Your explanation should clearly reference the types and relative strengths of the IMFs present in each substance. Justify your answer. Which species, HC6H7O2 or C6H7O2-, has a higher concentration? The ionization of HF in water is represented by the equation above. By practicing with previously released free-response questions (FRQs), you’ll be able to go into the exam knowing what it will look like and how to tackle the questions. Will the student be able to determine the mass of AgI produced to three significant figures? (h) The student claims that ΔS° for the process contributes to the thermodynamic favorability of the dissolution of urea at 25°C. For 0.2 M solution we require 0.2 moles of NaOH in 1 litre solution. Justify your answer. (c) Fe3+ ions interact more strongly with water molecules in aqueous solution than Fe2+ ions do. *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. The AP Chemistry exam covers a ton of content. (a) Determine the oxidation number of Cl in NaOCl. b 25.9 g of MgS in 861 mL of solution. (b) For a certain reaction C6H5OH to proceed at a significant rate, the phenol must be primarily in its deprotonated form, C6H5O-. Enthalpy of Reaction, Stoichiometry, Calorimetry, A student performs an experiment to determine the value of the enthalpy change for the oxidation-reduction reaction represented by the balanced equation above. 1.2 (a) NH4NO3 contains 2 N nitrogen, 4 H hydrogen, 3 O … Save my name, email, and website in this browser for the next time I comment. Circle the formula of the molecule that has the longest bond length. YOU DO NOT HAVE TO BALANCE IT. (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. including a calculation (d) Complete the electron dot diagram for C2H5OH by drawing in all of the electron pairs. The partial pressure of NO at equilibrium is 0.122 atm. They typically start with a scenario: a lab setup, a chemical reaction, etc. Balance the equation and identify its type: Pb(NO3)2(aqA) + 2NaI(aq)-->PbI2(s) + 2NaNO3(aq). (a) Based on the graphs above, what is the order of the reaction with respect to the blue food coloring? Assume that the specific heat of the reaction mixture is 3.94 J/gC and that the heat absorbed is negligable. (f) The pH of the soft drink is 3.37 after the addition of the KC6H7O2. Justify your answer in terms of Le Chatelier’s principle. Justify, (a) The images below show the buret before the titration begins and at the end point. (b) Determine the value of Ka for propanoic acid at 25 degrees Celsius. When I say a ton, I mean a TON. 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. (a) Write the net-ionic equation for the reaction between KC6H7O2 and HCl. (b) Write the rate law for the decomposition of NO2(g). Explain. 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. (b) Calculate the number of grams of Na2S2O3 needed to prepare 100.00 mL or 0.500 M Na2S2O3. Which of the two shapes is consistent with the fact that the ClF3 molecule has a dipole moment? Write a net ionic equation to show how codeine C18H21O3N behaves as a base in water.SolutionSoluti What is the pH of an aqueous solution with [H3O] 4×1013 M Solution[H3O] 4×1013 M PH log[Consider the reaction H2g I2g 2HIg. Explain how the data in the table are consistent with a first-order reaction. (d) According to the graph, what is the temperature change of the reaction mixture? 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. 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. (a) The particle-level representation of the equimolar mixture of NO and NO2 in the flask at the completion of the reaction between NO and O2 is shown below in the box on the right. 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. In the box below on the left, draw the particle-level representation of the reactant mixture of NO and O2 that would yield the product mixture shown in the box on the right. 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). H2SO4(aq) + 2NaOH(s) --> Na2SO4(aq) + 2H2O(l). Explain. I'm a streamer, intern, and content creator for Fiveable and production manager of the Homeroom podcast! (d) Based on concepts of atomic structure and periodicity, propose a modification to the student's previous hypothesis to account for the compounds that form between halogens and fluorine, Intermolecular Forces, Enthalpy of Formation. Justify, Chemical Reactions, Atomic Structure, Reaction Stoichiometry, Redox reactions and mass percent composition, Answer the following questions relating to Fe and its ions, Fe2+ and Fe3+. 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. Justify your answer in terms of the information above, Themodynamics, Applications of Thermodynamics, Molecular Structure, Lewis diagrams, formal charge, bond enthalpy, (a) Explain why the diagram on the left is the better representation for the bonding in fulminic acid. Omit solvent molecules and use arrows to show the movement of particles. ⚛️ Unit 1: Atomic Structure and Properties (7-9%) ? Unit 2: Molecular and Ionic Compound Structure and Properties (7-9%) ⚗️ Unit 3: Intermolecular Forces and Properties (18-22%) ? (c) The boiling point of Br2 is 332 K, whereas the boiling point of BrCl is 278 K. Explain this difference in boiling point in terms of all the intermolecular forces present between molecules of each substance. Explain why this is correct. Do you agree with the student’s claim? (a) Calculate the number of moles of CO2 present in the container after 20 minutes of heating (b) The student claimed that the final pressure in the container in each experiment became constant because all of the CaCO3 had decomposed. A particulate representation of a small representative portion of the buffer solution is shown below. (c) A student claims that delta S for the reaction is close to zero. When pale yellow chlorine gas is bubbled through a clear, colorless solution of sodium iodide, the solution turns brown. Predict whether the experimentally determined mass percent of I- will be greater than, less than, or equal to the amount calculated in part (e). When the solutions are combined, the student observes that the reaction mixture reaches an absorbance near zero too rapidly. (d) The student realizes that the precipitate was not completely dried and claims that as a result, the calculated Na2CO3 molarity is too low. At this temperature the initial partial pressures of N2 and O2 are 6.01 atm and 1.61 atm respectively. Is the pH of the buffer represented in the diagram greater than, less than, or equal to 3.40? 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. Each question, whether short or long, will test you on applying the material that you have learned all year. Justify. (fii) Explain how the student could use the measured value in part (f)(i) to calculate the initial concentration of CO32−(aq). In order to transwer for electrons with a smaller mask, Na and Ca are investigated as potential anodes. Which of the following indicators would be the bset choice for determining the end point of the titration? 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 … (c) Using the balanced equation for the oxidation-reduction reaction and the information in the table above, determine which reactant is the limiting reactant. (b) The reaction is known to be first order with respect to bleach. Write a balanced equation for the complete combustion of the following compound (assume that the products are carbon dioxide and water): Write a balanced chemical equation for the following decomposition reaction: Write a balanced net ionic equation for the following reaction. What is a distinguishing feature of every decomposition reaction? Justify your answer. (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? For butanoic acid the value of pKa is 4.83. Identify the reactants and products in the chemical reaction: hydrogen gas and sodium hydroxide are formed when sodium is dropped into water, Identify the reactants and products in the chemical reaction: in photosynthesis, carbon dioxide and water react to form oxygen gas and glucose.
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