Chapter 11 – Chemical Reactions In chemical reactions, old bonds are broken and new bonds are formed - the breaking of bonds requires energy (absorbs energy) - the forming of new bonds releases energy - the atoms involved are not created or destroyed, they just rearrange Ex: CH 4 + O 2 CO 2 + H 2 O Hydrocarbon – combo of C’s and H’s that burn (react with oxygen) to produce CO 2 and H 2 O. (s) – solid Fe (s) + O 2(g) Fe 2 O 3(s) (l) – liquid (g) – gas indicate physical state of matter(aq) – aqueous
MnO 2 H 2 O 2(l) H 2 O (l) + O 2(g) indicates a catalyst – a substance that speeds up a reaction without itself being used up.
Balancing Equations - same # of atoms on each side ___H 2(g) + ___O 2(g) ___H 2 O (l) ___Ag(NO 3 ) (aq) + ___Cu (s) ___Cu(NO 3 ) (aq) + ___Ag (s) ___Al (s) + ___O 2(g) ___Al 2 O 3(s) HW# 1a) __PbO 2 __PbO + __O 2 b) __P + __O 2 __P 4 O 10
#2a) carbon + oxygen carbon monoxide b) Potassium nitrate potassium nitrite + oxygen c) Hydrogen + sulfur hydrogen sulfide Ch11 HW#1 1,2
HW #1 - 1,2 1 c) _ Al + _ N 2 _ AlN d) _ Li + _ FeBr 2 _ Li Br + _Fe f) _ NaCl + _H 2 (SO 4 ) _ HCl + _ Na 2 (SO 4 ) g) _ H 2 + _ Fe 3 O 4 _ Fe + 4 H 2 O h) _ Al + _ Cu(SO 4 )_ Al 2 (SO 4 ) 3 + _ Cu
HW #1 - 1,2 1 c) 2 Al + 1 N 2 2 AlN d) _ Li + _ FeBr 2 _ Li Br + _Fe f) _ NaCl + _H 2 (SO 4 ) _ HCl + _ Na 2 (SO 4 ) g) _ H 2 + _ Fe 3 O 4 _ Fe + 4 H 2 O h) _ Al + _ Cu(SO 4 )_ Al 2 (SO 4 ) 3 + _ Cu
HW #1 - 1,2 1 c) 2 Al + 1 N 2 2 AlN d) 2 Li + FeBr 2 2 Li Br + Fe f) _ NaCl + _ H 2 (SO 4 ) _ HCl + _ Na 2 (SO 4 ) g) _ H 2 + _ Fe 3 O 4 _ Fe + 4 H 2 O h) _ Al + _ Cu(SO 4 )_ Al 2 (SO 4 ) 3 + _ Cu
HW #1 - 1,2 1 c) 2 Al + 1 N 2 2 AlN d) 2 Li + FeBr 2 2 Li Br + Fe f) 2 NaCl + H 2 (SO 4 ) 2 HCl + Na 2 (SO 4 ) g) _ H 2 + _ Fe 3 O 4 _ Fe + 4 H 2 O h) _ Al + _ Cu(SO 4 )_ Al 2 (SO 4 ) 3 + _ Cu
HW #1 - 1,2 1 c) 2 Al + 1 N 2 2 AlN d) 2 Li + FeBr 2 2 Li Br + Fe f) 2 NaCl + H 2 (SO 4 ) 2 HCl + Na 2 (SO 4 ) g) 4 H 2 + Fe 3 O 4 3 Fe + 4 H 2 O h) _ Al + _ Cu(SO 4 )_ Al 2 (SO 4 ) 3 + _ Cu
HW #1 - 1,2 1 c) 2 Al + 1 N 2 2 AlN d) 2 Li + FeBr 2 2 Li Br + Fe f) 2 NaCl + H 2 (SO 4 ) 2 HCl + Na 2 (SO 4 ) g) 4 H 2 + Fe 3 O 4 3 Fe + 4 H 2 O h) 2 Al + 3 Cu(SO 4 ) Al 2 (SO 4 ) Cu
2d) Iron(III)chloride + calcium hydroxide iron(III)hydroxide + calcium chloride e) sodium + watersodium hydroxide + hydrogen f) hydrogen + sulfurhydrogen sulfide
