0.285 mol.
The solution to this problem can be found through what is called dimensional analysis.
The first thing that needs to be identified is the atomic weight (or molar mass) of SiO2. This can be found in any chemistry text book (particularly the Periodic Table) or even a quick online search (I like to use wikipedia). While it is possible to find the specific atomic weight of the molecule SiO2, I find it simpler just to look up the atomic weights of the individual atoms in the molecule. Starting with silicon (Si), the atomic weight is 28.0855 g/mol. Oxygen (O) has the atomic weight of 15.9994 g/mol. Now, all one needs to do is add up the atomic weights of all the individual atoms to find the total atomic weight of the molecule. For SiO2, this would be 28.0855 g/mol + 15.9994 g/mol + 15.9994 g/mol (since there are 2 oxygen atoms). Notice also that I included the units. In dimensional analysis, it is very important to keep track of units.
This gives you a total of 60.0843 g/mol. Now we have identified the molar mass of the molecule SiO2. The units of the molar mass is g/mol, and we want to find how many moles (mol) are found in a certain mass (g) of SiO2. Now the dimensional analysis really comes into play.
Start with the values that are given in the question: 17.1 g SiO2. We can now convert this number to mols using the molar mass we identified previously: 60.0843 g/mol SiO2. Put into equation form:
17.1g SiO2 | 1 mol SiO2 _ or (17.1 g SiO2 x 1 mol SiO2)/60.0843 g SiO2
¯¯¯¯¯¯¯¯¯|60.0843 g SiO2
With this arrangement, we can see that the units of "g SiO2" will cancel out, and you will be left with "mol SiO2", which is exactly what you are trying to find! And the answer is: 0.285 mol.
The Atomic Mass of silicon dioxide, SiO2 is 28.1 + 2(16.0) = 60.1Amount of SiO2 = mass of pure sample/molar mass = 11/60.1 = 0.183mol
There are 0.183 moles of SiO2 in a 11 gram pure sample.
Do you mean the type of Mole that digs up your garden? If this is yes then you have an infestation.
.159 mol times 60.1 grams= 9.5559 grams
The answer is 0,203 moles.
91.224
Not many! 5.0 grams CaBr2 (1 mole/199.88 grams CaBr2) = 0.025 moles CaBr2
The mass of o,5 mole of uranium is 119,014455 g.
One mole is 6.02 × 1023 of anything. One mole of atoms is 6.02 × 1023 atoms, one mole of rice is 6.02 × 1023 grains, one mole of shoes is 6.02 × 1023 shoes.So you take 12 and multiply it with 6.02 × 1023 to get 7.22 × 1024
Multiple the moles of K2SO4 by the molecular weight of 174.2592 grams. That should equal 210.85 grams.
This is a complex tetrahedral formula, but SiO2 is the accepted formula for our purposes. I assume you mean 1.40 grams quartz. 1.40 grams SiO2 (1 mole SiO2/60.09 grams)(2 mole O/1 mole SiO2)(6.022 X 10^23/1 mole O) = 2.81 X 10^22 atoms of oxygen ( may need the tetrahedral formulation. In this form the O2 is shared and the form is SiO4. So, same ratios, different numbers. SiO2 is standard though )
10.00 X 10^28 = 1.0 X 1^29 ( always use scientific notation in chemistry ) 1.0 X 10^29 molecules silicon dioxide (1 mole SiO2/6.022 X 10^23)(2 mole O/1 mole SiO2)(16.0 grams/ 1 mole O) = 5.3 X 10^6 grams of oxygen
Ans:Quartz is SiO2. It has a formula weight of 60.1 g/mol. 3 grams of SiO2 is 0.05 moles.Each mole of SiO2 has 0.1 moles of oxygen since there are 2 oxygen atoms per formula unit of SiO2.(1 mole of anything is 6.02x1023 of anything.)0.1 mol oxygen atoms x 6.02x1023 oxygen atoms / mol oxygen atoms= 6.02 x 1022 oxygen atoms.Number of O atoms =6.02×1022
3.10 moles SiO2 (1 mole Si/1 mole SiO2)(6.022 X 1023/1 mole Si) = 1.87 X 1024 atoms of silicon =====================
4.003 grams
Na2SO4 10.0 grams Na2SO4 (1 mole Na2SO4/142.05 grams)(2 mole Na/1 mole Na2SO4)(22.99 grams/1 mole Na) = 3.24 grams of sodium -------------------------------
how many grams are in a mole of soda cans? show work
The answer is 165,23 grams.
72 grams
25 grams / (17 grams/mole) x 6.022x1023 molecules/mole = 8.9x1023 molecules
36 grams
Approx 658 grams.