Stoichiometry Predicting amounts of reagents needed or amounts
![Stoichiometry Predicting amounts of reagents needed or amounts of products made Stoichiometry Predicting amounts of reagents needed or amounts of products made](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-1.jpg)
![2 C 2 H 6 + 7 O 2 4 CO 2 + 6 2 C 2 H 6 + 7 O 2 4 CO 2 + 6](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-2.jpg)
![4 X 2 C 2 H 6 + 7 O 2 4 CO 2 4 X 2 C 2 H 6 + 7 O 2 4 CO 2](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-3.jpg)
![5 X 2 C 2 H 6 + 7 O 2 4 CO 2 5 X 2 C 2 H 6 + 7 O 2 4 CO 2](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-4.jpg)
![5 X 2 C 2 H 6 + 7 O 2 4 CO 2 5 X 2 C 2 H 6 + 7 O 2 4 CO 2](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-5.jpg)
![Coefficients in Balanced Equations • Give relative number of particles in rxn. • Give Coefficients in Balanced Equations • Give relative number of particles in rxn. • Give](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-6.jpg)
![Gas-Phase Equations • 1 mole of any gas occupies the same volume as any Gas-Phase Equations • 1 mole of any gas occupies the same volume as any](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-7.jpg)
![N 2(g) + 3 H 2(g) 2 NH 3(g) • How much hydrogen gas N 2(g) + 3 H 2(g) 2 NH 3(g) • How much hydrogen gas](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-8.jpg)
![A word about …. A word about ….](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-9.jpg)
![Single Replacement Reactions • A + BX AX + B • Element + Compound Single Replacement Reactions • A + BX AX + B • Element + Compound](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-10.jpg)
![Single Replacement Rxns 2 Li(s) + 2 H 2 O(l) 2 Li. OH(aq) + Single Replacement Rxns 2 Li(s) + 2 H 2 O(l) 2 Li. OH(aq) +](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-11.jpg)
![Single Replacement Rxns • Another common type is when one metal replaces another metal Single Replacement Rxns • Another common type is when one metal replaces another metal](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-12.jpg)
![Single Replacement Reactions • Metals have different reactivities. • You have to predict if Single Replacement Reactions • Metals have different reactivities. • You have to predict if](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-13.jpg)
![Single Replacement Rxns • Table J is an activity series. The more reactive a Single Replacement Rxns • Table J is an activity series. The more reactive a](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-14.jpg)
![Single Replacement Rxns • The rule is: • A metal can replace any metal Single Replacement Rxns • The rule is: • A metal can replace any metal](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-15.jpg)
![Ag(s) + Cu(NO 3)2(aq) ? • What is the metal and the metal cation? Ag(s) + Cu(NO 3)2(aq) ? • What is the metal and the metal cation?](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-16.jpg)
![Cu(s) + 2 Ag. NO 3(aq) ? • • What is the metal and Cu(s) + 2 Ag. NO 3(aq) ? • • What is the metal and](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-17.jpg)
![Single Replacement Reactions • 3 rd common type: • A nonmetal replaces another nonmetal Single Replacement Reactions • 3 rd common type: • A nonmetal replaces another nonmetal](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-18.jpg)
![Single Replacement Reactions • The rule is: • A more active halogen replaces a Single Replacement Reactions • The rule is: • A more active halogen replaces a](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-19.jpg)
![Single Replacement Reaction • Br 2(g) + 2 Na. F(aq) ? NR • Br Single Replacement Reaction • Br 2(g) + 2 Na. F(aq) ? NR • Br](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-20.jpg)
![Use Table J to predict if these reactions occur. • • K(s) + Zn. Use Table J to predict if these reactions occur. • • K(s) + Zn.](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-21.jpg)
![Summary: Predicting Single Replacement Reactions 1) Identify stand-alone element. 2) Determine if stand-alone element Summary: Predicting Single Replacement Reactions 1) Identify stand-alone element. 2) Determine if stand-alone element](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-22.jpg)
![A word about … A word about …](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-23.jpg)
![Reactions in aqueous solution • Many reactions, esp. many double replacement reactions, occur in Reactions in aqueous solution • Many reactions, esp. many double replacement reactions, occur in](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-24.jpg)
