35. 2Al + 3FeO ~ AhO, + 3Fe A ~ 2AhO~ 47. 2Al + 6Hel ~ 2AICh + 3Hz

Transcription

1 ANSWERS: Balance the following chemical equations: (Some may already be balanced.) 2. SR ~ 8 SO~ 3. 2HgO ~2Hg + O 2 4. Zn + 2HCI + ZnCI 2 + Hz 6. CIIHJ(, + 8Cb ~ 10C + 16HCI 35. 2Al + 3FeO ~ AhO, + 3Fe 12. 2K + Brl ~ 2KBr 39. 4A ~ 2AhO~ 41. C + H 2 0 ~ CO + Hz 17. 2KC10, ~ 2KCl KCIO, ~ 3KCI04 + KCI 44. FeCI, + 3NH 4 0H ~ Fe(OHh + 3NfL C) 22. FC20, + 3CO ~ 2Fe + 3C Al + 6Hel ~ 2AICh + 3Hz 23. PCI) + 4fhO ~ SHCI + H 3 P HzS + 8CI 2 ~ Sx + 16HCI 25. 3Fe + 4HzO ~ Fe~O. + 4Hz 50. 2NaOH + Cl- ~ NaCI + NaCIO + H20

2 The boxes shown below are pictorial representations of chemical reactions. The boxes on the left represent the reactants and the boxes on the right represent the products. Conert each diagram into a balanced chemical equation. Assume the reactions occur in the gas phase. 1. When writing formulas for the compounds in this problem, write hydrogen first. For compounds containing only oxygen and sulfur, write sulfur first in the formula.!@l Hydrogen 0 Oxygen Sulfur "...-'" ~.~~ t '~'.:.. ~'\ ~'" --~ -0 q~'y <\-C \~LO\~) ~ ~--~:;--~-2'~~~1 2. When writing formulas for the compounds in this problem, write hydrogen first for compounds that contain only hydrogen and oxygen. For compounds containing carbon, write carbon first in the Hydrogen 0 Oxygen Carbon 1 b CO C6 ~ c9 cy CO --~ ~~..~...L) C 0..:.z( '3\

