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" Name m Date 6 " Oxidation and Reduction Reactions Unit Test Study Guide 1. What are electrolytic cells? What are they used for? ) A oo tot wses Q‘&cfirfi‘ufifi(@(fi,&h cel .QMA%\O fo ’le @ nons EN\’\‘CLY\‘LG\LS X ‘{"0 GcEVr CQJA.Q/VV\_X el QJ\Q/\%«,‘) 2. What are voltaic/galvanic cells? What are they used for? B rondhet vaes a Spondaunge s (e cal va%\() nen B preducs locrciv (elacknest eroay) 3. What are some similarities and differences between electrolytic and voltaic cells? Sarwe. DL _ A ox Rad Cot VS Spndauneess y & v NGT G\SZ(‘,\'Y‘O!\S 'RO‘V\/ ‘Q’bm Arode — (adhede v Qunshs. b ('—) 7 € ('}> (D008 Plow doviards cothods V w&\oak\tr\sjfimdsabaﬂfij CBR«\\%&D cfi?s” S&i&i@b Ccf(&vcdki‘cm bgaer © 4. What is the’anode in an eleetrochermical cell? What is the cathode in and electrochemical cell? Which way do QQ\Vam'rv electrons always flow? ® T wrode \S & vnedel W oe S . W hos & (-) (oder)\ C,GICTCUMS e ccllede 5 6 weded, lowar on Aeb\e T . W hoana ) o\ Gle vonas G Hao codhvde. ana mducuk\ (D Tlecines oy Lo arode. s cothocks 5. What is the purpose of the salt bridge ina voltaic cell? o Chonog. balanu, . sl ons. af Tha groel and Qcﬂ?ncyé& .

6. Whatisan oxrdlzmg agent? What process does it undergo in chemical reaction? TﬂuL Swlostanca b@\r\g rcoLuLcQ_o‘l (H causes O\Cldufim) a. Identify the oxidizing agent in the following reaction. 0 412 +H-2H o Na + H,0 —» NaOH + H, 60X % (Ua° —= Not! +ic”> 2 red: 24+t 4 far s B.7 L P Y (mmmd 0gend- 7. What is a reducing agent? What process does it undergo in chemical reaction? 796_ Svbstancs, bur\f) ocichi zedd (causes resbvedion ) a. Identify the reducing agent in the following reaction O H-2= =t < Na + H,0 — NaOH + H, o Q\)a" — N1 +\e’> . cedt 24y —s Y0 Ne® is rcduc,ug wbavv’f

Write oxidation and reduction half reactions for the followmg processes. Be sure to label the oxidation state of each atom. 3. 10. 11. 12, o HY5Z 42 -\ 442y -z Zn + HNO3;— Zn(NOs); + NO; + H,0 oxidiation half reaction: ZV’\ ¢ —s Z)’\+L 4+ Ca— reduction half reaction: ¥5 ,._\,> (NT e s )2 o = |24l o Na + H,0— NaOH + H, oxidiation half reaction: © Q\I& sy I\fafi H&’)Z reduction half reaction: + + — G 20t t2e- — i) O oo~ g2 S Cu + 2AgNO; —» Cu(NOs;), + Ag oxidiation half reaction: © ¢ P Cu’ —3 (G reduction half reaction: il _ o) . f*g Hle- — N2 22 w32 5 ‘ 3CO + Fe,03 —» 3COZ + ZFe oxidiation half reaction: 2z oy C™ = v reduction half reaction: /‘ %3 . 1 (&1 ¥ 3e = e 2 \"W?, e MZL \ t2 .9 o2 ZKZCFZO7 + 2H,0 + 35_” 4KOH + 2Cr;,03 + 35S0, oxidiation half reaction: o T4 = QS _ 6 = L&’, > _% reduction half reaction: (GYW + Be- —> G(*3>L\

