what mass of sulfur must be used to produce 12.6.1L of gases sulfur dioxide at ST..?
105753
First you must find the number of moles of 12.6 Liters of SO2 gas at STP.\n\nAt STP an ideal gas (we will assume SO2 is an ideal gas) has a volume of 22.4 Liters.\nSo how many moles would be in 12.6 Liters?\n\nAfter you obtain the number of moles of SO2, then figure out how many moles of Sulfur there are in 1 mole of SO2.\nFor every 1 molecule of SO2, there is 1 Sulfur atom, so for every 1 mole SO2, there is 1 mole of Sulfur.  Knowing this, you can calculate the number of moles of Sulfur needed.\n\nBy multiplying tbe number of moles of Sulfur needed by the molar mass of Sulfur (32.07 g/mol) you can find the mass of the Sulfur required.
765234
1. To find the mass, first you need to find the atomic mass of each atom in the molecule. So:\nFe = 55.84 * 2 = 111.68\nS = 32.07\nO = 16 * 4 = 64\nand the (SO4) unit has 32.07 + 64 = 96.07\nSince there are three SO4 units in the molecule, thats 96.07 * 3 = 288.21 ; and adding the Fe, that's a total of 399.89 atomic mass units in the whole molecule.\n\nThat means that one mole of this molecule weighs 399.89 grams.\n\n2. Similar procedure: first add up the atomic masses of each atom in the molecule. \nC = 12.01 * 6 = 72.06\nH = 1.008 * 12 = 12.096\nO = 16 * 6 = 96\nfor a total of 180.156 atomic mass units in the whole molecule. That means that 180.156 grams would be exacly one mole, and we want to know how many moles in exactly 180 grams. So the answer is just a bit less than one mole, or 180 / 180.156, or .999134 moles.
14607
Sulfur - (300 K) (amorphous) 0.205 W/(m·K)\nhttp://en.wikipedia.org/wiki/Sulfur\nGlycerol - (20 C) 0.29 W/(m·K)\nhttp://www.hukseflux.com/thermal%20conductivity/thermal.htm
843713
You need to first balance this equation:\n\nCH4 + 2O2 ---> CO2 + 2H2O\n\n# of mole of 80.2 g CH4 = 80.2 / (12 + 4) = 5.01 moles\n\n# of moles of O2 needed = 5.01 * 2 = 10.03 moles\n\nTotal mass of O2 = 10.03 * (16 * 2) = 320.8 g
295876
See the reference below for a more complete description.\n\nHowever, consider a factory which emits sulfur dioxide\nwhich then mixes with water in the air:\n\nS02 + H20 ==> H2SO3      (the numbers should be subscripts)\n\nMy understanding is that with one more interaction with\nwater, it creates sulfuric acid and hydrogen:\n\nH2S03 + H20 ==> H2SO4 + H2\n\nThus, you have acid in the air which is carried down\nwith rain to be acid rain.
644831
The fast way to do this is to know that there are 22.4 liters per mole at STP for a gas.  The long answer is to use a gas law like the ideal gas law.  You should know from your class what gas law to use, but the ideal gas law is\n\nPV = nRT\n\nWhere \n  P = Pressure (1 atm at STP)\n  V = Volume (45 Liters)\n  n = number of moles\n  R = gas constant\n  T = temperature (298 deg C at STP)
289562
First of all, it's spelled stoichiometry.\nSTP=22.4L per mole\nmethane = CH4\nmolar mass of methane = 4*1.0079(mass of 4H) + 12.011(mass of C)=16.0426gCH4\n\nSo it would be like this\n3.35L / 22.4L * 16.042g = 2.39923g methane\n\nWith significant figures, it would be 2.40g methane
774536
Ultra low sulfur diesel has 15 ppm of sulfur. Normally the bitumen and diesel product, the hydrotreated diesel, is transformed by a fairly complicated process to produce low sulfur diesel fuel. The amount of coke in this fuel is not found in the ULSD fuel.
215604
C6H12O6(s) ---H2SO4--> 6C(s) + 6H2O(in H2SO4 solu.) + Heat
1053372
3.425 BTU/lb F in gas form
26549
sulfur dioxide\nsulfur dioxide\ncoffe shop owner
593588
atomic mass of S = 32.07, 64 grams of S = 64/32.07 ~= 2 moles\natomic mass of Be = 9.01, 20 grams of Be = 20/9.01 ~= 2.2 moles\natomic mass of Na = 22.99, 25 grams of Na = 25/22.99 ~= 1.1 moles.\n\nThe Na sample has the fewest atoms, followed by K, then S, then Be.
1029447
sulfuric acid is h2so4. convert 1600 kg to g so times by 1000. then take that number in grams and times by the molar mass of of sulfur (gSx1mol S/gS) then convert to moles of H2SO4 by using your balanced chemical equation(coefficients), with moles of S on bottom, moles of H2SO4 on top. everything cancels and your left with moles of sulfuric acid that you could make. if you need to take it another step to grams then you would then just use the molar mass of sulfuric acid.
952814
That would be correct if you were looking for the total mass of oxygen but you're not.  You're looking for sulfur.  You know the molecular weight of sulfur and you know the number of moles you need.  I'm not going to do it for you.
545660
Remember that in the case of the Sulfure or the Oxygen, you have to complete the amount of 8 electrones each, if you only leave single bond that will mean that the oxygens would only be using 6 out of 8 electrones, leaving the molecule extreamly unstable.
57069
Balancing we get, S8 + 4Cl2 ---> 4S2Cl2\n\nNo. of Moles = Weight/Molecular Mass \nThus, Moles of sulfur   = 56.68/(8 x 32) = 0.22\n      Moles of chlorine = 97.05/(2*35.5) = 1.37\n\nWe know 1 mole of sulfur requires 4 moles of Chlorine (Cl2)\nTherefore 0.22 moles sulfur will require 0.88 moles of Cl2\nThus sulphur being in limited amount will decide the amount of product formed i.e. it is limiting reagent.\n\nSince 1 mole sulfur produces 4 mole S2Cl2 thus 0.22 moles sulfur will produce 0.88 moles S2Cl2. Therefore weight of S2Cl2 produced is = moles x Molecular mass (S2Cl2)\n                  = 0.88 x (2*32(S2) + 2*35.5(Cl2))\n                  = 0.88 x 134\n                  = 117.92 gm
876129
The Claus process is catalytic reaction of hydrogen sulfide with sulfur dioxide to give elemental sulfur.\n2H2S + SO2 ===> 3S + 2H2O\nSome of the H2S is oxidized in air to SO2. The elemental sulfur is isolated in pure form. This makes it suitable for re-oxidation to SO2, further catalytic oxidation to SO3, and passage through the contact process to make pure, concentrated H2SO4. Amine sweetening refers to reaction of H2S innatural gas with amines, R3N, to give ammonium sulfides, 2R3NH+ + S=