how many hydrogen atoms would weigh one pound?
413959
Well, this is a simple factor labelling problem... I hope you aren't using this to have people do your homework... ;)\n\n1pound x (454 grams/pound) x (1 mol H atoms/1.0079g H atoms) x (6.022x10^23 H atoms/1 mol H atoms) = 2.71 x 10^26 H atoms\n\nnote to PaulB_23: periodic tables are in amu, which is also a ratio of grams per mole, not moles per kg, the 1.008 would just be 1.0079 rounded, I just went w/ a slightly more accurate #
143616
Electrons have a rest mass of 9.109 x 10^-31 kg.  Which means they weigh 8.93 x 10^-30 N, which is about 2.01 x 10^-30 lbs.
656440
The atomic weight is 15.9994, but we generally use the value of 16 for calculations.
797180
Atomic mass depends on the element. It accounts for all isotopes and does a sort of weighted average, depending on how often the isotope occurs in nature.\nMass number depends on the isotope.\n\nFor example, atomic mass of hydrogen is 1.0079. The mass number of most hydrogen atoms is 1. Deuterium is an isotope with a neutron in its nucleus, so its mass number is 2. Tritium is an isotope with two neutrons, so its mass number is 3.
814051
A pound of Ginger weighs one pound,and an ounce of Ginger weighs one ounce,and so on
99693
A pound of butter would weigh more than a pound note (Money)
234819
32...there are 16 ounces in a pound
931678
The density of helium is 0.1786 g/L, and the density of air is 1.2 kg/m^3.  With proper unit conversion, the density difference is 0.064lb/ft^3.  Therefore it takes 15.7 ft^3 of helium to lift one pound.
243768
1 kilogram is equal to 2.2026 Lbs.\n\nFor more weight conversions go to http://www.itinscales.com/weightcalc.htm
457002
That may be right, but the website just says that its 7 X 10^27-it doesnt explain how they figured it..\n\nSo lets see if we can figure how they got that number: There are 6 X 10^23 atoms per mole.  Lets say the average atom (most being hydrogen-1, followed by oxygen-16, and carbon-12) has a molar weight of 7.  So, 6 X 10^23 average atoms in the body would weigh 7 grams.  To get 70 kilograms, we have to multiply that by 10,000.  So, 2000 times 6 X 10^23 gets us about 6 X 10^27.  That's pretty close to 7 X 10^27.  I have a feeling that the real average molar weight per atom would be quite a bit smaller than 7, though.
344087
Straight from the Bureau of Engraving and Printing:\n\nThe approximate weight of a currency note, regardless of denomination is (1) one gram. There are 454 grams in one (1) U.S. pound, therefore, there should be 454 notes in (1) one pound(Avoirdupois system). If the troy system were used, there are (12) twelve ounces in (1) one pound; therefore, if one note weighs approximately (1) one gram, then (1) troy pound contains approximately 375 notes.
1022778
Mg2+ + 2HCl --> MgCl2 + H2 (gas)\n\nOkay, hydrogen.  As you can see in the above equation, for one atom of magnesium you'll produce two atoms of hydrogen.   \n\nLet's work out how much hydrogen you'll get in grams.\nAnd let's say that you have 1 gram of Mg.  First, what you need to do is work out how many atoms are in 1 gram of Mg.  \n\nThis is easy.  Simply:\n\n1 / atomic mass x Avagadro's constant = number of atoms.\n\nFor Mg, this equals:\n\n1 / 24.31 x 6.0221415×10^23 = 0.2477228 x 10^23 atoms.\n\nWe know that for every atom of Mg you'll produce 2 atoms of hydrogen.  So, that means you'll produce:\n\n2 x 0.2477228 x 10^23 = 0.4954456 x 10^23 atoms of hydrogen.\n\nTo work out how much 0.4954456 x 10^23 atoms of hydrogen weighs you just calculate, like this:\n\n0.4954456 / 6.0221415 x 1.008 = 0.0829 grams.\n\nAnd that's it.  1 gram of Mg will produce 0.0829 grams of hydrogen.
230962
i pound = 16 i ounce\n\n16 pound = 256 ounce
990209
1 pound = 0.454 kilograms
710153
Usually psi (pounds per square inch).\n\nAloha
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!
840490
One way to count atoms is by using the molar unit.\nSince different atoms have different weights (masses) the molar quantity of different elements will have different weights.  However, the molar quantity will have the same number of atoms - 6∙02 x 10^23.  This number value is known as Avogadro Constant.\n\nExamples:\n Hydrogen: 1 mole = 1g and contains 6∙02 x 10^23 atoms.\n Oxygen : 1 mole = 16g and contains 6∙02 x 10^23 atoms.\n Water :  1 mole = 18g and contains 6∙02 x 10^23 molecules.