how do I do a chemistry experiment where I have to figure out the moles of sucrose in bubble gum?
604031
get the mass of sucrose that you're dealing with\n\nget the atomic mass of sucrose itself\n\nmass of sucrose / atomic mass of sucrose = moles
577077
Chemical reactions are fun how about a baking soda volcano?\nor you can make an experiment showing air pressure and oxygen use, use a big clear jar( mayo peanut butter) a pie plate a bit of modeling clay a candle and some colored water and some pennies.\nplace the clay  in the center of the pie plate\nplace the pennies 2 or 3 high( you may wish to tape them, make 3 or 4 sets set them around the clay so they will support the jar up from the bottom of the pie plate\nplace a birthday candle into the clay  fill the pie plate with enough colored water to cover the edge of the jar and a little more when it is upside down on the pennies\nnow remove the jar, light the candle and replace the jar over it.\nThe candle will go out. this shows that fire needs oxygen and uses the oxygen in the jar.\nIf your jar is not too big you will see the water rise up into the jar. The gas in the jar has changed, it does not have the same pressure it did before the oxygen was removed. The pressure from the outside air makes the water rise. This demonstrates air pressure. Have the teacher light the candle. try it at home a few times you may have to change jar or glass size to get a good effect.\nI do not recommend the electric pickle experiment.
591409
BLUE GUM:\nThe gum base materials go into the mixer first (a large vessel with rotating blades). Next, the sweeteners, softeners, and colors are transferred and added.\nFollowing the initial mixing, the flavors are added, and then blending is continued very slowly, for just the right amount of time required by the formula. \n\nHOW GUM IS MADE: Gum Made By Confectioniers \n\nQuality Control specialists carefully inspect and test all ingredients before processing to make sure that every batch is pure and wholesome. Also, each batch of gum is tested during the processing operation to ensure the finest quality. \n\nThe manufacture takes place in a spotless, air-conditioned rooms and is closely monitored to meet the high standards of quality. The process begins with the accurate weighing of all the ingredients. The gum base materials go into the mixer first (a large vessel with rotating blades)*.\nNext, the sweeteners, softeners, and colors are transferred and added.\nFollowing the initial mixing, the flavors are added, and then blending is continued very slowly, for just the right amount of time required by the formula. At this point, the gum looks like stiff, colored bread dough. \n\n* The gum base is melted, washed and filtered then blended with synthethic and natural resins, etc. It is then heated, mixed, cooled and 'blcoked' for storage untill needed. \n\nWhen the blending is completed, the gum passes between rollers that press it into a flowing ribbon. The thick ribbon of fragrant gum moves through a sheeting machine, which is a series of rollers, each pair of rollers\nbeing set closer together, reducing the gum's thickness is stages. When the rollers press it to the exact thickness desired, the ribbon of gum is scored in a pattern of single sticks, long tapes or prepared in another way for packaging. \n\nThe next stop is the conditioning room. Here the temperature and humidity are carefully controlled to make sure the finished gum will stay on store shelves. \n\nThe process for making chunk bubble gum is essentially the same except that after the ingredients are blended, the mixture goes through an extruding process. This process changes the bubble gum into a solid, rope like form. To visualize what happends during extrusion, imagine pushing toothpast out of a tube. This rope is then put on a moving belt and passed through a conditioning tunnel to cool it and develop its texture.\nImmediately after this, the rope-shaped gum is cut into one-inch long chunks and individually wrapped. \n\nBubble gum balls are made the very same way. The mixture goes through an extruding process. This machine extrudes the gum into a long hollow rope like tube. The tube is then cut into small pieces then the ends are closed forming the hollow balls. The hollow balls are then put into a michine that puts an even coating of sealing substances like\ncandy/color over each then polishes each with edible waxes. \n\nThe final stage is packaging. Because of the various shapes and sizes of brands, packaging must take place on special machines. These machines package each gum according to its type. \n\nBubble Gum differs from chewing gum in that more rubber latex is used as a base ingredient for its greater elasticity. \n\n-X-X-X-X-X\n\nBASIC GUM INGREDIENTS \n\nCommon ingredients in gum are: sugar, gum base, corn syrup, softeners (like vegetable oil), flavoring, and coloring. Gum base is mostly synthetic (plastics and rubber), but it may also contain a natural product called latex.\nNatural latex is the sap from the trees of the rain forests. It is taken from the trees in much the same way as maple syrup. Some kinds of latex used in gum bases are: Chicle from the sapodilla tree, jeultong and sorva from trees of the same names. Gum manufacturers keep their recipes secret. Exact ingredients and differences between gums are a mystery. \n\nNatural and synthetic gum bases are melted together into syrup. Sugar, corn syrup and softeners are added and
1034078
You could do a base and acid mix and explain the reaction, such as vinegar and baking soda.\n\nAlso the erupting marshmallow mixture is pretty cool... and edible.\n\nCheck out this link for a bunch of cool activities you could do.\nhttp://www.calstatela.edu/dept/chem/chem2/LACTE/K12.html
196868
Put some vinegar in a small soda bottle.  Use a straw with an end of it cut so it is like a spoon to put baking soda in a balloon.  Carefully place the end of the balloon on the top of the soda bottle working around the grooves of the bottle, but not dumping the baking soda in yet.  When you are ready, lift the balloon up so that the baking soda dumps into the vinegar, and watch the balloon inflate.  You just showed a chemical reaction.
