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In a second experiment, the student prepares solutions of food coloring and bleach with concentrations that differ from those used in the first experiment. 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. Which species, HC6H7O2 or C6H7O2-, has a higher concentration? Half of the battle with AP Exams is knowing what to expect. (a) Explain how the graphs indicate that the reaction is second order. Draw in the species needed to accurately represent the major ionic species remaining in the solution after the reaction has been completed. 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. Would the final pressure be less than, greater than, or equal to 1.04 atm? 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. 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. Justify. (b) Calculate the rate constant, k, for the reaction at 350K. The following equation is incorrect. In a 0.0350M HF solution, the percent ionization of HF is 13.0 percent. Is the pH of the buffer represented in the diagram greater than, less than, or equal to 3.40? (b) The diagram below is incomplete. Justify that the reaction is thermodynamically favorable by calculating the value of E° for the reaction. In order to transwer for electrons with a smaller mask, Na and Ca are investigated as potential anodes. Justify you answer. I'm a junior in New Jersey. (a) Based on the student's hypothesis, what should be the formula of the compound that forms between chlorine and fluorine (b) In an attempt to verify the hypothesis, the student researches the fluoride compounds of the other halogens and finds the formula ClF3. (Do not do any numerical calculations.). 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. 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. Hello! 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? Two of them have the same length and the third is larger. (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? Save my name, email, and website in this browser for the next time I comment. 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? (c) After 20 minutes some CO2 was injected into the container, initially raising the pressure to 1.5atm. Identify the missing component of the cell, and explain its importance for obtaining a nonzero voltage (bi) Calculate the value of E for the half-reaction Cr3+ + 3e- --> Cr (bii) Write the balanced net-ionic equation for the overall reaction that occurs as the cell operates (biii) Calculate the value of delta Go for the overall cell reaction in J/molrxn, The complete photoelectron spectrum of an element is represented above (a) Identify the element (b) Calculate the value of the rate constant, k, for the radioactive decay. Justify. (d) Metal air cells need to be lightweight for many applications. Justify. Justify with calculation. Justify, (a) For trial 1, calculate the initial pressure, in atm, in the vessel at 625K. When I say a ton, I mean a TON. an ion that does not participate in the reaction. Your email address will not be published. (b) Calculate the pressure of the CO2(g) in the container at 425 K. (c) In terms of kinetic molecular theory, briefly explain why the pressure of the CO2(g) in the container changes as it is heated to 425 K. (d) The student measures the actual pressure of the CO2(g) in the container at 425 K and observes that it is less than the pressure predicted by the ideal gas law. In acidic medium: The reduction of MnO −4 ion into Mn2+ ion san be represented by the following ionic equation : 2 MnO −4 + 4H+ → Mn2+ + 2H2O + 5O or (1) What would happen if a match were struck in a room filled with oxygen? The difference in the mass of the alcohol burner before and after the combustion in this experiment is also 0.55g. Justify. 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. Justify (b) The solution is diluted with distilled water to a total volume of 1.00L. (b) Identify a compound from the table that can be dissolved in water to produce a basic solution. (f) The entropy change for the dissolution of urea, ΔS°soln , is 70.1 J/(mol⋅K) at 25°C. CaCl2(aq) + H2SO4(aq) + CaSO4(s) + 2HCl(aq). 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). The molar heat capacity of Al is 24J/molK, and the heat of fusion of Al is 10.7 kJ/mol. (c) Given that the concentration of KMnO4(aq) was 0.0235 M, calculate the number of moles of MnO4− ions that completely reacted with the H2C2O4. Justify your answer. 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. 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. Justify your answer. The student adds two drops of 3.0M HNO3 and stirs the sample, observing that the pH remains at 4.7. It looks like your browser needs an update. Justify your response. 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? Identify the type of reaction when aluminum reacts with bromine, Identify the type of reaction when copper reacts with aqueous silver nitrate, Identify the type of reaction when propane (C3H8) reacts with oxygen, Identify the type of reaction when lead (II) nitrate reacts with potassium iodide, Write the equation when aluminum reacts with bromine, Write the equation when copper reacts with aqeous silver nitrate, CU(s) + 2AgNO3(aq) --> Cu(NO3)2(aq) + 2Ag(s), Write the equation when propane (C3H8) reacts with oxygen, Write the equation when lead (II) nitrate reacts with potassium iodide, Pb(NO3)2(aq) + 2Kl(aq) --> Pbl2(s) + 2KNO3(aq), Write a balanced chemical equation when sodium iodide reacts with phosphoric acid, What type of reaction occurs when sodium iodide reacts with phosphoric acid, Write a balanced chemical equation when potassium oxide reacts with water, What type of reaction occurs when potassium oxide reacts with water, Write a balanced chemical equation when heating sulfuric acid produces water, oxygen and sulfur dioxide, What type of reaction occurs when heating sulfuric acid produces water, oxygen and sulfur dioxide, Write a balanced chemical equation when aluminum reacts with sulfuric acid, What type of reaction occurs when aluminum reacts with sulfuric acid, Write a balanced chemical equation when pentane (C5H12) reacts with oxygen, What type of reaction occurs when pentane (C5H12) reacts with oxygen. Explain why the student's claim is accurate (d) Which species, fulminic acid or isocyanic acid is present in higher concentration at equilibrium at 298K? Assume that initially all the gas present in the vessel is C4H6 (b) Use the data plotted in the graphs to determine the order of the reaction with respect to C4H6 (c) The initial rate of the reaction is 0.0010 mol/Ls calculate the rate constant k for the reaction at 625K, (a) Considering the value of K for the reaction, determine the concentration of Ba(EDTA)2- in the 100.0mL of solution. Explain your reasoning based on the student's observations (b) As the mass of the Sn electrode decreases, where does the mass go? (a) Identify a Brønsted-Lowry conjugate acid-base pair in the reaction. Unit 2: Molecular and Ionic Compound Structure and Properties (7-9%) ⚗️ Unit 3: Intermolecular Forces and Properties (18-22%) ? 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. 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). The course covers everything from quantum mechanics and atomic structure to properties of states of matter to acid-base titrations. (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? 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 … (f) The magnitude of the enthalpy change in kJ/Molrxn calculated from the results of the second experiment is the same as the result calculated in part (e)(ii). (a) Identify the species that was reduced in the titration reaction. (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. 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 …

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