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Write oxidation and reduction half reactions for the following and use them to write a balanced equation using the redox balancing method. Also, predict if the reactions are spontaneous or non-spontaneous by analyzing each half reaction and using table J. - > - 13. H,0 —»H; + O, oxidiation half reaction: -2 20 —s O, + e~ reduction half reaction: £\ i & CZ\ 2 —> W z/) B balanced equation: e —> IR, + 0, (2] 14, Fe + Mn*—» Fe¥ + Mn = oxidiation half reaction: e Te*™ - - —de7T 5 2 reduction half reaction: M NE420 - 8 Mn balanced equation: e * va*g—_—9 fe+ L dn® O 9 432 15.°Al + 0, —> ALO; oxidiation half reaction: <A\° > M 1 Re - ) ¢ reduction half reaction: (0, e — 207\ 3 balanced equation: W~ D, — 20,0, e,

16. Construct a functioning galvanic cell using the parts provided in the diagram as well as the following materials. ’ --Ba(s) --Co(s) --Co(NO3),(aq) --Ba(NO3), --NaCl(aq) Show the flow of the electrons, half reactions, processes, and ALL ions that are relevant to the critical processes in the cell. ef e — < ‘ Ca \\(\N\L/\ N ] L Ba (K02 Co (No5) Metals on Table J Process: mocbz,’hoh Process: I‘QQL\/LQJ"IN-/ Half Reaction: "\30:1 —> P’SCJH"* e~ Half Reaction: Cos™ 2 4 Zv_ ] G:) ¢ What is the cathode? What is its charge? () What is the anode? What is its charge? Bo (- What is the charge of the solition d‘(-JE to the reaction occurring in the beaker containing Ba(s)? psSiHve What is the charge of the solution due to the reaction occurring in the beaker containing Co(s)? MSCLfi i Which electrode is gaining mass? Co ( &%ofi) Which electrode is losing mass?

17. Construct a functioning electrolytic cell using the parts prowded in the diagram as well as the following materials. --LiF(/) --graphite electrodes Show the flow of the electrons, half reactions, processes, and ALL ions that are relevant to the critical processes ot e = Ry W T T, in the cell. _6, N O A 3 @ 41 NSNS i u@“ (L) - process: X idedTun process re.ducdion . Half—reaction;mj - > pz_ S P Ha]f—reaction:(b"’ He — LA) & Circle the anode of the battery. Box in the cathode of the battery. What is the charge of the anode? Why? (- Tl wlechalutic coll by te loloels What is the charge of the cathode? Why? (=) St reoson Why does the LiF salt have to be in a molten state? (s hore o e free o mmove What would happen if you flipped the‘battery around during the reaction? Lons wovld hare gpre Ha opposite. durechon \H,\L lett wov ld e boon e cothvee ard- ‘J(LJL onoole on e H%L#

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18. You want the fishing pole you used to win the Bassmaster Classic nickel plated for posterity. Diagram the flow of the electrons, solutions, half reactions, processes, and ALL ions that are relevant to the critical processes in the cell. e et fhoce o — (NU3)» Process: rtd/b\/(‘fi[’w Process 6% 1 dahon Half-reaction: £ J{ 1% +2e¢ — —> N Half-reaction: [\)‘ ¥ s M‘ '1’2+&L_ Circle the anode of the battery. Box in the cathode of the battery. What is the anode of tge cell? What is its charge? Ny anodi (+) What is the cathode of the cell? What is its charge? hclrwb pole ()} What is gaining mass? What is losing mass? Wi gnocls