2d) Iron(III)chloride + calcium hydroxide iron(III)hydroxide + calcium chloride 2 FeCl Ca(OH) 2 2 Fe(OH) CaCl 2 e) sodium + watersodium hydroxide + hydrogen Na + H 2 O Na(OH) + H 2 2 Na + 2 H(OH)2 Na(OH) + H 2 f) hydrogen + sulfurhydrogen sulfide H 2 + SH 2 S
Ch11.2 – Types of Reactions: Combination and Decomposition Only be certain of the outcome of a reaction by actually performing an experiment. 1. Combination Reaction - 2 or more substances react to form a single substance. Mg (s) + O 2(g) S (s) + O 2(g) SO 3(g) CaO (s) + H 2 O (l)
Only be certain of the outcome of a reaction by actually performing an experiment. 1. Combination Reaction - 2 or more substances react to form a single substance. 2 Mg (s) + O 2(g) 2 MgO (s) 2 S (s) + 3 O 2(g) 2 SO 3(g) CaO (s) + H 2 O (l) Ca(OH) 2(aq)
HW #3c) Ca + S d) Fe + O 2 (Iron (II) oxide)
HW #3c) Ca + S Ca + S CaS d) Fe + O 2 (Iron (II) oxide) 2 Fe + O 2 2 FeO
2. Decomposition Reactions – a single compound is broken down into 2 or more products. H 2 O (l) Mercury (II) oxide C 12 H 22 O 11 Ch11 HW#2 3,4
2. Decomposition Reactions – a single compound is broken down into 2 or more products. 2 H 2 O (l) 2 H 2 + O 2 Mercury (II) oxide Hg +2 O -2 2 HgO2 Hg + O 2 C 12 H 22 O C + 11 H 2 0 Ch11 HW#2 3,4
Ch11 HW#2 (3,4) 3a) _ Mg + _ O 2 b) P + O 2 Tetraphosphorous Decoxide e) _ NO + _O 2
Ch11 HW#2 (3,4) 3a) _ Mg + _ O 2 _ MgO 2 Mg + 1 O 2 2 MgO b) P + O 2 Tetraphosphorous Decoxide e) _ NO + _O 2 _ NO 2
Ch11 HW#2 (3,4) 3a) _ Mg + _ O 2 _ MgO 2 Mg + 1 O 2 2 MgO b) P + O 2 Tetraphosphorous Decoxide 4 P + 5 O 2 P 4 O 10 e) _ NO + _O 2 _ NO 2
Ch11 HW#2 (3,4) 3a) _ Mg + _ O 2 _ MgO 2 Mg + 1 O 2 2 MgO b) P + O 2 Tetraphosphorous Decoxide 4 P + 5 O 2 P 4 O 10 e) _ NO + _O 2 _ NO 2 2 NO + 1O 2 2 NO 2
Ch11 HW#2 (3,4) 4a) HBr b) NaCl c) Ag 2 O d) HgO
Ch11 HW#2 (3,4) 4a) HBr H 2 + Br 2 2 HBr H 2 + Br 2 b) NaCl Na + Cl 2 c) Ag 2 OAg + O 2 d) HgOHg + O 2
Ch11 HW#2 (3,4) 4a) HBr H 2 + Br 2 2 HBr H 2 + Br 2 b) NaCl Na + Cl 2 2 NaCl 2 Na + Cl 2 c) Ag 2 OAg + O 2 d) HgOHg + O 2
Ch11 HW#2 (3,4) 4a) HBr H 2 + Br 2 2 HBr H 2 + Br 2 b) NaCl Na + Cl 2 2 NaCl 2 Na + Cl 2 c) Ag 2 OAg + O 2 2 Ag 2 O 4Ag + O 2 d) HgOHg + O 2
Ch11 HW#2 (3,4) 4a) HBr H 2 + Br 2 2 HBr H 2 + Br 2 b) NaCl Na + Cl 2 2 NaCl 2 Na + Cl 2 c) Ag 2 OAg + O 2 2 Ag 2 O 4Ag + O 2 d) HgOHg + O 2 2 HgO 2 Hg + O 2
