What is the esiest way to find the mass of a molecule?
924159
It depends on what you have, if you know the mole of the molecule, you can determine the mass by converting molar mass (g/mol) into mass (g). The mole of the molecule can be found on the periodic table, but first you need to know the molecule formula of the compound. Then add it up.
697475
1) determine the mass of carbon, hydrogen and oxygen.\ncarbon: 7.849 g x (12 / 44) = 2.141 g\nhydrogen: 3.213 g x (2 / 18) = 0.357 g\noxygen: 3.215 - 2.141 - .357 = 0.717 g\n\n2) convert to moles.\ncarbon: 2.141 / 12 = 0.178 mol\nhydrogen: 0.357 / 1 = 0.357 mol\noxygen: 0.717 / 16 = 0.0448 mol\n\n3) divide each molar amount by the lowest value to obtain small integers\ncarbon: 0.178 / 0.0448 = 4\nhydrogen: 0.357  / 0.0448 = 8\noxygen: 0.0448 / 0.0448 = 1\n\nThe empirical formula of the substance is (C4H8O)n\nThe atomic masses add up to 72, which is also the molar mass of the compound. Therefore n=1 and we find C4H8O
843034
1. Modify the ideal gas equation such that molecular mass (MW)and weight of gas appear.\nIdeal gas equation: PV = nRT\nsince n (moles) = weight / MW = g/MW\nso, your equation will become PV = gRT/MW\nGiven your values, you will end up:\nMW = gRT/ PV\n\n2. Plug in the values:\n\nMW = 3.06g * 0.08206 L-atm/mol-K * (51.4 + 273 K) / 0.970atm * 1.00L\nMW = 83.98 g/mol\n- this is the molecular mass of your gas.\n\n3. Determine the molecular formula of the gas.\n-since you have 14.37% H, your C is 85.63%\n-assume 100g gas so that you'll have 14.37g H and 85.63g C\n-get the number of moles:\nH: 14.37g / 1g/mol = 14.37 mol H\nC: 85.63g / 12g/mol = 7.13 mol C\n\n- get the mole ratio: that is, 1 mol C is to 2 mol H.\n- determine your multiplier such that MW result will be approximately 83.98g/mol. In this case, its 6. \n\nSo, your molecular formula is C6H12.\n\nTo check,\n\nC: 6 * 12g/mol = 72g/mol\nH: 12 * 1g/mol = 12g/mol\ntotal: 84g/mol ~ 83.98g/mol
994333
Molar mass is the weight of a compound at a constant number of molecules.\n\nWhere are many uses in which it would be usefull, but for a non-chemist it would be meaningless. \n\nTher are numberous example I could give you where it would be usefull but all of these relate to chemisty. I will therefore make on up.\n\nSay someone wanted to destory a compound that was dangerous but that the agent to use was expensive or could not be keep for more than 24 hours. The compound that was to be destoried reacted on a 1 mole to 1 mole ratio. It is known that the compound we want to get rid off had a molar mass of 32 g/mol\nand there was 16 grams of the compound. So using the weight and molecular mass we can work out that the number of moles we have is 0.5. OK now nowing that our agent reacts on a ratio of 1:1 we need 0.5 moles of our agent. But our agent has a molecular mass of 64 g/mol, so the weight we need to use is 0.5 moles x 64 g/mol = 32 grams.
569202
Scientists use it today to calculate the amount of a substance, number of particles, that they have.  The molecular mass of something times the number of moles of the substance equals the mass in grams of the substance.  For example 1 mol of H2O equals 18g, and equals 6.02810^23 particles of water.
739949
For every molecule of H2SO4 there are 2 Hydrogen(H) atoms, 1 Sulfur(S) atom, and 4 Oxygen(O) atoms. So if there are 9.5 x 10^22 molecules of H2SO4 then are are also that number of sulfur molecules present.\n\nTo find how many grams 9.5 x 10^22 molecules weighs, use Avogadro's number. Dividing by Avogadro's number will tell you how many moles of Sulfur you have, and from that you can use the atomic mass of Sulfur to determine how many grams there are:\n\nAvogradro's number = 6.02 x 10^23\n\n(9.5 x 10^22) / (6.02 x 10^23) = 0.158 moles\n\nAtomic mass of Sulfur = 32.065 g/mol\n\nMultiply this by the number of moles of Sulfur you have to obtain the number of grams of Sulfur:\n\n32.065 * 0.158 = 5.067 g\n\nI hope this helps!
