41.7 grams tin (1 mole Sn/118.7 grams)(6.022 X 10^23/1 mole tin )(1 mole tin atoms/6.022 X 10^23)
= 0.351 moles of tin atoms in pure tin cup
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1.88 mol Zn ( 6.022 X10^23/1mol Zn ) = 1.13 X10^24 atoms.
The atomic mass of B is 10.8Amount of B = mass of pure sample/molar mass = 31.78/10.8 = 2.94mol There are 2.94 moles of the element boron in a 31.78g pure sample.
The formula mass of the compound sulfur dioxide, SO2 is 32.1 + 2(16.0) = 64.1Amount of SO2 = mass of pure sample/molar mass = 37.4/64.1 = 0.583mol There are 0.583 moles of sulfur dioxide in a 37.4g pure sample.
We assume that the quantity 56.22 is in grams. The formula mass of CF2Cl2 is 12.0 + 2(19.0) + 2(35.5) = 121.0Amount of CF2Cl2 = mass of pure sample/molar mass = 56.22/121.0 = 0.465mol There are 0.465 moles of CF2Cl2 in a 56.22 pure sample.
Well, firstly you need to know if it is pure gold. Assuming that it is, convert the grams to moles 19.7g Au x 1molAu/197.0gAu = 0.1moles Au And then, to get the number of atoms in 0.1 moles of gold, multiply it by Avogadro's number, 6.22x10^23 atoms per mole 0.1mol Au x 6.22x10^23atoms/mole = 6.22x10^22
The number of atoms in 1,2 moles of pure aluminum is 7,2265690284.1023.
1.88 mol Zn ( 6.022 X10^23/1mol Zn ) = 1.13 X10^24 atoms.
The atomic mass of B is 10.8Amount of B = mass of pure sample/molar mass = 31.78/10.8 = 2.94mol There are 2.94 moles of the element boron in a 31.78g pure sample.
The atomic mass of carbon, C is 12.0Amount of C = mass of sample/molar mass = 0.170/12.0 = 0.0142mol There are 0.0142 moles of carbon in a 0.170g pure sample.
The formula mass of the compound sulfur dioxide, SO2 is 32.1 + 2(16.0) = 64.1Amount of SO2 = mass of pure sample/molar mass = 37.4/64.1 = 0.583mol There are 0.583 moles of sulfur dioxide in a 37.4g pure sample.
The molecular formula of water is H2O. The atomic mass of H2O is 2(1.0) + 16.0 = 18.0Amount of H2O = mass of pure sample/molar mass = 75/18.0 = 4.17mol There are 4.17 moles of water in a 75 gram pure sample.
We assume that the quantity 56.22 is in grams. The formula mass of CF2Cl2 is 12.0 + 2(19.0) + 2(35.5) = 121.0Amount of CF2Cl2 = mass of pure sample/molar mass = 56.22/121.0 = 0.465mol There are 0.465 moles of CF2Cl2 in a 56.22 pure sample.
The molecular mass of fluorine gas, F2 is 2(19.0) = 38.0Amount of F2 = mass of sample/molar mass = 9.5/38.0 = 0.25mol There are 0.25 moles of fluorine in a 9.5g pure sample.
The atomic mass of the compound C6H8O7 is 6(12.0) + 8(1.0) + 7(16.0) = 192.01000mg is equivalent to 1g. Amount of C6H8O7 = mass of pure sample/molar mass = 1/192.0 = 0.00521mol There are 0.00521 moles of C6H8O7 in a 1000mg pure sample.
Well, firstly you need to know if it is pure gold. Assuming that it is, convert the grams to moles 19.7g Au x 1molAu/197.0gAu = 0.1moles Au And then, to get the number of atoms in 0.1 moles of gold, multiply it by Avogadro's number, 6.22x10^23 atoms per mole 0.1mol Au x 6.22x10^23atoms/mole = 6.22x10^22
You will need to convert to moles, and then atoms. Here is the equation: (5.10 grams over one) times (1 mol S over 32.06 g S) times (6.022 X 10 23 atoms over 1 mol S) the last part of the equation is read six point zero two two times ten to the twenty third.
3.58 X 1024 atoms of uranium (1 mole U/6.022 X 1023) = 5.94 moles uranium to be precise and with significant figures -------------------------------------------------------------------------------