![Dissolving • Covalent substance – sugar or C 6 H 12 O 6 • Dissolving • Covalent substance – sugar or C 6 H 12 O 6 •](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-25.jpg)
![Dissolving • Ionic substance – table salt or Na. Cl • Na. Cl(s) Na+(aq) Dissolving • Ionic substance – table salt or Na. Cl • Na. Cl(s) Na+(aq)](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-26.jpg)
![Double Replacement Reactions • Often occur when you mix 2 solutions of ionic compounds. Double Replacement Reactions • Often occur when you mix 2 solutions of ionic compounds.](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-27.jpg)
![Reactions producing Solids • • Precipitation: the opposite of dissolving! What do you see Reactions producing Solids • • Precipitation: the opposite of dissolving! What do you see](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-28.jpg)
![Reactions producing Solids 2 Na. OH(aq) + Cu. Cl 2(aq) 2 Na. Cl(aq) + Reactions producing Solids 2 Na. OH(aq) + Cu. Cl 2(aq) 2 Na. Cl(aq) +](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-29.jpg)
![Complete Ionic Equations 2 Na+(aq) + 2 OH-(aq) + Cu 2+(aq) + 2 Cl-(aq) Complete Ionic Equations 2 Na+(aq) + 2 OH-(aq) + Cu 2+(aq) + 2 Cl-(aq)](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-30.jpg)
![Net Ionic Equations 2 Na+(aq) + 2 OH-(aq) + Cu 2+(aq) + 2 Cl-(aq) Net Ionic Equations 2 Na+(aq) + 2 OH-(aq) + Cu 2+(aq) + 2 Cl-(aq)](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-31.jpg)
![Reactions that form Water HBr(aq) + Na. OH(aq) H 2 O(l) + Na. Br(aq) Reactions that form Water HBr(aq) + Na. OH(aq) H 2 O(l) + Na. Br(aq)](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-32.jpg)
![Reactions that form Gases HCl(aq) + Na. HCO 3(aq) H 2 CO 3(aq) + Reactions that form Gases HCl(aq) + Na. HCO 3(aq) H 2 CO 3(aq) +](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-33.jpg)
![Reactions that form Gases HCl(aq) + Na. HCO 3(aq) H 2 O(l) + CO Reactions that form Gases HCl(aq) + Na. HCO 3(aq) H 2 O(l) + CO](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-34.jpg)
![Conservation of Charge • Total charge on reactant side must equal total charge on Conservation of Charge • Total charge on reactant side must equal total charge on](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-35.jpg)
- Slides: 35
![Stoichiometry Predicting amounts of reagents needed or amounts of products made Stoichiometry Predicting amounts of reagents needed or amounts of products made](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-1.jpg)
Stoichiometry Predicting amounts of reagents needed or amounts of products made
![2 C 2 H 6 7 O 2 4 CO 2 6 2 C 2 H 6 + 7 O 2 4 CO 2 + 6](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-2.jpg)
2 C 2 H 6 + 7 O 2 4 CO 2 + 6 H 2 O • How much CO 2 will be produced if 4 moles of C 2 H 6 are consumed? Identify a stoichiometry problem: 1) You always get a balanced chemical equation. 2) The problem will ask how many moles or how many liters given a certain amount of something else. 3) The equation has a arrow.
![4 X 2 C 2 H 6 7 O 2 4 CO 2 4 X 2 C 2 H 6 + 7 O 2 4 CO 2](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-3.jpg)
4 X 2 C 2 H 6 + 7 O 2 4 CO 2 + 6 H 2 O • How much CO 2 will be produced if 4 moles of C 2 H 6 are consumed? 4 moles C 2 H 6 ______ 2 moles C 2 H 6 = X moles CO ______2 4 moles CO 2 X = 8 moles CO 2
![5 X 2 C 2 H 6 7 O 2 4 CO 2 5 X 2 C 2 H 6 + 7 O 2 4 CO 2](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-4.jpg)
5 X 2 C 2 H 6 + 7 O 2 4 CO 2 + 6 H 2 O • How much H 2 O will be produced in the combustion of 5 moles of C 2 H 6? 5 moles C H 2 6 ______ 2 moles C 2 H 6 = X moles H O 2 ______ 6 moles H 2 O X = 15 moles H 2 O
![5 X 2 C 2 H 6 7 O 2 4 CO 2 5 X 2 C 2 H 6 + 7 O 2 4 CO 2](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-5.jpg)
5 X 2 C 2 H 6 + 7 O 2 4 CO 2 + 6 H 2 O • How much oxygen will react with 5 moles of C 2 H 6? 5 moles C H 2 ______6 2 moles C 2 H 6 = X moles O 2 ______ 7 moles O 2 X = 17. 5 moles O 2
![Coefficients in Balanced Equations Give relative number of particles in rxn Give Coefficients in Balanced Equations • Give relative number of particles in rxn. • Give](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-6.jpg)
Coefficients in Balanced Equations • Give relative number of particles in rxn. • Give relative number of moles in rxn. • Coefficients give relationship between moles of each component in equation. • You use these relationships in MOLE-MOLE problems to convert from moles of 1 substance to moles of another substance.
