A P Chemistry Practice Test Ch 17 Electochemistry A-Books Pdf

A P Chemistry Practice Test Ch 17 Electochemistry A
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9 What is the coefficient of the bromide ion when the following redox equation is balanced. BrO Fe OH 2 Br Fe OH 3 basic solution, A 4 B 3 C 2 D 1 E 5. 10 What is the coefficient of Fe3 when the following equation is balanced. CN Fe3 CNO Fe2 basic solution, A 1 B 2 C 3 D 4 E 5. 11 The balanced half reaction in which sulfate ion is reduced to sulfite ion is a process. A three electron, B four electron, C two electron, D one electron. E six electron, 12 The half reaction occurring at the anode in the balanced reaction shown below is. 3MnO4 aq 24H aq 5Fe s 3Mn2 aq 5Fe3 aq 12H2O l, A Fe2 aq Fe3 aq e.
B MnO4 aq 8H aq 5e Mn2 aq 4H2O l, C Fe s Fe3 aq 3e. D 2MnO4 aq 12H aq 6e 2Mn2 aq 3H2O l, E Fe s Fe2 aq 2e. 13 The purpose of the salt bridge in an electrochemical cell is to. A provide a source of ions to react at the anode and cathode. B provide oxygen to facilitate oxidation at the anode. C provide a means for electrons to travel from the anode to the cathode. D provide a means for electrons to travel from the cathode to the anode. E maintain electrical neutrality in the half cells via migration of ions. 14 In a voltaic cell electrons flow from the to the. A salt bride anode, B anode cathode, C anode salt bridge. D salt bridge cathode, E cathode anode, A 96485 C B 1 J C C 1 C J D 1 J s E 1 amp s. Table 20 1, Half Reaction Ee V, F2 g 2e 2F aq 2 87.
Cl2 g 2e 2Cl aq 1 359, Br2 l 2e 2Br aq 1 065, O2 g 4H aq 4e 2H2O l 1 23. Ag e Ag s 0 799, Fe aq e Fe aq 0 771, I2 s 2e 2I aq 0 536. Cu2 2e Cu s 0 34, 2H 2e H2 g 0, Pb2 2e Pb s 0 126, Ni2 2e Ni s 0 28. Li e Li s 3 05, 16 Which of the halogens in Table 20 1 is the strongest oxidizing agent. E All of the halogens have equal strength as oxidizing agents. 17 Which one of the following types of elements is most likely to be a good oxidizing agent. A transition elements, B alkaline earth elements, C lanthanides.
D alkali metals, E halogens, Table 20 1, Half Reaction Ee V. F2 g 2e 2F aq 2 87, Cl2 g 2e 2Cl aq 1 359, Br2 l 2e 2Br aq 1 065. O2 g 4H aq 4e 2H2O l 1 23, Ag e Ag s 0 799, Fe aq e Fe aq 0 771. I2 s 2e 2I aq 0 536, Cu2 2e Cu s 0 34, 2H 2e H2 g 0. Pb2 2e Pb s 0 126, Ni2 2e Ni s 0 28, Li e Li s 3 05.
18 Using Table 20 1 which substance can be oxidized by O2 g in acidic aqueous solution. A Ni 2 aq B Br2 l C Ag s D Cu2 aq E Br aq, Table 20 2. Half reaction Ee V, Cr3 aq 3e Cr s 0 74, Fe2 aq 2e Fe s 0 440. Fe3 aq e Fe2 s 0 771, Sn4 aq 2e Sn2 aq 0 154, 19 The standard cell potential Ee cell for the voltaic cell based on the reaction below is V. Sn2 aq 2Fe3 aq 2Fe2 aq Sn4 aq, A 1 39 B 0 46 C 0 617 D 1 21 E 0 46. 20 The standard cell potential Ee cell for the voltaic cell based on the reaction below is V. 3Sn4 aq 2Cr s 2Cr3 aq 3Sn2 aq, A 0 89 B 1 94 C 0 59 D 2 53 E 1 02.
21 The relationship between the change in Gibbs free energy and the emf of an electrochemical cell is given by. A DG B DG nRTF C DG D DG E DG nFE, Table 20 2, Half reaction Ee V. Cr3 aq 3e Cr s 0 74, Fe2 aq 2e Fe s 0 440, Fe3 aq e Fe2 s 0 771. Sn4 aq 2e Sn2 aq 0 154, 22 Which of the following reactions will occur spontaneously as written. A Sn4 aq Fe2 aq Sn2 aq Fe s, B 3Sn4 aq 2Cr s 2Cr3 aq 3Sn2 aq. C 3Fe s 2Cr3 aq 2Cr s 3Fe2 aq, D Sn4 aq Fe3 aq Sn2 aq Fe2 aq.
E 3Fe2 aq Fe s 2Fe3 aq, 23 The standard cell potential Ee cell for the reaction below is 0 63 V The cell potential for this reaction is. V when Zn2 1 0 M and Pb2 2 0 10 4 M, Pb2 aq Zn s Zn2 aq Pb s. A 0 74 B 0 52 C 0 63 D 0 85 E 0 41, 24 Consider an electrochemical cell based on the reaction. 2H aq Sn s Sn2 aq H2 g, Which of the following actions would change the measured cell potential. A lowering the pH in the cathode compartment, B increasing the pressure of hydrogen gas in the cathode compartment.