933475
You just need the density of sugar. That will give you the weight/vol.\nDivide 1g by the density will give you the volume of 1g.\n\n Then take the cube root of the volume to find the size of the cube.\n\nI search and found the density to be 1.6 g/cm^3\n\nso, if it were 1 g/cm^ the cube would be 1 cm on a side\nif it were 2 g/cm^ the cube would be (1/2)^(1/3) on a side.\n\nJust calculate (1/1.6)^(1/3) = s length of side of your cube in cm.
30706
test the reactions of different substances in water. like um put in sugar and salt and then say it dissolved. And put in oil and say it freakin stayed seperate or whatever it does
913627
Hey, i'm doing that for Chem coursework too! AS right?\nanyway, im not entirely sure, but the most important bit you need is a gas syringe to measure the volume of gas.\nOther bits u will need r:\n-conical flask on tripod, with bunsen underneath.\n-A bung with a glass tube in, to put in the conical flask.\n-This tube leads to the gas syringe, via a rubber seal.\n-Remember the CaCO3 goes in the conical flask.\n-Now all you need to do is heat the CaCO3.\n\nYour welcome!
279807
A lot depends upon how hungry you are when you start putting them in (in my case it is usually zero) :)\n\nIf it is a serious question and you can't afford to buy enough jellybeans to test it out, then buy a small bag, empty them into a small straight glass, so that the glass is full, and slowly pour some sugar into the glass until the gaps are filled up (gently tap the glass to make the sugar settle).\n\nEmpty all the jellybeans out and put the sugar back into the glass, measure how high the sugar is (ie. 1 inch) put the sugar back in the bag.\n\nNow fill the glass up with water, but less the height you measured (ie. 1 inch).... This gives you the volume of the jellybeens, now count the jellybeans and divide the volume by the number of jellybeans, you now have the volume of 1 jellybean.\n\nNow it is just a matter of finding out how big that jar you mentioned is and dividing it's volume by the volume of 1 jellybean.\n\nPresto you have the number of jelly beans in your jar :)\n\nPS. some jellybean manufacturers might have different sizes, try to find a typical sized bean :)
898790
ok...\nweigh a sample of hydrated gypsum,\nput it in an oven set at 110 degrees C for a day or so. will evaporate the H2O\nre-weigh.\nfrom the difference, the weight of h2o is found, and then number of moles can be found.\nmoles = mass / MW.\n\nthen determine number of moles in gypsum sample left.\nthen you will have a ratio.\nand that ratio should be 1:2\nie calcium sulfate dihydrate, CaSO4·2H2O.\n\ncheers
805979
6.85% x 2.500 x 10^3 = 171.25g\n\nDon't waste your time trying to figure out the molecular weight of sucrose.  That is irrelevant.
32482
To find how many grams are in a solution, you need to know how many moles there are. \n\n1 M= 1 mole/L\nor Molarity = moles/volume\n\nmoles= Molarity*volume= (0.033 L)(0.150 M)=.00495 moles.\nYou have to convert mL to L because molarity is in L.\n\nGrams is moles multiplied by molar mass.\nMolar mass is calculated by adding the masses of the individual elements.\nmolar mass= 2N + 8H + 1S + 4O\n=2(14.0) + 8(1.00) + 1(32.1) + 4(16.0)\n=164.2 g/mol\n\ngrams= (164.2 g/mol)(.00495 mol)= .81279 g (NH4)2SO4\n\ngrams= 0.813 g (NH4)2SO4.  (sig figs)
362008
vinegar and baking soda. \nWill also be fun experiment for them!
177885
Take various juices and put food coloring in them. Have some students taste the juices and see if they are fooled. Copy that down and make a chart for every juice and how many were fooled and not. It should be interesting. (I suggest water into purple to look like grape juice...and so on for others)
969783
1) determine the mass of carbon, hydrogen and oxygen.\ncarbon: 6.406 g x (12 / 44) = 1.747 g\nhydrogen: 5.244 g x (2 / 18) = 0.583 g\noxygen: 4.664 - 1.747 - .583 = 2.334 g\n\n2) convert to moles.\ncarbon: 1.747 / 12 = 0.146 mol\nhydrogen: 0.583 / 1 = 0.583 mol\noxygen: 2.334 / 16 = 0.146 mol\n\n3) divide each molar amount by the lowest value\ncarbon: 0.146 / 0.146 = 1\nhydrogen: 0.583 / 0.146 = 4\noxygen: 0.146 / 0.146 = 1\n\nWe have now arrived at the answer: the empirical formula of the substance is CH4O.\nThe atomic masses add up to 32, which is also the molar mass of the compound.
470391
http://www.rpi.edu/dept/bcbp/molbiochem/MBWeb/mb1/part2/sugar.htm\n\nSimple web search
550253
This time we use oxygen to burn the sugar:\n\nSugar + Oxygen = Carbon Dioxide + Water + Energy\n\nUsing glucose:\nC_6H_12O_6 + 6 O_2 -> 6 CO_2 + 6H_2O + Energy