2. Objective/Warm-Up SWBAT review topics for the final. If you have 30 g of NaCl or 100 g of NaCl, which would have the greater % of Cl? Why? Calculate the % of Cl in 100 g of NaCl. 5:004:304:003:303:002:302:001:301:000:300:00

3. Objective/Warm-Up SWBAT review topics for the final. Perform the following conversions: 420.27 g Pb(CO 3 ) 2 = ______________ moles 33.2 g KCl = _____________ formula units 7.2 x 10 20 atoms Cu = _____________ grams Cu 5:004:304:003:303:002:302:001:301:000:300:00

4. Percent Composition- mass of element x100% total mass Empirical Formula- simplest ratio of elements Molecular Formula- “unreduced”, real, actual formula of elements Examples: Empirical Formula CH 2 ONO 2 HO Molecular Formula C 6 H 12 O 6 N2O4N2O4 H2O2H2O2

5. Change from Empirical to Molecular A compound has a molecular mass of 90 g/mol and an empirical formula of HCO 2, what is the molecular formula?

6. Percent Hydrate If you have a hydrate that weighs a total of 150 grams and you heat it so that only 70 grams are left, what percent was water?

7. C. Types of Yields of Products 1. Theoretical Yield the calculated amount that should be produced 2. Actual Yield the measured amount of a product 3. Percent Yield the efficiency of the reaction found from the ratio of the actual yield to the theoretical yield x 100 ( A/T x 100)

8. 1. When the proper amount of NH 3 reacts with enough O 2, 120.0 g of NO was produced. Tom performed the experiment, but actually produced 98.0 g NO. What is the % yield of NO? D. % Yield Stoichiometry Problems 4 NH 3 + 5 O 2  4 NO + 6 H 2 O 98.0 g NO 120.0 g NO X 100= 81.7%

9. 2. When 36.8 g of NH 3 react with excess of oxygen, the actual yield of water is 56.2 g. What is the % yield of water? 36.8 g NH 3 68.16 g NH 3 X108.1 g H 2 O= 58.4 g H 2 O 56.2 g H 2 O 58.4 g H 2 O X 100= 96.2%

10. Warm-Up: 2AlCl 3  2Al + 3Cl 2 If 35.0 g of aluminum chloride are decomposed, how many grams of chlorine are produced? What is the percent yield if only 8.50 g Cl 2 are produced? 5:004:594:584:574:564:554:544:534:524:514:504:494:484:474:464:454:444:434:424:414:404:394:384:374:364:354:344:334:324:314:304:294:284:274:264:254:244:234:224:214:204:194:184:174:164:154:144:134:124:114:104:094:084:074:064:054:044:034:024:014:003:593:583:573:563:553:543:533:523:513:503:493:483:473:463:453:443:433:423:413:403:393:383:373:363:353:343:333:323:313:303:293:283:273:263:253:243:233:223:213:203:193:183:173:163:153:143:133:123:113:103:093:083:073:063:053:043:033:023:013:002:592:582:572:562:552:542:532:522:512:502:492:482:472:462:452:442:432:422:412:402:392:382:372:362:352:342:332:322:312:302:292:282:272:262:252:242:232:222:212:202:192:182:172:162:152:142:132:122:112:102:092:082:072:062:052:042:032:022:012:001:591:581:571:561:551:541:531:521:511:501:491:481:471:461:451:441:431:421:411:401:391:381:371:361:351:341:331:321:311:301:291:281:271:261:251:241:231:221:211:201:191:181:171:161:151:141:131:121:111:101:091:081:071:061:051:041:031:021:011:00 YOU HAVE ONLY ONE MINUTE LEFT ON THIS QUESTION 0:590:580:570:560:550:540:530:520:510:500:490:480:470:460:450:440:430:420:410:400:390:380:370:360:350:340:330:320:310:300:290:280:270:260:250:240:230:220:210:200:190:180:170:160:150:140:130:120:110:100:090:080:070:060:050:040:030:020:010:00 Objective: SWBAT use stoichiometry to solve limiting reactant problems using a balanced chemical equation. 35.0 g AlCl 3 X 1 mol AlCl 3 133.35 g AlCl 3 X 3 mol Cl 2 2 mol AlCl 3 X 70.9 g Cl 2 1 mol Cl 2 =27.9 g Cl 2 % yield=8.50 g/27.9 g Cl 2 x100% = 30.5%

11. Concentration Concentration- amount of solute in a given amount of solvent or solution Molarity- moles solute L solution molality- moles solute kg solvent

12. Acids and Bases AcidBase ArrheniusReleases H+ ions (HCl) Releases OH- ions (NaOH) Bronsted- Lowery H+ (proton or hydronium ion) donor (HCl) H+ (proton or hydronium ion) acceptor (NH 3 ) LewisElectron pair acceptor (BH 3 ) Electron pair donor (NH 3 )

13. Types of Mixtures Solution- a homogeneous mixture, particles in a solution are about the size of molecules, approximately 1 nanometer Suspension- Those that make up suspensions are larger than 1,000 nanometers. Colloid- mixtures whose particles are larger than the size of a molecule but smaller than particles that can be seen with the naked eye. Finally, colloidal particles range in size between 1 and 1,000 nanometers. Colloids are also called colloidal dispersions because the particles of which they are made are dispersed, or spread out, through the mixture.