, less than, or equal to [NO3-]? The table above gives the molecular structures and boiling points for the compounds CS2 and COS. (a) In terms of the types and relative strengths of all the intermolecular forces in each compound, explain why the boiling point of CS2 is higher than that of CO2 (b) A 10.0g sample of CS2 is put in an evacuated 5.0L rigid container. The ionization of HF in water is represented by the equation above. Justify. (i) If the oxidation of the Fe in the original sample was incomplete so that some of the 7.531g of product was FeO instead of Fe2O3, would the calculated mass percent of Fe in the original sample be higher, lower, or the same as the actual mass percent of Fe? A formula is a unique identifier of a substance. Write a balanced chemical equation for the following: Write a balanced chemical equation for the decomposition reaction: Use the activity series of metals to write a balanced chemical equation for the following single-replacement reaction: Zn(s) + 2AgNO3(aq) --> Zn(NO3)2(aq) + 2Ag(s), 2AL(s) + 3H2SO4(aq) --> AL2(SO4)3(aq) + 3H2(g). (e) Which solution should the student add to I2 to reduce it to I-? (b) Identify a compound from the table that can be dissolved in water to produce a basic solution. Who knows, it might be useful on the exam even if not directly tested! Briefly describe an experiment, including the initial conditions that you would change and the data you would gather to determine whether the rate of the reaction depends on the concentration of OH-, Gas phase equilibrium, titration, acids and bases, (a) Write the expression for the equilibrium constant Kp for the forward reaction (b) A student injects N2 and O2 into a previously evacuated, rigid vessel and raises the temperature of the vessel to 2000C. Justify. Justify your answer. including a calculation (d) Complete the electron dot diagram for C2H5OH by drawing in all of the electron pairs. Explain how the data in the table are consistent with a first-order reaction. In the box below, draw a lewis electron-dot diagram (or diagrams) for the HCO3- ion that is/are consisten with the given information. Justify, (a) The images below show the buret before the titration begins and at the end point. (b) Urea has a high solubility in water, due in part to its ability to form hydrogen bonds. All of the questions aligned to the current format and content requirements of the exam and listed below. (f) The entropy change for the dissolution of urea, ΔS°soln , is 70.1 J/(mol⋅K) at 25°C. (bi) Calculate the value of the equilibrium constant, K, for the reaction at 298K (bii) If both PNO and PNO2 in the vessel are initially 1.0atm, will PN2O3 at equilibrium be equal to 1.0 atm? Using principles of atomic structure, explain why the radius of the Fe2+ ion is larger than the radius of the Fe3+ ion. (e) Write the expression for the equilibrium constant, Keq , for the decomposition of BrCl. Balance the equation and identify its type: Pb(NO3)2(aqA) + 2NaI(aq)-->PbI2(s) + 2NaNO3(aq). Explain this change in terms of the collisions between reactant particles (c) Considering that the flask gets cooler as the reaction proceeds, what drives the chemical reaction between NaHCO3 and HC2H3O2? (c) A second student performs the experiment using the same mass of water at the same initial temperature. (a) Calculate the number of moles of C2H4 (i) That are actually produced in the experiment and (ii) that would be produced if the dehydration went to completion (b) Calculate the percent yield in the experiment (c) Do the thermodynamic data for the reaction support the student's claim? What is the pressure in the container once all of the CS2 has vaporized? Write balanced net ionic equation for K2SO4aqCaI2aqCaSO4sKIaq Express your answer as a che a When 100 mL of weak acid HA was titrated with 0.09381 M NaOH 27.63 mL was required to reach the I keep getting this problem wrong..help. Justify your answer. Academia.edu is a platform for academics to share research papers. (e) What is the approximate value of the C-O-H bond angle in the ethanol molecule (f) During the dehydration experiment, C2H4 and unreacted C2H5OH passed through the tube into the water. (a) Explain how the graphs indicate that the reaction is second order. YOU DO NOT HAVE TO BALANCE IT. The molar heat capacity of Al is 24J/molK, and the heat of fusion of Al is 10.7 kJ/mol. (b) Write the rate law for the decomposition of NO2(g). Justify your answer in terms of oxidation numbers (b) The student used a 50.0 mL buret to add the KMnO4(aq) to the H2C2O4(aq) until a faint lavender color was observed in the flask, an indication that the end point of the titration had been reached. (ei) Using information from the table above, write a net ionic equation between the Sn electrode and the Cu(NO3)2 solution that would be thermodynamically favorable and justify. Justify with explanation or calculation, A student sets up a galvanic at 298K that has an electrode of Ag immersed in a 1.0M solution of Ag+ and an electrode of Cr immersed in a 1.0M solution of Cr3+, as shown above (a) The student measures the voltage of the cell shown and discovers that it is zero. (b) The diagram below is incomplete. Now how much volume of concentrated (1M) NaOH solution be taken which contains 0.2 moles of NaOH can be calculated as follows: If 1 mol is present in 1 L or 1000 mL then 0.2 mol is present … Omit solvent molecules and use arrows to show the movement of particles. and then ask you to apply concepts from chemistry to answer questions about the scenario, such as calculating equilibrium constants or temperature changes. Indicate whether you agree or disagree and why (di) Complete the Lewis dot diagram of the HNO2 molecule in the box below, including any lone pairs (dii) Based on your completed diagram, identify the hybiridzation of the nitrogen atom (ei) Determine the initial concentration of the HNO2 solution (eii) estimate the value of pKa for HNO2 (f) During the titration, after a volume of 15mL of 0.100M KOH has been added, which species, HNO2 or NO2- is present at a higher concentration? Net ionic equations, stoichiometry, acid-base equilibria, (a) Write the net ionic equation for the reaction that occurs when the solutions of Na2CO3 and Ca(NO3)2 are mixed. Solutions of sodium fluoride and dilute hydrochloric acid are mixed. (b) For a certain reaction C6H5OH to proceed at a significant rate, the phenol must be primarily in its deprotonated form, C6H5O-. Using the information in the table above, calculate the absolute molar entropy, S°, of aqueous urea (g) Using particle-level reasoning, explain why ΔS°soln is positive for the dissolution of urea in water. Each question, whether short or long, will test you on applying the material that you have learned all year. Is the pH of the buffer represented in the diagram greater than, less than, or equal to 3.40? Write a balanced equation for the following double-replacement reaction: H2C2O4(aq) + 2KOH(aq) --> K2C2O4(aq) + 2H2O(l), CdBr2(aq) + Na2S(aq) --> CdS(s) + 2NaBr(aq), Write a balanced equation for the complete combustion of butene (C4H8), Write a balanced equation for the complete combustion of propanal (C3H6O). In a second experiment, the student prepares solutions of food coloring and bleach with concentrations that differ from those used in the first experiment. Calculate the value of [Fe2+] in the solution if it takes 17.48 mL of added 0.0350M KMnO4 to reach the equivalence point of the titration. (a) Given that the spacing between polymer chains PP and PVC is similar, the beads that sink are made of which polymer? The initial and final volume readings of the solution in the buret are shown below. The product that is not ionized is given: A yellow precipitate formed with aqueous solutions of sodium sulfide and cadmium nitrate were mixed in a beaker. The difference in the mass of the alcohol burner before and after the combustion in this experiment is also 0.55g.
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