Ch11 HW#2 (3,4) 4e) Copper (I) chloride f) Copper (II) chloride
Ch11 HW#2 (3,4) 4e) Copper (I) chloride Cu +1 Cl -1 2 CuCl 2 Cu + Cl 2 f) Copper (II) chloride
Ch11 HW#2 (3,4) 4e) Copper (I) chloride Cu +1 Cl -1 2 CuCl 2 Cu + Cl 2 f) Copper (II) chloride Cu +2 Cl -1 1 CuCl 2 1 Cu + 1 Cl 2
Ch11.2 Cont. Single Displacement Reactions – atoms of one element replace the atoms of a second element in a compound. Zn +HCl Li + H 2 O Mg + AgNO 3 Mg +KNO 3
HW# 5 d) Cl 2(l) + KI (aq) I 2 +KCl f) Cu (s) +FeSO 4(aq) Fe + Cu 2 SO 4
Double Replacement Reactions – involves the exchange of positive ions between 2 compounds. Usually one of the following occurs: 1.One product is a precipitate. Na 2 S (aq) + Cd(NO 3 ) 2(aq) CdS (s) + NaNO 3(aq)
Double Replacement Reactions – involves the exchange of positive ions between 2 compounds. Usually one of the following occurs: 1.One product is a precipitate. Na 2 S (aq) + Cd(NO 3 ) 2(aq) CdS (s) + NaNO 3(aq) 2. One product is a gas, bubbles out. NaCN (aq) + H 2 SO 4(aq) HCN (g) + Na 2 SO 4(aq)
Double Replacement Reactions – involves the exchange of positive ions between 2 compounds. Usually one of the following occurs: 1.One product is a precipitate. Na 2 S (aq) + Cd(NO 3 ) 2(aq) CdS (s) + NaNO 3(aq) 2. One product is a gas, bubbles out. NaCN (aq) + H 2 SO 4(aq) HCN (g) + Na 2 SO 4(aq) 3. One product is a molecule, possibly water. Ca(OH) 2 + HCl (aq) CaCl 2(aq) + H(OH) (l) Ch11 HW#3 5,6
Ex: AgNO 3(aq) + KCl (aq) Ch11 HW#3 5,6
HW #3 - 5,6 5a) _ Ag (s) + _ KNO 3(aq) b) _ Zn (s) + _ AgNO 3(aq) c) _ Al (s) + _ S 2 SO 4(aq) e) _ Li (s) + _ H 2 O (l)
HW #3 - 5,6 5a) 1 Ag (s) + 1 KNO 3(aq) 1 K + 1 AgNO 3 b) _ Zn (s) + _ AgNO 3(aq) c) _ Al (s) + _ S 2 SO 4(aq) e) _ Li (s) + _ H 2 O (l)
HW #3 - 5,6 5a) 1 Ag (s) + 1 KNO 3(aq) 1 K + 1 AgNO 3 b) 1 Zn (s) + 2 AgNO 3(aq) 2 Ag + 1 Zn(NO 3 ) 2 c) _ Al (s) + _ S 2 SO 4(aq) e) _ Li (s) + _ H 2 O (l)
HW #3 - 5,6 5a) 1 Ag (s) + 1 KNO 3(aq) 1 K + 1 AgNO 3 b) 1 Zn (s) + 2 AgNO 3(aq) 2 Ag + 1 Zn(NO 3 ) 2 c) 2 Al (s) + 3 S 2 SO 4(aq) 3 H Al 2 (SO 4 ) 3 e) _ Li (s) + _ H 2 O (l)
HW #3 - 5,6 5a) 1 Ag (s) + 1 KNO 3(aq) 1 K + 1 AgNO 3 b) 1 Zn (s) + 2 AgNO 3(aq) 2 Ag + 1 Zn(NO 3 ) 2 c) 2 Al (s) + 3 S 2 SO 4(aq) 3 H Al 2 (SO 4 ) 3 e) 2 Li (s) + 1 H 2 O (l) 1 H Li 2 O
