121.760
Very close to 11.0g/cm³. 5% antimonial lead is 10.92g/cm³ and 10% antimonial lead 10.50g/cm³.
6.61 - 6.72, Average = 6.66
6.61
There are two formulas, one containing 71.5 parts of tin to 27.8 of lead, the other 78.2 of tin to 21.7 of lead. I work with Pewter in hard Tech/ Metal works, Unleaded Pewter is made of Tin(soft metal) Copper(used in many alloys) and Antimony(metalloid). Pewter is made of the materials above
We assume 100 grams of the compound and turn those percentages into grams and get the moles. 50.7 grams antimony (1 mole Sb/121.8 gram) = 0.41626 moles antimony ================================ Now, the smallest mole number (antimony) becomes 1 and the other number is divided by it(antimony) to get the empirical numbers. 0.62467 moles Se/0.41626 moles Sb = 1.5 ----------------so, this happens sometimes and this is what we do (SbSe1.5)*2 = Sb2Se3 -----------------The empirical formula Antimony selenide
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36 + 2 + 10 + 3 = 51 electrons = 51 protons = Antimony (Sb)
The density of 2-methylpropane is 2,52 g/L.
There are two formulas, one containing 71.5 parts of tin to 27.8 of lead, the other 78.2 of tin to 21.7 of lead. I work with Pewter in hard Tech/ Metal works, Unleaded Pewter is made of Tin(soft metal) Copper(used in many alloys) and Antimony(metalloid). Pewter is made of the materials above
We assume 100 grams of the compound and turn those percentages into grams and get the moles. 50.7 grams antimony (1 mole Sb/121.8 gram) = 0.41626 moles antimony ================================ Now, the smallest mole number (antimony) becomes 1 and the other number is divided by it(antimony) to get the empirical numbers. 0.62467 moles Se/0.41626 moles Sb = 1.5 ----------------so, this happens sometimes and this is what we do (SbSe1.5)*2 = Sb2Se3 -----------------The empirical formula Antimony selenide
The density of lead is 11.34 g/cc Therefore the volume of 2 g of lead will be 2/11.34 = 0.1764 cc
The atomic mass of an element is the weighted average of the masses of its isotopes. You know that: Antimony-121 has a mass of 120.9038 u, x% abundance Antimony-123 has a mass of 122.9042 u, y% abundance There are only 2 isotopes for antimony and their percent abundances should add up to 100%. In other words: x% + y% = 100% y = 1-x (percentages written as decimals) So, now let's put everything together. In order to calculate the atomic mass, multiply the percent abundance of an isotope by its atomic mass; then add the product of all the isotopes: (Atomic Mass of Antimony-121)(Percent Abundance of Antimony-121) + (Atomic Mass of Antimony-123)(Percent Abundance of Antimony-123) = Atomic Mass of Element Antimony (120.9038 amu)(x) + (122.9042 amu)(y) = 121.760 amu Replacing 1-x for y gives: (120.9038 amu)(x) + (122.9042 amu)(1-x) = 121.760 amu Solve for x: 120.9038x + 122.9042 -122.9042x = 121.760 amu -2.0040x = -1.1442 x = 0.57096 = 57.096% Solve for y: y = 1 - x y = 1 - 0.57096 = 0.42904 = 42.904%
1 cup of 2% milk has about 5 grams of fat on average.
Sn+3 S-2 <--- these are the ions and their charges Sn+3 Sn+3 S-2 S-2 S-2 <--- the charges have to add up to zero, so two +3 antimony ions cancel out three -2 sulfur ions Sn2S3 <--- simplify Note that Antimony III sulfide is also called stibnite or antimonite
2
Lead and zinc account for 2 and 3 percent of U.S. nonferrous metals production, respectively.
First find the volume, then multiply by the density of lead. Density of lead = 0.41 pounds per cubic inch.Volume = (area of base) * (length) = (pi * r2) * (length) = 3.14 * (0.75 in / 2)2 * (3 in) = 1.32 in3. Then (0.41 lb / in3) * (1.32 in3) = 0.54 pounds, or 8.6 ounces
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36 + 2 + 10 + 3 = 51 electrons = 51 protons = Antimony (Sb)
Lead has atomic number 82, if it loses 2 protons and 2 neutrons (ie an alpha particle) it becomes mercury with atomic number 80. Only lead-204 (1.4 percent of natural lead) and lead-210 (trace only) appear to do this, and 204 has such a long half life that it is regarded as stable, so your postulated reaction does not seem to be typical of lead as a whole.