FARC What is the oxidation number of oxygen in HSO4 ? 1. +1 @—2 . +6 4. —4 Which half-reaction correctly represents a reduction reaction? 1. Sn’+2¢ — Sn* 2. Na’+e —Na* 3. Li+e —Li @ Br,’ +2e” — 2Br~ In the redox reaction: Fe(s) + CuSO4(ag) — FeSO4(agq) + Cu(s), there is a conservation of 1. mass, only 2. charge, only both mass and charge ” neither mass nor charge In an electrolytic cell, oxidation takes place at the @ anode, which is positive / 2. anode, which is negative 3. cathode, which is positive 4. cathode, which is negative ‘Which half-reaction correctly represents reduction? Fe** +2¢ — Fe’ 2. Fe*' +e —Fe™ M& 2 3. Fel+2¢ — Fe** i 4. Fe'+e — Fe*' 0 Which redox equation is rrectly balanced” 1. Cr’*+Mg—Cr+ Mg2+ W@ 2. APT+K— Al+K 3. Sn*"+H, — Sn+2H" _ }@ @Brz+Hg—>HgZ++2Br W‘/ ® ] 7 e & 3 The diagram represents a voltaic cell. Which statement correctly describes the direction of flow for the ions in this cell when the switch is closed? 1. Jons move through the salt bridge from B to C, only. 2. Jons move through the salt bridge from C to B, only. Tons move through the salt bridge in both directions. 4. Tons do not move through the salt bridge in either direction. The diagram represents a voltaic cell. When the switch is closed, which group of letters correctly represents the direction of electron flow? 1. A-B—-C—D &®A4—-F—-E—-D 3. D-C—>B—4 4 D->F—>E—A4 5.

In which compound does chlorine have an oxidation number of +7? @ HClo, 2. HCIO; 3. HCIO2 4. HCIO Given the reaction: _Hger + éAgo — _(_Hg0 + & A g1+ When the equation is completely balanced using the smallest whole-number coefficients, the coefficient of Hg will be The diagram shows a voltaic cell. The reaction occurs at 1 atmosphere and 298 K. ? Switch Voltmeter v 1.0 M Ph{NO,), Zn'(s) + P (ag) —= Zii(aq) + PB’ (s) When the switch is closed, what occurs? 1. Pbis oxidized and electrons flow to the Zn electrode. 2. Pbisreduced and electrons flow to the Zn electrode. Zn is oxidized and electrons flow to the Pb electrode. 4. Znisreduced and electrons flow to the Pb \ electrode. Given the reaction: Ca(s) + Cu**(ag) — Ca**(aq) + Cu(s) What is the correct reduction half-reaction? @ Cu”(aq) +2¢ — Cu(s) 2. Cu**(ag) — Cu(s) +2e” 3. Cu(s) +2e — Cu’ *(aq) 4. Cu(s) — Cu**(aq) +2¢~ In the reaction: 2Al(s) + 3Cu* (ag) — 2A1*(ag) + 3Cu(s) The Al(s) 1. gains protons 2. loses protons 3. gains electrons loses electrons The purpose of a salt bridge in a voltaic cell is to 1. allow for the flow of molecules between the solutions @ allow for the flow of ions between the solutions 3. prevent the flow of molecules between the solutions 4. prevent the flow of ions between the solutions (+) FORK TO BE S———" PLATED BATTERY AQNO, [ag) PSS 77 The diagram represents the electroplating of a metal fork with Ag(s). Which part of the electroplating is represented by the fork? WQ 1. the anode, which is the negative electrode \QJ @ the cathode, which is the negative electrod 3. the anode, which is the positive electrode 4. the cathode, which is the positive electrode

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(&) FORK TO BE ] PLATED BATTERY AgNO, (aq) LTI The diagram represents the electroplating of a fork with Ag(s). Which equation represents the half- reaction that takes place at the fork? 1. Ag"+NO;” — AgNO; 2. AgNO; — Ag"+NO;~ @ Ag +e — Ag(s) 4. Ag(s) — Ag +e An electrolytic cell is different from a voltaic cell because in an electrolytic cell 1. aredox reaction occurs 2. aspontaneous reaction occurs 3. an electric current is produced @ an electric current causes a chemical A ) reaction Electrode A Which type of cell does the diagram represent? @electrolytic, with the anode at 4 2. electrolytic, with the cathode at 4 3. voltaic , with the anode at 4 4. voltaic , with the cathode at 4 In which species does hydrogen have an oxidation number of -1? 1. H,O 2. H; @ NaH 4. NaOH SWITCH ( BEAKER Sn™ (ag) SOLUTION The diagram shows an electrolytic cell in which the electrodes are tin and copper. When the switch is closed, what will happen to the two electrodes? 1. B will dissolve and 4 will become coated with tin. A will dissolve and B will become coated with tin. 3. Bwill dissolve and 4 will become coated with copper. 4. A will dissolve and B will become coated with copper. SWITCH 4 BEAKER Cu [s]) Sn” [aq) SOLUTION The diagram shows an electrolytic cell in which the electrodes are tin and copper. In this electrolytic cell, electrode 4 is designated as the Given the reaction: Fe(s) + Sn4+(aq) — Fe2+(aq) F Sn**(ag) @ anode and is positive 2. anode and is negative 3. cathode and is positive 4. cathode and is negative 1. Fe(s) @ sn*(aq) 3. Fe*'(ag) 4. Sn**(aq) Cuts) Quth -