HW#3 - 5,6 6a) HCl (aq) + Ca(OH) 2(aq) b) Ag 2 SO 4 + AlCl 3 c) KOH + H 3 PO 4
6a) HCl (aq) + Ca(OH) 2(aq) Ca +2 Cl -1 + H(OH) ___HCl (aq) + ___Ca(OH) 2(aq) ___CaCl 2 + ___H(OH) 2 HCl (aq) + 1 Ca(OH) 2(aq) 1 CaCl H(OH) b) Ag 2 SO 4 + AlCl 3 c) KOH + H 3 PO 4
6a) HCl (aq) + Ca(OH) 2(aq) Ca +2 Cl -1 + H(OH) ___HCl (aq) + ___Ca(OH) 2(aq) ___CaCl 2 + ___H(OH) 2 HCl (aq) + 1 Ca(OH) 2(aq) 1 CaCl H(OH) b) Ag 2 SO 4 + AlCl 3 Ag +1 Cl -1 + Al +3 SO 4 -2 ___ Ag 2 SO 4 + ___AlCl 3 ___AgCl + ___Al 2 (SO 4 ) 3 3 Ag 2 SO AlCl 3 6 AgCl + 1 Al 2 (SO 4 ) 3 c) KOH + H 3 PO 4
6a) HCl (aq) + Ca(OH) 2(aq) Ca +2 Cl -1 + H(OH) ___HCl (aq) + ___Ca(OH) 2(aq) ___CaCl 2 + ___H(OH) 2 HCl (aq) + 1 Ca(OH) 2(aq) 1 CaCl H(OH) b) Ag 2 SO 4 + AlCl 3 Ag +1 Cl -1 + Al +3 SO 4 -2 ___ Ag 2 SO 4 + ___AlCl 3 ___AgCl + ___Al 2 (SO 4 ) 3 3 Ag 2 SO AlCl 3 6 AgCl + 1 Al 2 (SO 4 ) 3 c) KOH + H 3 PO 4 K +1 PO H(OH) ___KOH + ___H 3 PO 4 ___K 3 PO 4 + ___H(OH) 3 KOH + 1 H 3 PO 4 1 K 3 PO H(OH)
6d) H 2 SO 4 + Al(OH) 3 e)SrBr 2 + (NH 4 ) 2 CO 3
6d) H 2 SO 4 + Al(OH) 3 Al +3 SO H(OH) ___H 2 SO 4 + ___Al(OH) 3 ___Al 2 (SO 4 ) 3 + ___H(OH) 3 H 2 SO Al(OH) 3 1 Al 2 (SO 4 ) H(OH) e)SrBr 2 + (NH 4 ) 2 CO 3
6d) H 2 SO 4 + Al(OH) 3 Al +3 SO H(OH) ___H 2 SO 4 + ___Al(OH) 3 ___Al 2 (SO 4 ) 3 + ___H(OH) 3 H 2 SO Al(OH) 3 1 Al 2 (SO 4 ) H(OH) e)SrBr 2 + (NH 4 ) 2 CO 3 Sr +2 CO NH 4 +1 Br -1 ___SrBr 2 + ___(NH 4 ) 2 CO 3 ___SrCO 3 + ___NH 4 Br 1 SrBr (NH 4 ) 2 CO 3 1 SrCO NH 4 Br
Ch11.2c – Combustion Reactions An element or compound reacts with oxygen producing energy in the form of heat and light. Hydrocarbons: ___CH 4 + ___O 2 ___C 2 H 6 + ___O 2 ___C 3 H 8 + ___O 2 Methane Ethane Propane
ID type of rxns & balance HW - 8a) ___Hf + ___N 2 ___Hf 3 N 4 ____ b) ___Mg + ___H 2 SO 4 ___MgSO 4 + ___H 2 ____ c) ___C 2 H 6 + ___O 2 ___CO 2 + ___H 2 O____ d) ___Pb(NO 3 ) 2 + ___Na I ___Pb I 2 + ___NaNO 3 ____ Ch11 HW #4 7,8
7 a) Butane gas, C 4 H 8 ___C 4 H 8 + ___O 2 ___CO 2 + ___H 2 O b) Glucose, C 6 H 12 O 6 ___C 6 H 12 O 6 + ___O 2 ___CO 2 + ___H 2 O c) Octane, C 8 H 18 ___C 8 H 18 + ___O 2 ___CO 2 + ___H 2 O Ch11 HW#4 7,8
7 a) Butane gas, C 4 H 8 1 C 4 H O 2 4 CO H 2 O b) Glucose, C 6 H 12 O 6 ___C 6 H 12 O 6 + ___O 2 ___CO 2 + ___H 2 O c) Octane, C 8 H 18 ___C 8 H 18 + ___O 2 ___CO 2 + ___H 2 O Ch11 HW#4 7,8
