The number of grams of sulfur containing the same number of atoms as 5.00 moles of oxygen atoms is...?
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.
1019766
sulphur exhibits valencies of 2 , 4 or 6 depending upon the conditions of reaction...it exhibits +4 oxidation state in SO2,+6 in SO3,H2SO4 and so on+2 in S2Cl2...is tthat enough...
774704
S + O2 --> SO2\n\nmole of S needed to be converted = 5.00 / 32 = 0.15 mole\nmole of O2 = 0.15 mole\nBy using ideal gas theory:\nP * V = n * R * T\n5.15 * V = 0.15 * 0.082 * 310\nV = 0.74 litre\n\npeace\nvixklen
1027887
Compounds are composed of two or more elements.\nElemental molecules are like the diatomic gases:\nF2, O2, N2, Cl2: composed of a single element.\nor the allotropes of sulfur :\n``Sulfur in the solid state ordinarily exists as cyclic crown-shaped S8 molecules. Sulfur has many allotropes besides S8. Removing one atom from the crown gives S7, which is responsible for sulfur's distinctive yellow color. Many other rings have been prepared, including S12 and S18. By contrast, its lighter neighbor oxygen only exists in two states of chemical significance: O2 and O3. Selenium, the heavier analogue of sulfur can form rings but is more often found as a polymer chain.´´
771710
eight, an element forms a compound with another element to achieve a full outer shell of electrons, in the case of sulphur, its outer shell is full with eight electrons, it achives this by sharing electrons with oxygen atoms
518927
(46.2 grams)/(32 grams per mole) = 1.44 moles of Oxygen (O2)
810256
With percent, always assume a 100g sample.\n\n21.96% S = 21.96gS\n78.04% F = 78.04gF\n\nConvert grams to moles using molar mass\n\n21.96gS * 1molS/32.06gS = .685 mol S\n78.04gF * 1molF/19.00gF = 4.12 mol F\n\nTake the smallest answer and divide the other by that.  In this case, we'll use .685 mol S.\n\n.685 mol S/.685 = 1 moles S\n4.12 mol F/.685 = 6.01 moles F\n\nNow, just write it out!\nYour empirical formula would be SF6.
833745
first you have to balance the equation:\n2SO2+O2=2SO3\n\n1) 96gO2*(1moleO2/32g O2)= 3mole O2\n2) 3mole O2*(2moles SO3/1mole O2)=6mole SO3\n3) 6moles SO3*(80.1g SO3/1mole SO3)=480g SO3
782235
Avagardro's Number = one mole, and all of the masses on the periodic table are in grams/mole.One mole of P equals 30.97g, so d. (c is the only other logical answer, but O2 has a molar mass of 32g/mole beacuse 1 oxygen has a molar mass of 16)\n\nGet used to moles, you'll see them all throughout chemistry.
802786
I'll show you how to do one; then you'll know how to do the rest:\n\na. On the periodic table, find the atomic weight for both Fe and O.\nFe = 55.845, O = 15.9994\nMultiply by the number of atoms of each in each molecule of Fe2O3 to get the molecular mass (the mass, in grams, of one mole of the compound) of Fe2O3:\n2(55.845) + 3(15.9994) = 159.6882\nDivide 150 by this number to get the number of moles:\n150/159.6882 = 0.939 moles
566520
Fe(s)+H2SO4(aq)excess--> Fe2+(aq) + SO42-(aq)+H2(g)\n\nratio is 1:1\n\n5gFe/55.85g/molFe= .090mol\n\nand\n\n1 molar solution =1 mole per liter\n\nso,\n\n.09mol(1 liter/1mol)= .09L or 90mls
703295
A mole of ANYTHING contains Avogadro's number of particles, which is 6.02x10^23 of them.  So if 1 mol of gold =6.02x10^23, then 3.21 mol of gold will have: 3.21mol x (6.022x10^23 atoms/mol)=...atoms of gold
247406
hope this helps...\n\nZinc sulfide\n\nMolecular Formula: ZnS \n\nMolecular Weight: 97.5 g/mol
450501
Sorry this is a brief response: figure out the moles of gas in the reactants side of the equation. 5 moles of oxygen means there are 5 moles of gas. Then use Ideal gas law:\n\nPV = nRT\n\nSo, you know Volume (1500 mL), n (5 moles x molecules of O2 per mole), and T (25C + 273C = 298 K). Calculate P.\n\nFor n:\n5 moles (6.022x10^23atoms/moles) (2 atoms/molecule)\n\nHope that helps....
47119
One gram of Fe = .450 mole\n\nMultiply that by Avogadro's number :\n0.450 mol x 6.022E -1023 \nWill yield the number of atoms in ONE GRAM...\nMultiply that number by your desired number of grams will give you your answer...
179528
1 mole of a substance means 6.023 x 10^23 molecules..so thr will be 6.023 x 10^23 no of carbon disulphide molecules. now each CS2 molecule has one carbon and 2 sulphur atoms  .so there will be 6.023 x 10^23 atoms of carbon and 2 x 6.023 x 10^23 sulphur atoms
96063
It's AvOgadro :-)\nThe number is 6.0221415...x10exp23 (that is, followed by 23 zeroes).\nThis valuable number represents the number of atoms, molecules, etc. in a gram mole of any chemical substance.\nAvogadro (he had a really long name) proposed in 1811 that equal volumes of gases, at the same temperature and pressure, contain equal numbers of molecules. More about this story in the second link.