Activity Series (Table J) 19. According to Reference Table J, which pair will react spontaneously at 298K? A) Cu+Hz0 B) Au+H20 @ ca+H:0 D) Ag+H0 20. Based on Reference Table J, which reaction will take place spontaneously? &YBa(s) +2 Na*(aq) — Ba?*(aq) + 2 Na(s) B) Mg(s) + Ca?*(aq) — MgZ*(aq) + Ca(s) C) Ix(g) + 2 Br(aq) — 2 I(aq) + Br2(g) D) Cla(g) + 2 F(aq) — 2 Cl(aq) + F2(g) 21. According to Reference Table J, which atom-ion pair will react spontaneously? A) Zn + Ca?* EDAg + Awst C) Pb + Co?* D) Ni + Al 22. According to Ref e J, which species is the strongegtoxidizing agent? - (\’b gl B) Li* i &F© ) ”XQM © F D) Li(s) 23. Based on Reference Table J, which metal will not react with 1 M HCI? A) Zn(s) Au(s) C) Ni(s) D) Sa(s) 24. Based on Reference Table J, which of the following ions in aqueous solution is most easily oxidized? ABr@ I COF D)Cr 25. According to Reference Table J, which species can reduce Cr3* jons? @ Al B) Fe¥* C)Ni D) Sn?* 26. According to reference Table J, which reaction will occur spontaneously? @ Ag* +Cu(s) - Ag(s) + Cu™ B) Fe2"+ Hg(e) — Fe(s) + Hg?* C) Co* + Cu(s) — Co(s) + Cu?* D) Mg + Sn¥* — Mg(s) + Sn#* 28. According to Reference Table J, which metal will react spontaneously with H*? @ B)yAu C)Cu D)Ag 29. Lead is a product of the reaction between a solutien of lead (IT) nitrate and A)Cu @Fe C)Au D) Ag 30. Based on Reference Table J, wh1 h mdafion most likely to occur? @ Mg — Mg +2e~ % /fiy D) Cu — Cu?* +2e- 31. According to Reference Table I, which ion will oxidize Fe? A) Ca* A) Au — AudT+3e~ B) Ag— Agl¥+1le” B) Mg2+ @ Cut &C) Zn* 2. Based on Reference Table J, which of the following elements is the most actively oxidized? @st B ©OF Dcu 33. The half-reaction 2 H(aq) + 2 — Ha(g) will occur when Hf(aq) reacts with A) Hy(h) B) Ag(s) <) Cu(s) @ Pos) 34. Based on Reference Table J, which reaction will take place spontaneously? A)2Au+6HY 52 A0 +3H B) Cu+2H » CuZ* +H @ Po+2H" > P +H, D) 2Ag+2H »2Ag +H2 35. According to Reference Table T, which halogen will react spontaneously with Au(s) to produce Au? —= OOdr2ec 27. According to Reference Table J, which ion is ) F: B) I C) Cl2 D) Br2 most easily reduced? @ 2 ) I ) Cl2 D) Brz A1 X @ gl 3ly reducosl C) Mg D) Al “‘{ . Version 1 Page2 REDOX HW PACKET -20

chemchpt17AktiveRvw_Unit_9_ANSWERS_new

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