7 a) Butane gas, C 4 H 8 1 C 4 H O 2 4 CO H 2 O b) Glucose, C 6 H 12 O 6 1 C 6 H 12 O O 2 6 CO H 2 O c) Octane, C 8 H 18 ___C 8 H 18 + ___O 2 ___CO 2 + ___H 2 O Ch11 HW#4 7,8
7 a) Butane gas, C 4 H 8 1 C 4 H O 2 4 CO H 2 O b) Glucose, C 6 H 12 O 6 1 C 6 H 12 O O 2 6 CO H 2 O c) Octane, C 8 H 18 2 C 8 H O 2 16 CO H 2 O Ch11 HW#4 7,8
Balance & ID 8)e) ___Fe + ___O 2 ___Fe 3 O 4 ______ f) __Hg(NO 3 ) 2 + __NH 4 SCN __Hg(SCN) 2 + __NH 4 NO 3 ______ g) __(NH 4 ) 2 SO 4 + __NaOH __NH 4 OH + __Na 2 SO 4 ______
Balance & ID 8)e) 3 Fe + 2 O 2 1 Fe 3 O 4 Combination f) __Hg(NO 3 ) 2 + __NH 4 SCN __Hg(SCN) 2 + __NH 4 NO 3 ______ g) __(NH 4 ) 2 SO 4 + __NaOH __NH 4 OH + __Na 2 SO 4 ______
Balance & ID 8)e) 3 Fe + 2 O 2 1 Fe 3 O 4 Combination f) 1 Hg(NO 3 ) NH 4 SCN 1 Hg(SCN) NH 4 NO 3 Double Replacement g) __(NH 4 ) 2 SO 4 + __NaOH __NH 4 OH + __Na 2 SO 4 ______
Balance & ID 8)e) 3 Fe + 2 O 2 1 Fe 3 O 4 Combination f) 1 Hg(NO 3 ) NH 4 SCN 1 Hg(SCN) NH 4 NO 3 Double Replacement g) 1 (NH 4 ) 2 SO NaOH 2 NH 4 OH + 1 Na 2 SO 4 D.R.
Types of Chemical Reactions Synthesis Reaction: a+b ab 2H 2 (g)+O 2 (g) 2H 2 O(g) Decomposition Reaction: ab a+b 2H 2 O(l) Electric Current 2H 2 (g)+O 2 (g) Single Displacement Reaction: a+bc ac+b Zn(s)+Cu(NO 3 ) 2 (aq) Zn(NO 3 ) 2 (aq)+Cu(s) Double-Displacement Reaction: ab+cd ad+cb AgNO 3 (aq)+NaCl(aq) AgCl(s)+NaNO 3 (aq) Combustion Reaction: ab+O 2 oxide of a + oxide of b CH 4 (g)+2O 2 (g) CO 2 (g)+2H 2 O(g)
Ch11.5 – Net Ionic Equations AgNO 3(aq) + KCl (aq)
Ch11.5 – Net Ionic Equations AgNO 3(aq) + KCl (aq) Ag + (aq) + NO 3 - (aq) + Na + (aq) + Cl - (aq) AgCl (s) + Na + (aq) + NO 3 - (aq) AgNO 3(aq) + KCl (aq) AgCl (s) + KNO 3(aq) Net Ionic Eqn: Ag + (aq) + Cl - (aq) AgCl (s)
Ex 1) ID the spectator ions: a) HCl (aq) + ZnS (aq) b) Cl 2(g) + NaBr (aq)
Ex 1) ID the spectator ions: a) HCl (aq) + ZnS (aq) H 2 S (g) + ZnCl 2(aq) H + (aq) + Cl - (aq) + Zn +2 (aq) + S -2 (aq) H 2 S (g) + Zn +2 (aq) + 2Cl - (aq) NIE: 2H + (aq) + S -2 (aq) H 2 S (g) b) Cl 2(g) + NaBr (aq) Br 2(l) + NaCl (aq) Cl 2(g) + Na +1 (aq) + Br -1 (aq) Br 2(l) + Na + (aq) + Cl - (aq) NIE: Cl 2(g) + 2Br -1 (aq) Br 2(l) + 2Cl - (aq)
c) HCl (aq) + NaOH (aq)
c) HCl (aq) + NaOH (aq) NaCl (aq) + H(OH) (l) H + (aq) + Cl - (aq) + Na + (aq) + OH - (aq) Na + (aq) + Cl - (aq) + H(OH) l NIE: H + (aq) + OH - (aq) H(OH) (l) Ch11 HW#5 9 – 11
