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AP Chemistry Electrochemistry WS 0809 key

AP Chemistry Electrochemistry WS 0809 key - AP Chemistry...

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Unformatted text preview: AP Chemistry: Electrochemistry ( AP Chemistry Electrochemistry WS 0809.doc Name: 2% Date: Per: 1. Zinc metal reacts with nitric acid, HN03, to produce a number of products, depending on how dilute the acid solution is. In a concentrated solution, zinc reduces nitrate ion to ammonium ion; zinc is oxidized to zinc ion, Zn“. Write the net ionic equation for this reaction. a. —-> Zni—ch’ icy/”+4 ’Vl’z" -—> NW" + 3”“) an" , ‘ , 7’27”» 5! +88 03n'+20fi*+N03 ”V2nH+NHY++3/lzoj 2. Permanganate ion oxidizes sulfite ion in basic solution according to the following equation: Mn04'(aq) + 5032-(aq) -) Mn02(.5) + SO42-(aq) Use the half-reaction method to complete and balance this equation. I . 2 ’- + .— 3¢’+V/'/++ M" 0‘1 ' -% Mn 02— + ZHLO ylfl+ 503 2- a $07 {.ffll at? bc' H11” + 2mm,- -—> Zwak W410 324,0 +35%:— _,, 250, 2— +6!” + M: - / ‘ a - ../' 2k” ¥+2Mn09’+w+3$032 _>ZNn&4/Y7yzo +35%? M [II/20 *zfihoy-‘Pgaa‘b'b Zflflat3591+ziffj 3. A voltaic cell is constructed from a half-cell in which a cadmium rod dips into a solution of cadmium nitrate, Cd(NO3)2, and another half-cell in which a silver rod dips into a solution of silver nitrate, AgN03. The two half-cells are connected by a salt bridge. Silver ions are reduced during the operation of the < voltaic cell. Draw a sketch of the cell. Label the anode and cathode, showing the corresponding half- reactions at these electrodes. Indicate the electron flow in the external circuit (with a lightbulb), the signs of the electrodes, and the direction of cation migration in the half-cells. 4. Write the condensed cell notation in w IC e electrode reactions are: 2H+(aq) + 2e" —) H2(g) Zn(s) —) Zn2+(aq) + 2e" 2" I in; N “Zr‘ Huylflt 5. Write the cell reaction for the voltaic cells: a. TI TI+ Sn2+ Sn (5) I (aq) ll 4 (all (s) M 5—“ 2+4 29' .9 Sm) 0X¢ Tl) ’5 7—] + e 3 b- ' Zn(s) I Zn2+(aq) H Fe3+(aq)fFe2+(aq) | Pt I 0x{ En —=> Zn“ +Ze’ ‘ F 34. .. F14“ flbal‘ 9/7) +€ 3 &Iwz) 6. The cell potential of a particular voltaic cell with the cell reaction: H922+<an + H2(9) <—> 2Hg(.) + 2H+<aq) , is 0.650V. Calculate the maximum electrical work of this cell when 0.5009 of H2 is consumed. l 'Aéo: WIkA¥ ' ’ M F E 2 (2)(% «My my) :‘I’b W 7 I WW /;, 0/_b_3/w’ : .nymi H1: -/wz/z7’tr( 176M) 3 ”"0 3 7. a. Order the fo lowing;- oxidizmg agents by' Increasing strength under standard-state conditions: ‘ Cl2( ), H202( ), F834- ( ) a 9 aq aq Fag/1437 4 011(1) A ”101(43) (IHCMS7’VU Ill/K“ WWW/II; [via/«I141: ) b. Order the following reducing agents by increasing strength under standard-state conditions: Hm), Al(s), CU(s) Cu 4 ”2. L m ”30me /; "”50”“ relay/n?» FUI‘W’M [II fiWAV‘ Im‘fhk“ 8. Consider the reaction: Does the reaction go spontaneously In the direction indicated, under standard conditions? No, 2“ch Mug/IQ”; pfl/WIL’W/ /*’ /W 71%". Irv-ms Fe 7+1», fiffiamfl 2;.” ~a£n {-0 7W) 9. Llsing standard electrode potentials, calculate the standard free-energy change at 25.0°C for the reaction: What happens to the free-enzergy if the coefficients of the reaction are doubled? What about the cell L potential? £722” 3(45/0 .,. 0,7é) , /.§’(Q l/ A6”? —n 9:32, : —(1)(%,W0)(/.54) = *30/017 o .I' a: #:602qu Jen/doles Cel/ paM/k/ row)”: {A 54/w/ 10. a. Wha is the cell potential of the following voltaic cell at 25. 0°C? r 0.35! r 0.76 ; /, /§ l/ 5" Zn | Zn2+ (1.. 00x10 5M) H Cu2+ (0.100M) | CU) ; a“ _ .5- (S) 0' bis—igévyka a HOV/(- ’28 543)] Max/6 > E00” 3 Ewll ”Eng TNHQ: -564” ( ’ 2, '4 (Dy/00 b. What' Is the equili rium constant, Keq, for this reaction under standard conditions? 5 /. 27? 7-“ o 0012613 Mr 5., we. M». W 11. When an aqueous solution of copper(II)sulfate, (0504, is Z’ectrolyzed, copper metal is deposited: CU2+(aq) + 26 —-) CU(5) (The other electrode gives oxygen. 2H20 —> 02 + 4H+ + 4e'). If a constant current is passed for 5.00h and 404mg of copper metal was deposited, what was the current? (99 (/70 c}; : 1226.524C , 1, 7/6 ,/z7w{”< £2? ,oawealfw :0 6 3.127 6;.5’5’3/g IMO” nzéw’flfcflgom s ’3 '06 9/43: 12. Write a net ionic equation for the expected reaction when the electrolysis of NiSO4(aq)' Is conducted ’0 using an Inert platinum anocfilandanickgl):acthc§|i P+ +2; Hm M f 5017/ mi‘ ,4, ”046,344 2371/ WI1+Z° ”’6 _ flM +1“, IV: Cull/000’ MY/W éao VC/Cucéal [CWWLV H RQI/ 01+ w” 4. '~/e flak/,0 90 8’ng '11-’20 +11. #9 H1f3)+10”;5)5“/F41‘° N7MIN$ acid! 1‘11 44' MflZ-Aa/ [Vial/[$43 bdMLf-A 1+hwhb?) /‘ Oxwll’r"! , 2M.2):L2~H7’0 AZUI;+OZ(j)fyé/;¢a ...
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