One mole of CH2F2 has a mass of (12.011)+2(1.0079)+2(18.9984) g = 52.0236 g
19 g of CH2F2 is equivalent to 19/52.0236 moles = 0.3652 moles
For every mole of CH2F2 there are 2 F atoms, and 1 mole of a substance has 6.022 x 10^23 entities.
So 19 g of CH2F2 has 2(0.3652)(6.022 x 10^23) F atoms = 4.40 x 10^23 F atoms.
1 mole of any element is its atomic weight (from the periodic table) in grams.1 mole of atoms of an element is 6.022 x 1023 atoms (Avogadro's number).1 mole F = 18.9984032g F1 mole F = 6.022 x 1023 atoms FConvert atoms of F to moles F.3.011 x 1023 atoms F x (1mole F/6.022 x 1023 atoms F) = 0.5000 mole FConvert moles F to g F.0.5000 mole F x (18.9984032g F/1mole F) = 9.499g Fe
There are 1.93 moles in 1.16 x 10^23 fluorine atoms. This calculation is done by dividing the number of atoms by Avogadro's number (6.022 x 10^23 atoms/mol).
2
2 atoms of S + 10 atoms of F = 12 atoms total
Since the volume of an atom is determined by the radius of its electron cloud, we can use the atomic radius to approximate the volume each atom occupies. The atomic radius of Cs is larger than that of F, so more F atoms would be needed to occupy the same volume as one Cs atom. Approximately 9 F atoms are needed to occupy the same volume as one Cs atom.
The Lewis structure of CH2F2 is represented as H-C-H with a double bond to C and a single bond to F on each side of the C atom. This arrangement allows each atom to have a full valence shell and minimizes formal charges.
To find the number of moles in 1.01e23 fluorine atoms, divide the given number of atoms by Avogadro's number, which is approximately 6.022e23. So, 1.01e23 F atoms / 6.022e23 atoms/mol ≈ 0.168 moles of F atoms.
1 mole F = 6.022 x 1023 atoms F 2.5mol F x 6.022 x 1023 atoms F/1mol F = 1.5 x 1024 atoms F
Carbon is the middle atom, there are no double bonds you just add the 4 other atoms around it in a tetrahedral structure (if you haven't done this yet don't worry about it) .. :H: .. l .. :F-C-F: '' l '' :H: '' hope that works out :S
1 mole of any element is its atomic weight (from the periodic table) in grams.1 mole of atoms of an element is 6.022 x 1023 atoms (Avogadro's number).1 mole F = 18.9984032g F1 mole F = 6.022 x 1023 atoms FConvert atoms of F to moles F.3.011 x 1023 atoms F x (1mole F/6.022 x 1023 atoms F) = 0.5000 mole FConvert moles F to g F.0.5000 mole F x (18.9984032g F/1mole F) = 9.499g Fe
There are 1.93 moles in 1.16 x 10^23 fluorine atoms. This calculation is done by dividing the number of atoms by Avogadro's number (6.022 x 10^23 atoms/mol).
2 atoms of S + 10 atoms of F = 12 atoms total
To find the number of moles in 76 grams of fluorine, you first need to determine the molar mass of fluorine, which is approximately 19 grams per mole. Then, you divide the given mass (76 grams) by the molar mass of fluorine to get the number of moles. In this case, 76 grams of fluorine is equal to approximately 4 moles.
2
Amount of F atoms = (1.50x1023)/(6.02x1023) = 0.249mol Note: F in elemental form exists as diatomic F2 so the amount of fluorine gas would be 0.125mol.
To determine the number of atoms in 2NaF, we first need to break down the formula. "2Na" indicates 2 atoms of sodium, while "F" represents 1 atom of fluorine. Therefore, 2NaF contains a total of 3 atoms: 2 atoms of sodium and 1 atom of fluorine.
There are three elements in SnF2: one tin (Sn) atom and two fluorine (F) atoms.