what do you do in chapter 17 for chemistry?
595913
My chapter 17 is about Reaction Energy and Reaction Kinetics\n\nsections:\n\n17-1 Thermochemistry\n17-2 Driving Force of Reactions\n17-3 The Reaction Process\n17-4 Reaction Rate
404386
I BLEW UP MY VERY FIRST EXPERIMENT\n\nI have the dubious distinction of having been the only one I know to have\nblown-up my very first chemistry experiment.  Basically it was done not so\nmuch to acquire knowledge as to familiarize us with the equipment.  The\nidea was to put some materials on a flat piece of steel, place it on a ring\nabove a bunsen burner, and heat it.  As I recall we had a strip of\nmagnesium, some sugar, a piece of iron, some sulfur and a few other odds &\nends.  The sulfur was the only thing that did anything interesting (so\nfar).  It's important to note the arrangement of the counters on which we\nworked.  The tops had a sink off to one end and there were two gas valves\nfor the burners, one on each side of the sink's faucet with the outlets\npointing toward the sink.\n\nAnyway, once I had successfully made the collection of stuff on the steel\nplate red hot and noted the results on paper it was time to clean up.\nUnfortunately in the process of shutting down the heat I had pulled the\nhose off the gas valve shortly before turning it off.  The gas collected in\nthe sink.  When the hot metal met the gas: WHOOMP!  Credible observers tell\nme I was standing there momentarily enveloped by a bright blue ball\n that stretched from the sink to the ceiling.  I lost most of my eyebrows,\nthe hair on my arms, but got a fairly good haircut once I'd shampooed the\nodor out.
337510
For math, do your homework every night. Go and ask your teacher questions every time you don't understand. \n\nFor history, find out before hand what will be on the tests and what formats they'll be in. Ask your teacher how you can best study for them. \n\nAs for your grades in general, do EVERY single assignment, even if they seem dumb. All the points add up by the end of the quarter.
1151125
for understanding organic chem u must know all the reactions by heaart, that u can do by preparing charts of various reaction n relating each other . the more u read more u become strong in it. books by s chand publication is good
198230
Go to:\nhttp://www.cliffsnotes.com/WileyCDA/LitNote/id-150.html
1185308
I did this.\n\nMath - If you have problems in the back of each chapter for review, look at each one and determine if you know the steps to solve it, if yes - move on, if no, review that area of the chapter and do a couple of practice problems.  Then move on.\n\nBe sure that you are bing honest with yourself - the only person you are hurting is yourself, if you skip ones that you are unsure of.\n\nThis may work for science as well.\n\nAs for literature.  Get together with others in your class and discuss salient points in each story - review you class notes and move on...\n\nHistory - chapter review for dates and events and the inter-dependencies.\n\nGet off the computer.  Do the work - each day.
581516
I would suggest that you cover in your subject orientation specifics of\n1. Textbook(s) required\n2. Approximate amount of homework/outside reading expected\n3. Lab safety\n4. Lab report format\n5. Any other classroom policies (cell phones on manner mode, class attendance, number of absences tolerated, etc)\n6. Test policies and schedules\n\nIn short, what should the students expect in your class. \n\nAnd most of all, I would give them a brief but heart-felt why chemistry is important not only for their grade but in this world. If you don't know this, you better research it before you start teaching it.\n\nBest of luck, fellow teacher.
597404
Read the chapter(s) thoroughly, make notes and go through them on a regular basis. Scrutinize each and every point or phrase or date, and that the best way
905163
1) determine the mass of carbon, hydrogen and oxygen.\ncarbon: 65.45% x 4.13 g = 2.703 g\nhydrogen: 5.49% x 4.13 g = 0.227 g\noxygen: 29.06% x 4.13 g = 1.200 g\n\n2) convert to moles.\ncarbon: 2.703 / 12 = 0.225 mol\nhydrogen: 0.27 / 1 = 0.227 mol\noxygen: 1.200 / 16 = 0.0750 mol\n\n3) divide each molar amount by the lowest value to obtain small integers\ncarbon: 0.225 / 0.075 = 3\nhydrogen: 0.227 / 0.075 = 3\noxygen: 0.075 / 0.075 = 1\n\nThe empirical formula of the substance is (C3H3O)k\nThe atomic masses add up to 55. To find k we need the molar mass of the compound. Use PV=nRT and plug in the data given *in the correct SI units*. Solve for n the number of moles in the sample. You problably find 5.51/55 or 5.51/110 so that k=1 or 2
690662
http://cwx.prenhall.com/bookbind/pubbooks/hillchem3/medialib/media_portfolio/text_images/CH08/FG08_17.JPG
744727
go to inorganic industral chemistry book
266694
Balance the equation.\n\nDetermine what the limiting reactant is.\n\nDetermine how much product can be produced from the limiting reactant.\n\nDetermine how much of each reactant is needed to fully react the limiting reactant.  The remainder of each reactant is the excess.
1044758
Refer with 10th class chemistry book.
242431
Practice.\n\nPracticing helps you learn the important things quicker.  When you have to constantly use a formula over and over again, it becomes easier.  Get experinece working the types of problems you will be asked.\nAlso, a good chem. lab section will help too, you get practical experience and you see that this stuff actually does have a use in real life.
819482
why dont you check out the XII th comprehensive chemistry practical reader??.........or anyother practical readers available in the market...............suggested ones are like soap formation........food adulteration.........fruit and vegetable juice analysis, toothpaste analysis.........caffeine.........aspirin......tanic acid found in tea leaves..........sea water .........all u have to do is buy that comprehensive  chemistry practical reader and choose from the given list............................\nbest of luck!!! :)
146440
1. Identify the problem. \n\n2. Refer to as many sources as possible.\n\n3. Ask an appropriate question. \n\n4. Develop a hypothesis.\n\n5. Do the experiment.\n\n6. Keep good records of the methods and results.\n\n7. Report the experiment.\n\n8. Analyze the results.\n\n9. Develop a conclusion.
1083567
I don't know if there is a standard format, and formats usually very from subject to subject.  I can send you an undergrad chem lab report.  What email address should I send it to?