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