chemchpt17AktiveRvw_Unit_9_ANSWERS_new

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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\
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,
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