C increasing the Sn2 in the anode compartment, D increasing the pH in the cathode compartment. E Any of the above will change the measure cell potential. 25 One of the differences between a voltaic cell and an electrolytic cell is that in an electrolytic cell. A electrons flow toward the anode, B a nonspontaneous reaction is forced to occur. C an electric current is produced by a chemical reaction. D O2 gas is produced at the cathode, E oxidation occurs at the cathode. 26 How many minutes will it take to plate out 2 19 g of chromium metal from a solution of Cr3 using a current of. 35 2 amps in an electrolyte cell, A 1 92 B 5 77 C 346 D 115 E 17 3. 27 How many grams of Ca metal are produced by the electrolysis of molten CaBr2 using a current of 30 0 amp for. 10 0 hours, A 112 B 448 C 0 0622 D 224 E 22 4, 28 How many grams of copper will be plated out by a current of 2 3 A applied for 25 minutes to a 0 50 M solution.
of copper II sulfate, A 0 019 B 1 1 C 0 036 D 2 2 E 1 8 x 10 2. 29 A voltaic cell is constructed with two silver silver chloride electrodes where the half reaction is. AgCl s e Ag s Cl aq Ee 0 222 V, The concentrations of chloride ion in the two compartments are 0 0222 M and 2 22 M respectively The cell emf. A 0 00222 B 0 232 C 0 118 D 0 212 E 22 2, 30 How many seconds are required to produce 4 00 g of aluminum metal from the electrolysis of molten AlCl3. with an electrical current of 12 0 A, A 2 90 105 B 3 57 103 C 27 0 D 9 00 E 1 19 103. Advanced Placement Chemistry 1996 Free Response Questions. 7 Sr s Mg2 Sr2 Mg s, Consider the reaction represented above that occurs at 25 C All reactants and products are in their standard states.
The value of the equilibrium constant Keq for the reaction is 4 2 x 1017 at 25 C. a Predict the sign of the standard cell potential E for a cell based on the reaction Explain your prediction. b Identify the oxidizing agent for the spontaneous reaction. c If the reaction were carried out at 60 C instead of 25 C how would the cell potential change Justify your. d How would the cell potential change if the reaction were carried out at 25 C with a 1 0 molar solution of. Mg NO3 2 and a 0 10 molar solution of Sr NO3 2 Explain. e When the cell reaction in d reaches equilibrium what is the cell potential. Advanced Placement Chemistry 1996 Free Response Answers. Question 1 is question 4 in previous years question 2 is question 1 in previous years and questions 3 4 are. questions 2 3 in previous years, students are now allowed 10 minutes to answer question 1 after which they must seal that portion of the. delta is used to indicate the capital Greek letter. square root applies to the numbers enclosed in parenthesis immediately following. All simplifying assumptions are justified within 5. One point deduction for a significant figure or math error applied only once per problem. No credit earned for numerical answer without justification. a two points, The sign of the cell potential will be positive. because any one is sufficient, K is greater than 1. the reaction is spontaneous occurs, E for Sr2 is more positive. Standard reduction potential for Sr more negative, Note only 1 point earned for just E positive because Keq positive.
b one point, The oxidizing agent is Mg2, c two point. The cell potential would increase, Since all ions are at 1 M Q for the system is 1 and E RT nF ln K. so as T increases so should E, Note no credit lost if student recognizes Keq dependence on T For temperature change in this problem decrease in. ln K term is small relative to the term RT nF, No change because in the Nernst equation Ecell E RT nF ln Q. ln Q 0 and Ecell E, Note this second approach earns 1 point only.
d two points, Ecell will increase, In the equation Ecell E 0 0592 n log Q. Q 0 1 therefore log Q is negative therefore term after E is positive therefore Ecell increases. with the concentration of Mg2 larger than that of Sr2 Le Chatelier s principle predicts the reaction will have a. larger driving force to the right and a more positive Ecell. e one point, At equilibrium Ecell 0, Note balanced neutral or no net reaction not accepted. Answer Key, Testname CH 17 PRAC TEST ELECTROCHEMISTRY TST. MULTIPLE CHOICE Choose the one alternative that best completes the statement or answers the question. ID chem9b 20 1 1, ID chem9b 20 1 2, ID chem9b 20 1 3. ID chem9b 20 1 5, ID chem9b 20 1 9, ID chem9b 20 1 10.
ID chem9b 20 1 11, ID chem9b 20 1 12, ID chem9b 20 1 15. ID chem9b 20 1 19, ID chem9b 20 1 23, ID chem9b 20 1 25. ID chem9b 20 1 27, ID chem9b 20 1 28, ID chem9b 20 1 32. ID chem9b 20 1 33, ID chem9b 20 1 35, ID chem9b 20 1 37. ID chem9b 20 1 40, ID chem9b 20 1 44, ID chem9b 20 1 45.
Answer Key, Testname CH 17 PRAC TEST ELECTROCHEMISTRY TST. ID chem9b 20 1 47, ID chem9b 20 1 49, ID chem9b 20 1 51. ID chem9b 20 1 59, ID chem9b 20 1 60, ID chem9b 20 1 62. ID chem9b 20 1 65, ID chem9b 20 2 2, ID chem9b 20 2 10. A P Chemistry Practice Test Ch 17 Electochemistry MULTIPLE CHOICE Choose the one alternative that best completes the statement or answers the question

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