![GasPhase Equations 1 mole of any gas occupies the same volume as any Gas-Phase Equations • 1 mole of any gas occupies the same volume as any](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-7.jpg)
Gas-Phase Equations • 1 mole of any gas occupies the same volume as any other gas. At STP, 22. 4 L. • So coefficients in equations represent the ratio of the volumes of gases involved in the reaction. • For rxns where all reactants & products are gases, volume-volume problems. • Unit doesn’t matter as long as it’s constant throughout.
![N 2g 3 H 2g 2 NH 3g How much hydrogen gas N 2(g) + 3 H 2(g) 2 NH 3(g) • How much hydrogen gas](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-8.jpg)
N 2(g) + 3 H 2(g) 2 NH 3(g) • How much hydrogen gas will react with 15 liters of nitrogen gas? 15 L N 2(g) _____ 1 L N 2(g) = X = 45 L H 2(g) X L H 2(g) _____ 3 L H 2(g)
![A word about A word about ….](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-9.jpg)
A word about ….
![Single Replacement Reactions A BX AX B Element Compound Single Replacement Reactions • A + BX AX + B • Element + Compound](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-10.jpg)
Single Replacement Reactions • A + BX AX + B • Element + Compound New Element + New Compound
![Single Replacement Rxns 2 Lis 2 H 2 Ol 2 Li OHaq Single Replacement Rxns 2 Li(s) + 2 H 2 O(l) 2 Li. OH(aq) +](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-11.jpg)
Single Replacement Rxns 2 Li(s) + 2 H 2 O(l) 2 Li. OH(aq) + H 2(g) • In this reaction, a metal replaces a hydrogen in a water molecule.
![Single Replacement Rxns Another common type is when one metal replaces another metal Single Replacement Rxns • Another common type is when one metal replaces another metal](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-12.jpg)
Single Replacement Rxns • Another common type is when one metal replaces another metal in a compound. • Cu(s) + 2 Ag. NO 3(aq) 2 Ag(s) + Cu(NO 3)2(aq)
![Single Replacement Reactions Metals have different reactivities You have to predict if Single Replacement Reactions • Metals have different reactivities. • You have to predict if](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-13.jpg)
Single Replacement Reactions • Metals have different reactivities. • You have to predict if a given metal and a given compound will react or not.
![Single Replacement Rxns Table J is an activity series The more reactive a Single Replacement Rxns • Table J is an activity series. The more reactive a](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-14.jpg)
Single Replacement Rxns • Table J is an activity series. The more reactive a metal, the easier it loses its valence electrons. • The most active metal is at the top • The least active metal is at the bottom • Use Table J to determine if a reaction will occur.
![Single Replacement Rxns The rule is A metal can replace any metal Single Replacement Rxns • The rule is: • A metal can replace any metal](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-15.jpg)
Single Replacement Rxns • The rule is: • A metal can replace any metal listed below it that is in a compound. • It cannot replace any metal listed above it.
![Ags CuNO 32aq What is the metal and the metal cation Ag(s) + Cu(NO 3)2(aq) ? • What is the metal and the metal cation?](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-16.jpg)
Ag(s) + Cu(NO 3)2(aq) ? • What is the metal and the metal cation? • Ag and Cu+2 • Locate Ag and Cu in Table J. • Ag is below Cu so this reaction will not go. Ag is less reactive than Cu.
