1 mole F atoms = 6.022 x 1023 F atoms
1.01 x 1023 F atoms x (1mol F atoms/6.022 x 1023 Fe atoms) = 0.168mol Fe
Boron trifluoride is BF3. So each mole of BF3 contains 1 moles of boron (B) and 3 moles of fluorine (F). Thus, 3 moles of BF3 contains NINE moles of fluorine.
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.
a carbon atom can share electrons with up to four other atoms.
The answer is SeF6.This is figured by:2.231 grams of Se divided by 78.79 g/mol = 0.0283 moles of Se3.221 grams of F divided by 18.998 g/mol = 0.1695 moles of F0.1695 moles of Se/0.0283 moles of F = 5.9909 ~ 6 moles of Se/mole of FSo SeF6
C-Cl bonds are easier to break than C-F bonds.
The answer is two moles of F atoms or 1 mole of F2 molecules.
Approx. 0,1 mole F2 (o,2 mole as F).
The mass of 4 moles of fluorine F atoms is 151,98 g (because fluorine is a diatomic element).
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
(76 g F) * (1mol F/ 19g F) = 4 moles of F
each mole has avogadro's number of atoms in it, which is 6.02 x 10 to the 23rd power. so, 4 x 6.02 x 10 23 power of atoms
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.
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
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.
0.8 moles Explanation: from the equation we can see, 2 mole A l is needed to react completely with 3 mole F e O so, 3 moles of F e O needs 2 moles A l so, 1 mole F e O needs 2 3 moles A l so, 1.2 mol F e O needs 2 × 1.2 3 moles A l = 0.8 moles A l
Boron trifluoride is BF3. So each mole of BF3 contains 1 moles of boron (B) and 3 moles of fluorine (F). Thus, 3 moles of BF3 contains NINE moles of fluorine.
2.67 g NF3 x 1 mole NF3/71 g NF3 x 3 mole F/mole NF3 = 0.113 moles Fluorine