L>mmsanotherstage2019.com: typical Mass of One MoleculeMole ConversionsCalculating the typical Mass the One Molecule as soon as calculating the typical mass the one molecule, execute the following:Calculate the molar mass of the substanceDivide the by Avogadro"s NumberBy the way, the an approach to calculate the typical mass that one atom of an element is exactly the same as for calculating the mean mass of one molecule the a compound.Also, note that I save using the word "average." since each facet in a compound has actually several isotopes, a mole of a link (say H2O) is created of molecules of slightly different weights. For example, hydrogen has actually two stable isotopes while oxygen has three. This leader to ripe different feasible combinations the isotopes.Since there is no practical way to different out all the different weights, what us wind up measuring is the average weight of one molecule, which means that no one, solitary molecule has the weight calculated. (That particular fact often gets tested.)Example #1: What is the average mass of one molecule of H2O?1) calculation the molar mass.

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You space watching: What is the typical mass of a single silicon atom in gramsThe molar mass of water is 18.015 g/mol. This to be calculated by multiply the atomic weight of hydrogen (1.008) by two and including the result to the weight for one oxygen (15.999).Please remember that you need the molar mass first when make the efforts to uncover the median mass of one molecule.2) division the substance"s molar fixed by Avogadro"s Number.18.015 g/mol–––––––––––––––=2.992 x 10¯23 g6.022 x 1023 mol¯1
3) keep in mind that the last answer has actually been rounded to four significant figures (from 2.9915 - note use of round off with five rule). Also, keep in mind that the unit that mole cancels.Example #2:
calculate the mean mass (in grams) the one molecule the CH3COOH (molar fixed = 60.0516 g/mol)molar mass ---> 60.0516 g/mol–––––––––––––––=9.972 x 10¯23 gAvogadro"s Number --->6.022 x 1023 mol¯1
Example #3:
identify the mean mass in grams for one atom of gold (molar mass = 196.666 g/mol).196.666 g/mol–––––––––––––––=3.266 x 10¯23 g6.022 x 1023 mol¯1
By the way, one older surname for the molar mass of an element is gram-atomic weight. Um, er, it"s the one the mmsanotherstage2019.com learned way back when he was just a sprout.Example #4:
recognize the fixed (in grams) of one atom the gold-198.Note that this inquiry asks around one particular isotope. Because that that, us must find the gram-atomic load for the one isotope (often called the isotopic mass), no the molar fixed (also referred to as the typical atomic weight) because that gold (the worth we supplied in instance #3). Wikipedia has actually a table listing the masses for every the isotope of gold.The value for gold-198 is 197.968 g/mol. The problem set up is:197.968 g/mol–––––––––––––––=3.287 x 10¯23 g6.022 x 1023 mol¯1
Note that this is not an average. It is the actual mass of every gold-198 atom.Example #5:
calculate the massive of a solitary atom of silver:Silver has actually two steady isotopes, for this reason its molar mass is a weighted average of those two values. That method that what is calculate in the video is actually the average mass of a solitary atom of silver.You should be mindful of this because you may have an instructor the emphasizes the average element of the calculation while others may disregard it completely.Example #6: identify the mass of 125 atoms of palladium.Solution:Done in dimensional analysis style.106.42 g1 mol125 atoms–––––––x–––––––––––––––x––––––––=2.21 x 10¯20 g1 mol6.022 x 1023 atoms1
Example #7:
recognize the massive of one molecule of U235F6.

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See more: Tap that Ass: What walk It median To Tap the Ass: What Is It? What Does that Mean?Solution:1) note that the fixed of a certain isotope is required. Because that that, us go to the Internet and look the up:235.0439 g/mol2) over there is one an ext unusual facet to this problem:Only one stable isotope the fluorine is existing in nature. In other words, 100% of every fluorine atoms in nature sweet the very same amount:18.9984 g/molBy the way, the longest-lived stormy isotope of fluorine has a half-life that is a bit much less than 110 minutes. In a chemical sense, the ain"t existing in nature!3) calculate the molar fixed of U235F6:349.0343 g/mol4) calculation the actual massive of one molecule the U235F6:349.0343 g/mol / 6.022 x 1023 molecules/mol = 5.796 x 10¯22 5) Why would certainly I to speak actual mass fairly than average mass? This is due to the fact that fluorine has actually only one isotope in nature and also uranium (which has two isotope in nature) is limited to just one specific isotope.Example #8: deserve to you swim in a exchange rate billion (1.00 x 1018) molecule of water?Solution:The best way to recognize if you deserve to swim in this lot of water is to determine the mass of water present. I"ll do it dimensional analysis style.1 mol18.015 g1.00 x 1018 moleculesx–––––––––––––––––––x––––––––=0.0000299 g6.022 x 1023 molecules1 mol
No, girlfriend can"t swim in that amount of water.I decided to look into just how much water vapor is in an median breath. Assume 500 mL because that a breath. I think 5% water vapor by volume. That means 25 mL that water vapor. I think room temperature and also pressure. Usage PV = nRT:(1.00 atm) (0.025 L) = (n) (0.08206 l atm / mol K) (293 K)n = 0.00103978 mol(0.00103978 mol) (18.015 g/mol) = 0.0187 gExample #9:
How countless water molecules would certainly be compelled to create one drop (0.010 g)?Solution:1) determine average fixed of one molecule the water:18.015 g/mol / 6.022 x 1023 molecules/mol = 2.99153 x 10¯23 g/molecule2) Determine variety of molecules in one fall of water:0.010 g / 2.99153 x 10¯23 g/molecule = 3.3 x 1020 molecules (to two sig figs)3) Here"s an additional approach, set up in dimensional evaluation style:1 mol6.022 x 1023 molecules0.010 gx–––––––x––––––––––––––––––––=3.3 x 1020 molecule (to 2 sig figs)18.015 g1 mol
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