![Cus 2 Ag NO 3aq What is the metal and Cu(s) + 2 Ag. NO 3(aq) ? • • What is the metal and](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-17.jpg)
Cu(s) + 2 Ag. NO 3(aq) ? • • What is the metal and the metal cation? Cu and Ag+1 Locate Cu and Ag in Table J. Cu is above Ag in Table J. Cu is more reactive than Ag. This reaction will go. • 2 Ag(s) + 2 Cu(NO 3)2(aq)
![Single Replacement Reactions 3 rd common type A nonmetal replaces another nonmetal Single Replacement Reactions • 3 rd common type: • A nonmetal replaces another nonmetal](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-18.jpg)
Single Replacement Reactions • 3 rd common type: • A nonmetal replaces another nonmetal in a compound. • Halogens are often the nonmetal. • Halogens also have different reactivities. • Look at Table J. • Most active halogen = fluorine at top. • Least active halogen = iodine at bottom.
![Single Replacement Reactions The rule is A more active halogen replaces a Single Replacement Reactions • The rule is: • A more active halogen replaces a](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-19.jpg)
Single Replacement Reactions • The rule is: • A more active halogen replaces a less active halogen that is part of a compound in aqueous solution. • F 2(g) + 2 Na. Br(aq) 2 Na. F(aq) + Br 2(l) • This reaction occurs because F 2 is above Br 2.
![Single Replacement Reaction Br 2g 2 Na Faq NR Br Single Replacement Reaction • Br 2(g) + 2 Na. F(aq) ? NR • Br](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-20.jpg)
Single Replacement Reaction • Br 2(g) + 2 Na. F(aq) ? NR • Br 2 is below F 2 in Table J. This reaction does not occur.
![Use Table J to predict if these reactions occur Ks Zn Use Table J to predict if these reactions occur. • • K(s) + Zn.](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-21.jpg)
Use Table J to predict if these reactions occur. • • K(s) + Zn. Cl 2(aq) Yes Fe(s) + Na 3 PO 4(aq) No Cu(s) + Mg(NO 3)2(aq) No Yes Al(s) + Sn. Cl 2(aq) No Ca(s) + KBr(aq) Yes Ti(s) + Pb(NO 3)2(aq) No Cl 2(g) + HF(aq) F 2(g) + Ca. I 2(aq) Yes
![Summary Predicting Single Replacement Reactions 1 Identify standalone element 2 Determine if standalone element Summary: Predicting Single Replacement Reactions 1) Identify stand-alone element. 2) Determine if stand-alone element](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-22.jpg)
Summary: Predicting Single Replacement Reactions 1) Identify stand-alone element. 2) Determine if stand-alone element is a metal or a nonmetal. (For the purposes of Table J, H 2 is a metal. ) 3) Compare the stand-alone element to the corresponding element in the compound. 4) If the stand-alone element is higher in Table J than the corresponding element in the compound, then the reaction occurs.
![A word about A word about …](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-23.jpg)
A word about …
![Reactions in aqueous solution Many reactions esp many double replacement reactions occur in Reactions in aqueous solution • Many reactions, esp. many double replacement reactions, occur in](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-24.jpg)
Reactions in aqueous solution • Many reactions, esp. many double replacement reactions, occur in water. • What happens when substances dissolve in water? • Depends on if they are ionic or covalent.
![Dissolving Covalent substance sugar or C 6 H 12 O 6 Dissolving • Covalent substance – sugar or C 6 H 12 O 6 •](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-25.jpg)
Dissolving • Covalent substance – sugar or C 6 H 12 O 6 • C 6 H 12 O 6(s) C 6 H 12 O 6(aq) • The sugar molecules are spread out among the water molecules.
![Dissolving Ionic substance table salt or Na Cl Na Cls Naaq Dissolving • Ionic substance – table salt or Na. Cl • Na. Cl(s) Na+(aq)](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-26.jpg)
Dissolving • Ionic substance – table salt or Na. Cl • Na. Cl(s) Na+(aq) + Cl-(aq) • The ions are spread out among the water molecules.
