molecular weight of Allyl propionate?
449290
Allyl propionate has a molecular weight of 114.1438 amu.  A good site to go on for this sort of information is www.chemfinder.com, I use it frequently.
1126461
This is how you do it.\nYou need to find out the mass of hexane first. Calculate the mass of hexane by subtracting the mass of empty beaker from the mass of beaker with hexane. Once you obtain the mass of hexane, divide it by the volume which is 5ml. You will get your density in units g/ml. I hope this was enough help. E-mail if you need more than this.
782126
The molecular mass of Iodomethane (CH3I) is 141.94 g/mol.\n\n1g/141.94g/mol = 0.007 moles.\n\n.007 x 6.02 x 10^23 = 4.21 x 10^21 molecules.
43865
The molecular mass (abbreviated MM) of a substance (less accurately called molecular weight and abbreviated as MW) is the mass of one molecule of that substance, relative to the unified atomic mass unit u (equal to 1/12 the mass of one atom of carbon-12). Due to this relativity, the molecular mass of a substance is commonly referred to as the relative molecular mass, and abbreviated to Mr.\n\nThe molecular mass can be calculated as the sum of the atomic masses of all the atoms of any one molecule. The molecular mass can also be measured directly using mass spectrometry. In mass spectrometry, the molecular mass of a small molecule (< ~200 atoms of a given element) is exact, that is, the sum of the most common isotopes of each element. Of larger molecules, it is average, or calculated using the elemental mass number or the periodic table, since there is likely to be a statistical distribution of atoms representing the isotopes throughout the molecule.\n\nThe molar mass of a substance is numerically equal to the molecular mass, but expressed in mass units per mole, usually as g/mol (grams per mole).\n\nExample: \nThe atomic mass of hydrogen is 1.00784 u and that of oxygen is 15.9994 u; therefore, the molecular mass of water with formula H2O is (2 × 1.00784 u) + 15.9994 u = 18.01508 u. Therefore, one mole of water weighs 18.01508 grams. However, the exact mass of hydrogen-1 (the most common isotope) is 1.00783, and the exact mass of oxygen-16 (the most common isotope) is 15.9949, so the mass of the most common single molecule of water is 18.0105 u. \nMolecular mass or molar mass are used in stoichiometry calculations.\n\nSince molecules are created by chemical reactions, not nuclear reactions, a molecule's molecular mass exactly equals the sum of the atomic masses of its constituent atoms.\n\nThe gram-molecular weight is the molecular weight of a chemical compound expressed in grams. Thus the molecular weight of calcium carbonate is 100 therefore the gram-molecular weight is 100 g. The Gram Molecular Weight is frequently used, particularly for calculating the concentration of solutions. Thus a molar solution will contain the gram molecular weight of a chemical dissolved to produce one litre of solution.\n\nHandy Little Calculator:\nhttp://www.chemie.fu-berlin.de/cgi-bin/molform
363124
detlaH=H(products) - H(Reactants)\n\n200KJ/mol
880546
you should learn how to do your own homework hun you'll never be a chemist with someone else doing your work.\n\n\nuse the molar mass from the periodic table (units = g/1mol)\n\nCl = 35.5\nH = 1.00\n\nMolar mass, formula weight, molecular weight, formula mass = 36.5 grams HCl/1 mol HCl\n\n\nThis is a simple problem is you can't do this problem maybe you should try changing majors.  I hear history or english is nice.
502594
If your compound has the formula C6H10, then the molecular weight would be 82 grams/mole\n\nYou could have one of 13 different compounds -- \n2,3-dimethyl-1,3-butadiene\n3-3-dimethylbutyne\nCyclohexene\nany one of the five hexadienes\nany one of three hexynes\n4-methyl-1-pentyne\n4-methyl-2-pentyne\n\nWhat is the rest of the question regarding the 5.3*10^-23 odr?
828480
1 mol of the compound has a mass of 146.1 gram.\n1) determine the mass of carbon, hydrogen and oxygen.\ncarbon: 146.1 g x 49.31% = 72.04 g\nhydrogen: 146.1 g x 6.9% = 10.08  g\noxygen: 146.1 g x 43.79% = 63.98 g\n\n2) convert to moles.\ncarbon: 72.04 / 12.01 = 5.998 mol\nhydrogen: 10.08 / 1.008 = 10.00 mol\noxygen: 63.98 / 16.00 = 3.999 mol\n\n3) divide each molar amount by the lowest value o obtain small integers \ncarbon:  6\nhydrogen: 10\noxygen: 4\n\nThe empirical formula of the substance is (C6H10O4)n\nThe atomic masses add up to 146.1, which is also the molar mass of the compound. Therefore n=1 and we find C6H10O4
452333
its cis 1,4 polyisoprene(polymer)\n\nH2C=C(CH2)-CH=CH2
954638
It seems that you have problems with moles and Avagadro's number. You will need to refer to your periodic table to get the molecular weights that your teacher wants you to use.\n\nSo get the molecular weights of the elements you are working with from your periodic table and substitute in the formula.\n\nI am using round numbers to show the substitution you should know how many decimal points you need to work to.\n\nHG atomic weight 200\nO atmic weight 16\n\nSubstitute in the formula to get the masses involved\n\n2 HgO(s) - 2 Hg(l) + O2(g) Hrxn = 181.6 kJ\n 2 (200g + 16g)   =  2(200g) + 2(16g) = 181.6 kj  \n\n432g oxide decomposes releasing 181.6Kj\n\nQuestion a)\nStraightforward ratio. X = the no of KJ required\n\n572g/432g = xkj/181.6kj\n\nYou'll need to calculate the molecular mass from you periodic table substitute it for the 432 and then refine the equation.\n\nQuestion b) Straightforward ratio. X = the no of KJ required\n\nYou'll need to calculate the molecular mass from you periodic table substitute it for the 432 and then refine the equation.\n\n289/181.6 = xg/432\n\nA mole is the amount of pure substance containing the same number of chemical units as there are atoms in exactly 12 grams of carbon-12 (i.e., 6.023 X 1023). This involves the acceptance of two dictates -- the scale of atomic masses and the magnitude of the gram. Both have been established by international agreement. Formerly, the connotation of "mole" was "gram molecular weight." Current usage tends to apply the term "mole" to an amount containing Avogadro's number of whatever units are being considered. Thus, it is possible to have a mole of atoms, ions, radicals, electrons, or quanta. This usage makes unnecessary such terms as "gram-atom," "gram-formula weight," etc.