856873
The balanced chemical equation and the molecular weights of the reactants and products.\n\nIn simplest form, assume\n\nXY + AB = XB + AY.\n\nAssume the molecular weight of XY is 50, and of XB 35.\n\nFor every 50 grams (or pounds, tons, or any other measure of mass) of XY you use, you will get 35 grams (or whatever) of XB.\n\nEDIT:\n\nOK. Atomic weights are H=1, S=32, Cl=35.5, Fe=56. Molecular weights are FeS=88, HCl=36.5, H2S=34, FeCl2=127.One gram molecular weight of each is its molecular weight in grams. So if you react 88 grams of FeS with 36.5 x 2 grams of HCl (the balanced equation tells you that you need 2 moles of HCl, so you multiply by 2), you will get 34 grams of H2S and 127 grams of FeCl2. \n\nNotice that the weights balance. You put in 88 + (36.5 X 2) grams, or 161 grams. You got out 127 + 34, or 161 grams.\n\nYou need the mass of any one of those compounds - either reactant or product - to determine all the others. Calculate the moles of the one for which you have the mass, determine the ratio of the moles of that one to the others, multiply by that ratio and then multiply result by molecular weight.
578713
U can a measure the mass of an object accurately using a Physical Balance.\nUnit of mass is kg in SI unit ysstem.\nMore accurate ways of measuring mass is done now.\n\nU can calculate it's weight by a formulae:\nW=mg.\nW-Wieght\nm-mass\ng-aceleration due to gravity (9.8 ms^-2)
1067776
You get the molecular, or formula, weight from the periodic table.  Add the atomic weights for Na and Cl.
609831
pv=nrt\nmeasure pressure, volume, and temperature to find the number of moles, n\n\nfind the mass of the gas\n\nmass of gas/ moles of gas= molecular mass (g/mol)
944140
when you are doing conversions from moles to grams and so forth, you'll always use the molar mass (g/mol)\n\nCH3I = 141.94 g/mol ( just add up the molecular weights for each mol of each element)\n\n1.00g (1 mol/141.94 g) ..... just make grams cancel out so you'll have moles....works for every conversion...make sure your units cancel out and what u want is left on top.
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.
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
95148
Actually, the mass of a proton is 1.00727664669 atomic mass units.\n\nAn atomic mass unit is defined such that Carbon 12 is exactly 12.  The carbon atom weighs less than 12 times the proton (because of nuclear binding energy).
834362
1) determine the mass of carbon, hydrogen and oxygen.\ncarbon: 4.203 g x (12 / 44) = 1.146 g\nhydrogen: 3.441 g x (2 / 18) = 0.382 g\noxygen: 3.060 - 1.569 - .262 = 1.532 g\n\n2) convert to moles.\ncarbon: 1.146 / 12 = 0.0955 mol\nhydrogen: 0.382 / 1 = 0.382 mol\noxygen: 1.532 / 16 = 0.0958 mol\n\n3) divide each molar amount by the lowest value to obtain small integers\ncarbon: 0.0955 / 0.0955 = 1\nhydrogen: 0.382 / 0.0955  = 4\noxygen: 0.0957 / 0.0955 = 1\n\nThe empirical formula of the substance is (CH4O)n\nThe atomic masses add up to 32, which is also the molar mass of the compound. Therefore n=1 and we find CH4O.
754188
you divide the mass by the volume\n1.2.14 g/cm^3\n2..82 g/cm^3\ngood luck!
995159
Use the atomic weights of the individual elements, and add them together.  For instance, if I had water, H2O:\n\nH - 1.01 g * 2 = 2.02 g\nO - 16.00 g\n\nSo the molar mass of H2O would be 18.02 g/mol.\n\nIf I wanted to convert from grams to moles, I would divide the grams by the molar mass.  Grams cancels out to be left with moles.\n\nIf I wanted to convert from moles to grams, I would multiply the moles times the molar mass.  Moles would then cancel out to be left with grams.