![Double Replacement Reactions Often occur when you mix 2 solutions of ionic compounds Double Replacement Reactions • Often occur when you mix 2 solutions of ionic compounds.](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-27.jpg)
Double Replacement Reactions • Often occur when you mix 2 solutions of ionic compounds. – 1 product may be water or – 1 product may be a gas or – 1 product may be a solid • We say these reactions “go to completion. ”
![Reactions producing Solids Precipitation the opposite of dissolving What do you see Reactions producing Solids • • Precipitation: the opposite of dissolving! What do you see](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-28.jpg)
Reactions producing Solids • • Precipitation: the opposite of dissolving! What do you see in the following clips: S 1043. mov S 1045. mov S 1046. mov S 1050. mov S 1057. mov S 1058. mov and S 1060. mov
![Reactions producing Solids 2 Na OHaq Cu Cl 2aq 2 Na Claq Reactions producing Solids 2 Na. OH(aq) + Cu. Cl 2(aq) 2 Na. Cl(aq) +](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-29.jpg)
Reactions producing Solids 2 Na. OH(aq) + Cu. Cl 2(aq) 2 Na. Cl(aq) + Cu(OH)2(s) Complete Chemical Equation
![Complete Ionic Equations 2 Naaq 2 OHaq Cu 2aq 2 Claq Complete Ionic Equations 2 Na+(aq) + 2 OH-(aq) + Cu 2+(aq) + 2 Cl-(aq)](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-30.jpg)
Complete Ionic Equations 2 Na+(aq) + 2 OH-(aq) + Cu 2+(aq) + 2 Cl-(aq) 2 Na+(aq) + 2 Cl-(aq) + Cu(OH)2(s) Substances that are ions in solution are written as ions in solution.
![Net Ionic Equations 2 Naaq 2 OHaq Cu 2aq 2 Claq Net Ionic Equations 2 Na+(aq) + 2 OH-(aq) + Cu 2+(aq) + 2 Cl-(aq)](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-31.jpg)
Net Ionic Equations 2 Na+(aq) + 2 OH-(aq) + Cu 2+(aq) + 2 Cl-(aq) 2 Na+(aq) + 2 Cl-(aq) + Cu(OH)2(s) Notice that some ions do not participate in the reaction. They are spectator ions. Cross out all the spectator ions & you get the net ionic equation. 2 OH-(aq) + Cu 2+(aq) Cu(OH)2(s)
![Reactions that form Water HBraq Na OHaq H 2 Ol Na Braq Reactions that form Water HBr(aq) + Na. OH(aq) H 2 O(l) + Na. Br(aq)](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-32.jpg)
Reactions that form Water HBr(aq) + Na. OH(aq) H 2 O(l) + Na. Br(aq) H+(aq) + Br-(aq) + Na+(aq) + OH-(aq) H 2 O(l) + Na+(aq) + Br-(aq) H+(aq) + OH-(aq) H 2 O(l)
![Reactions that form Gases HClaq Na HCO 3aq H 2 CO 3aq Reactions that form Gases HCl(aq) + Na. HCO 3(aq) H 2 CO 3(aq) +](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-33.jpg)
Reactions that form Gases HCl(aq) + Na. HCO 3(aq) H 2 CO 3(aq) + Na. Cl(aq) H 2 CO 3(aq) H 2 O(l) + CO 2(g) ___________________ HCl(aq) + Na. HCO 3(aq) H 2 O(l) + CO 2(g) + Na. Cl(aq)
![Reactions that form Gases HClaq Na HCO 3aq H 2 Ol CO Reactions that form Gases HCl(aq) + Na. HCO 3(aq) H 2 O(l) + CO](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-34.jpg)
Reactions that form Gases HCl(aq) + Na. HCO 3(aq) H 2 O(l) + CO 2(g) + Na. Cl(aq) H+(aq) + Cl-(aq) + Na+(aq) + HCO 3 -(aq) H 2 O(l) + CO 2(g) + Na+(aq) + Cl-(aq) H+(aq) + HCO 3 -(aq) H 2 O(l) + CO 2(g)
![Conservation of Charge Total charge on reactant side must equal total charge on Conservation of Charge • Total charge on reactant side must equal total charge on](https://slidetodoc.com/presentation_image_h/0f12f361d8ed8e3baa2fddaf9e68f683/image-35.jpg)
Conservation of Charge • Total charge on reactant side must equal total charge on product side.
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