897570
Dimensional analysis is easier than it first seems.\n\nFirst you need to know the molecular weight of CO2.\n\nCarbon +2(Oxygen) = 12 + 2(16) = 44 grams per mole\n\n[The above step is not dimensional analysis.]\n\nLet's say somebody asks you how many moles 440 grams of CO2 is.\n\nThis is where we do dimensional analysis.\n\n(1 mole CO2 / 44 grams CO2) * (440 grams CO2 / ? CO2)\n\nThe / sign indicates "divided by", so imagine the parts over each other.  That makes it easier but I cannot do it here in text.\n\nThe first part of the above equation is stating that for every mole of CO2, there are 44 grams of CO2.  The second part says that we have 440 grams of CO2, and want to find out how many moles we have.\n\nThe trick here is to have the terms, one above the other, so that the units cancel out and you end up with the desired unit.  Our desired unit here is the mole - we want to know how many moles are in 440 grams of CO2.  So, that is why in the above, (1 mole CO2) is on top of (44 grams CO2).  If we allow 440 grams to be on top in the next term, then grams cancels out, and moles is the only unit left.  This is what we want.\n\nSo if we solve the above\n\n(1/44)*(440/1) = 440/44 = 10 moles of CO2.\n\nSo, 440 grams of CO2 is the same as 10 moles of CO2.\n\nhope this helps\n\nyay
778176
Use the periodic table of the elements.  The "weights" are in grams per mol.  Just use algebra and solve for the number of mols.  Then you know how many atoms there are by the number of mols which is a definite number.
1134842
a fat molecule triacylglycerol
937928
Iodomethane CH3I has a relative molecular mass of 142 ( C = 12;  +  H3 = 3  +  I  =  127)\nIodomethane is a liquid.\nIt is dense (because of the iodine) 2.28 times heavier than water\nIt has a boiling point of 42C\n\nHalf the volume of calcium hydroxide would be needed because it is dibasic ( has two OH groups)\n\n  Ca(OH)2  +   2HCl  =   CaCl2 +  2H2O     \n  2NaOH  +  2HCl   =  2NaCl +  2H2O  (the reason for all the 2's is to have the same amount of acid in both equations)\n\nThe mass of calcium hydroxide needed to make up a 1 Molar solution is 74g  ( Ca = 40  O = 16 and H = 1)\n\nHowever you wouldn't be able to make a 1 molar solution of calcium hydroxide as it isn't soluble enough!
1104461
Synonyms: Acetic acid ethyl ester; Acetic ether; Acetoxyethane; Ethyl Acetic Ester; Ethyl ethanoate \nCAS No.: 141-78-6 Molecular Weight: 88 Chemical Formula: CH3COOC2H5 \n\nPhysical and Chemical Properties\nAppearance: Clear liquid. \nOdor: Fruity odor. \nSolubility: 1 ml/10ml water @ 25C \nSpecific Gravity: 0.902 @ 20C/4C \npH: No information found. \n% Volatiles by volume @ 21C (70F): 100 \nBoiling Point: 77C (171F) \nMelting Point: -83C (-117F) \nVapor Density (Air=1): 3.0 \nVapor Pressure (mm Hg): 76 @ 20C (68F) \nEvaporation Rate (BuAc=1): 6 \nhttp://acad.udallas.edu/chemdept/hendrickson/MSDS/ethyl_acetate_msd.htm
236093
EDTA has a molecular mass of 292.28 g/mol.
365485
I assume you mean molecular weight.\n\nSince carbon weights 12 grams, and oxygen weighs 16:\n12+(16*2) = 44 grams.\n\nYou have to give the amount of CO^2, in ML to get Moles.\n\nSo generically speaking, 1 mol of CO^2 weighs 44 grams, 2 mol weights 88 grams, and so on.\n\nTo calculate the amount of atoms in it, you would have to times it with Avogadro's number. (6.0221415 × 10)