9. Distinguish between the complete equation and the net ionic equation. 10. Write the NIE: a. Pb(ClO 4 ) 2(aq) + NaI (aq) PbI 2(s) + NaClO 4(aq) b. Zn (s) + HCl (aq) ZnCl 2(aq) + H 2(g) c. Ca(OH) 2(aq) + H 3 PO 4(aq) Ca 3 PO 4(aq) + H 2 O (l)
Ch11 HW#5 9 – Distinguish between the complete equation and the net ionic equation. 10. Write the NIE: a. Pb(ClO 4 ) 2(aq) + NaI (aq) PbI 2(s) + NaClO 4(aq) Pb +2 (aq) + 2I -1 (aq) PbI 2(s) b. Zn (s) + HCl (aq) ZnCl 2(aq) + H 2(g) c. Ca(OH) 2(aq) + H 3 PO 4(aq) Ca 3 PO 4(aq) + H 2 O (l)
Ch11 HW#5 9 – Distinguish between the complete equation and the net ionic equation. 10. Write the NIE: a. Pb(ClO 4 ) 2(aq) + NaI (aq) PbI 2(s) + NaClO 4(aq) Pb +2 (aq) + 2I -1 (aq) PbI 2(s) b. Zn (s) + HCl (aq) ZnCl 2(aq) + H 2(g) Zn (s) + 2H +1 (aq) Zn +2 (aq) + H 2(g) c. Ca(OH) 2(aq) + H 3 PO 4(aq) Ca 3 PO 4(aq) + H 2 O (l)
Ch11 HW#5 9 – Distinguish between the complete equation and the net ionic equation. 10. Write the NIE: a. Pb(ClO 4 ) 2(aq) + NaI (aq) PbI 2(s) + NaClO 4(aq) Pb +2 (aq) + 2I -1 (aq) PbI 2(s) b. Zn (s) + HCl (aq) ZnCl 2(aq) + H 2(g) Zn (s) + 2H +1 (aq) Zn +2 (aq) + H 2(g) c. Ca(OH) 2(aq) + H 3 PO 4(aq) Ca 3 PO 4(aq) + H 2 O (l) 3(OH) -1 (aq) + 3H +1 (aq) 3H 2 O (l)
11. Complete each and write NIE: a. Al (s) + H 2 SO 4(aq) b. HCl (aq) + Ba(OH) 2(aq)
11. Complete each and write NIE: a. Al (s) + H 2 SO 4(aq) Al 2 (SO 4 ) 3(aq) + H 2(g) Al (s) + H +1 (aq) + SO 4 -2 (aq) Al +3 (aq) + SO 4 -2 (aq) + H 2(g) Al (s) + 2H +1 (aq) Al +3 (aq) + H 2(g) b. HCl (aq) + Ba(OH) 2(aq)
11. Complete each and write NIE: a. Al (s) + H 2 SO 4(aq) Al 2 (SO 4 ) 3(aq) + H 2(g) Al (s) + H +1 (aq) + SO 4 -2 (aq) Al +3 (aq) + SO 4 -2 (aq) + H 2(g) Al (s) + 2H +1 (aq) Al +3 (aq) + H 2(g) b. HCl (aq) + Ba(OH) 2(aq) BaCl 2(aq) + H(OH) (l) H +1 (aq) + Cl -1 (aq) + Ba +2 (aq) + OH -1 (aq) Ba +2 (aq) + Cl -1 (aq) + HOH (l) H +1 (aq) + OH -1 (aq) H(OH) (l)
Ch11 Review #1 1. __NaNO 2 + __FeSO 4 __Na 2 SO 4 + __Fe(NO 2 ) 2 2. __Al 2 (SO 4 ) 3 + __HCl __H 2 SO 4 + __AlCl 3 3. __BaCl 2 + __Na 2 SO 4 __NaCl + __BaSO 4 4. __KCl + __Pb(NO 3 ) 2 __KNO 3 + __PbCl 3 5. __Mg + __HCl __MgCl 2 + __H 2 6. __C 2 H 5 OH + __O 2 __CO 2 + __H 2 O 7. __HgO __Hg + __O 2 8. __KClO 3 __KCl + __O 2 9. __Na 2 O + __H 2 O __NaOH 10. __MnO + __HCl __MnCl 2 + __H 2 O 11. __Al + __HCl __AlCl 3 + __H __AgNO 3 + __NaCl __AgCl + __NaNO __Fe + __CuSO 4 __FeSO 4 + __Cu 14. __N 2 + __H 2 __NH __HgO __Hg + __O 2