3 For each of the ionic and molecular compounds listed below, show how the compound dissociates or ionizes when placed in water. In the middle column, show the dissociation or ionization reaction and in the last column show the best representation of that compound in water. If the compound is insoluble, write insoluble in the middle column. When you are finished, circle all of the compounds that are acids and bases. Compound How Substance Exists in Dissociation or Ionization Reaction / Water V~ ~ypochlorous ~ acid HCIO(aq) + H20(l)~H30\aq) + ClO'(aq) HCIO(aq) sodium chloride ~~C\l~1\ ~ ~ ~~"'1\ ~ ey(<1)\ We-\CS~\ + (J0~\ POiOdiC acid) M.L 181') \- \-\LOe-') ----") \~:P~"'1)\- J:(~\ ttf7..p r c""t') t I0-f) siler chloride A~C\cS\ ~(,\C$) '-J \J.a-~CO~(""1) =>: )'W~L&'l\\-(0,0f\ sodium carbonate ~ t ~- ;Z~",t~1\ zinc nitrate ~V\ (to,) J~'}\ ---:J 20~C?\~).Uh~ ': CO~~;l'\ ;2-r- -,~\ 2tf\( ""~ ~ ~ i», (qs. ) ~mo~ia(nh0 tj~~().~ \j U,0 U \ V Ic '::0tassium hydrox~ -\- \\)..ou) ~ \\t~\"'f\ \- O~~ ~\ ~ ~~\0~\ \(08.(at\ => \,z~1\ ~ O~0b\ \,( ~"14\ t 01l"ln Sr (c.a-"':)~)~a1\ -':) {(""f\ t-- ~C1~P)1 c.jf \ '- 1f~'l \ + )(2 \i<.02("''i~ strontium acetate ~ '2r- - '-~ 7-t- ~ II ~- T u c C!:C2H2CI02~ ~ \-\~ ~J..c..\(J) (<>."ij " '\Pc.t\ ~ ~\O~.;\ ~ ( ')~)C\6~""1\ \\L 1 \-\')G\O')(,"i 7-~~:1\ iron(iii) sulfate st-,2- Fe..;2..(So~~3.,(<'11" -~ t :SS.O'1~;~\ A F~,,'i\ \-- SS0<-t(~1) - t -. ~rchloric acid) r\l\l)<-j (9",\ -\ \- C\Ol..t"'0QI mercury(i) (HCV ammonium sulfide \.\LO(-t) ----=s> \\,<0 (<'/.:j\ \- C\D~~ \~ ~O~'i" 'J u I U' ~ '\;1. S e.\ l-1c\.?-.scs ") \- - t-\w(oj 'i') -\: \-\).p(}.\ ~ ~ (p(c,~\ \-- GJ(44\ \-\C0(~'\\ 'V t- --- \- perchlorate \J 'V\ ~ C\0 c, ~i'\ -=J U\-\'\ (~.\- C\O~'-a,'t) tj ~Ltl"''\\ t- -":::> ~ \.~~\ \ 0\-\(4';)) ~ (9q, \- CLOc,(:,1J ~dium/hydrox~ NC\()\-\~~"\ \J t - \U t 04~4~J potassium oxalate ~2S~ ~ t \J.1C),Ot.; (0.4) - ~ :zl( (4'1\ \-- C)o, (4{\ 2\j~a~ ~ C20'-1~01\. ~ ~ t... l-\lso<-i(o"{) ~ t-\l.o~\--"') \-\:\01"'11 ~ t\sp~~ \ \-\~O~t\ -\- \-\~~ 01) aluminum perchlorate A \ (ClO~\~0't) - J A\1:~\ 3c\OL;la.\\ It\ ~:~\ t- ~C\o,(An potassium dihydrogen phosphite (HC2H3D0 t( ~}~o~'\ H(7.- ~~~ O"} L~1\ (41\ - ':J \( ~..'\\ \-- \~ 2~D'{(~e;\ \( ~~~\ \- \~l-po~~~,\\ t- '1..- -\- '\- '-"' ~- ~ ~Lc)(!-\ -:;;;; %0\" u;r- C))P~"'1: t\ C:L~.) ( """\~ ( CH3COOH) (JA :)LCO l-\ fi'\\ t \.-\2.001 ~ t-.\-!.,()~{\ 1-C~7LQ)(,,\{, Ct\-"{ (0() 1-\ fa.q\ <, ---! J

4 CHEM 130 Spring 2008 Conert each statement below into a balanced chemical equation. If the products are not gien, you must predict what the products will be. Most of these reactions are double displacement reactions. In your balanced chemical equation, make sure you include the physical states of the reactants and products. 1) Potassium metal reacts with fluorine gas to produce potassium fluoride. 2) Nitrogen gas reacts with hydrogen gas under high temperature to form ammonia gas. ~\\"~GV\ +~~JVllk) ~..1.L5' '\- 3>~L(~ ~ 2.\)\-\ :)Cy r: 3) Sulfur trioxide gas dissoles in water to form sulfuric acid. 4) Solid calcium carbonate is heated to form solid calcium oxide & carbon dioxide gas. 5) Water undergoes electrolysis to form oxygen gas & hydrogen gas.

5 CHEt4 130 ::spr3..ng ) Aluminum metal is placed in aqueous norodortc acid and forms aqueous aluminum chloride and hydrogen gas. () t \ r \.'. n A' (" ';:'\\. ~A,(5') +- b AC\ (~D -...:> L..~" 1~l4t) '\- ~)~~i2.<:)) 7) Copper metal is immersed in a siler chlorite solution, aqueous copper(u) chlorite and solid siler are formed. L-.:> ($) ~ 2t\ ~ OO;L(""~ ---":> G.{uoZJ2(4t) of- 2A:y:-&) 8) Aqueous barium bromate is mixed with aqueous lithium phosphate. h '\ :So\\0\ 9) Hydrochloric acid reacts with aejucet1s magnesium hydroxide. 11) propane gas, C3HSI is burnedtcornbusted). C3\.\~5> \- 50.2J~) --:> 3CO~("51,L C.:i \ \ F'>.,,nLU{~) 12) Liquid MT8E, CSH120, is burnedjcombusted). /j \\ /, S/"0-c Cs ( H,'LV( t).\-\?p.)...(~ --/ '--...!...'-S' -- 4-!SO--(~ -), ~.)