Balance and list type of reaction: 16. silver + sulfur silver sulfide______ 17. __Al + __Fe 2 O 3 __Fe + Al 2 O 3 _____ 18. mecury(II)oxide mercury + oxygen______ 19. potassium chloride + silver nitrate______
20. Ca + HCl_______ 21. C 2 H 5 OH + O 2 _______ 22. hydrogen + Fe 2 O 3 iron + steam_______ 23. carbon + oxygen carbon monoxide_______ 24. __Al 2 (SO 4 ) 3 + Ca(OH) 2 aluminum hydroxide + CaSO 4 ______
Ch11 Rev WS II Classify: 1. 2KCL 3 2KCl + 3O 2 ______ 2. HCl + NaOH NaCl + H 2 O______ 3. Mg + 2HCl MgCl 2 + H 2 ______ 4. 2H 2 + O 2 2H 2 O______ 5. 2Al + 3NiBr 2 2AlBr 3 + 3Ni______ 6. 4Al + 3O 2 2Al 2 O 3 ______ 7. 2NaCl 2Na + Cl 2 ______ 8. CaCl 2 + F 2 CaF 2 + Cl 2 ______ 9. AgNO 3 + KCl AgCl + KNO 3 ______ 10. N 2 + 3H 2 2NH 3 ______ 11. 2H 2 O 2 2H 2 O + O 2 ______ 12. (NH 4 ) 2 SO 4 + Ba(NO 3 ) 2 BaSO 4 + 2NH 4 NO 3 ______ 13. MgI 2 + Br 2 MgBr 2 + I 2 ______ 14. SO 3 + H 2 O H 2 SO 4 ______ 15. 6KCl + Zn 3 (PO 4 ) 2 3ZnCl 2 + 2K 3 PO 4 ______
Balance: 1. __CH 4 + __O 2 __CO 2 + __H 2 O 2. __Na + __I 2 __NaI 3. __N 2 + __O 2 __N 2 O 4. __N 2 + __H 2 __NH 3 5. __KI + __Cl 2 __KCl + I 2 6. __HCl + __Ca(OH) 2 __CaCl 2 + __H 2 O 7. __KClO 3 __KCl + __O 2 8. __K 3 PO 4 + __HCl __KCl + __H 3 PO 4 9. __S + __O 2 __SO __KI + __Pb(NO 3 ) 2 __KNO 3 + __PbI __CaSO 4 + __AlBr 3 __CaBr 2 + __Al 2 (SO 4 ) __H 2 O 2 __H 2 O + O __Na + __H 2 O __NaOH + __H 2
14. __C 2 H 6 + __O 2 __CO 2 + __H 2 O 15. __Mg(NO 3 ) 2 + __K 3 PO 4 __Mg 3 (PO 4 ) 2 + __KNO 3 Write and balance: 1. Hydrogen plus oxygen yield water. 2. Nitrogen plus hydrogen yield ammonia. 3. Aluminum bromide plus chlorine yield aluminum chloride and bromine. 4. Hydrochloric acid plus sodium hydroxide yield sodium chloride and water.
Ch11 Test Review 1. Iron + oxygen Iron(III)product formed 2. Phosphoric acid + Magnesium hydroxide 3. Cadmium(II)phosphate + Ammonium sulfide
4. Zinc sulfide + Oxygen 5. Calcium hydroxide + Aluminum acetate 6. Barium nitrate + Iron(III)sulfate 7. Sodium + Aluminum carbonate
8. Sulfuric acid + Aluminum hydroxide 9. Nitric acid + Potassium carbonate 10. Bromine + Cesium iodide