There are 53.4 grams of F2 in 1.73 moles of F2. This is calculated using the molar mass of fluorine (F2) which is 37.9968 g/mol.
The balanced chemical equation for the reaction between F2 and NH3 is: 3 F2 + 4 NH3 -> 6 HF + N2 From the equation, we can see that 3 moles of F2 react with 4 moles of NH3. To find the moles of F2 required to react with 3.50 moles of NH3, we can set up a proportion: 3 moles F2 / 4 moles NH3 = x moles F2 / 3.50 moles NH3 Solving for x, we find that 2.625 moles of F2 are required. To convert this to grams, we use the molar mass of F2 which is approximately 38.00 g/mol. 2.625 moles F2 x 38.00 g/mol = 99.75 grams of F2 required to react with 3.50 moles of NH3.
To find the mass of 5.20 x 10^22 molecules of F2, first calculate the molar mass of F2 (38.00 g/mol). Then, convert the number of molecules to moles by dividing by Avogadro's number (6.022 x 10^23). Finally, multiply the moles by the molar mass to get the mass in grams, which is approximately 3.1 grams.
1 mole F2 = 37.996g F2 = 6.022 x 1023 molecules F2 85g F2 x 6.022 x 1023 molecules F2/37.996g F2 = 1.3 x 1024 molecules F2
Given the balanced equation Kr + 3F2 --> KrF6 In order to find how many moles of F2 are needed to produce 3.0 moles of KrF6, we must convert from moles to moles (mol --> mol conversion). 3.0 mol KrF6 * 3 molecules F2 = 9.0 mol F2 --------- 1 molecule F2
F2 has a linear shape.
first, you need to have a balanced equation. this is S8 + 24F2 = 8SF6 start with your given, which is 17.8g of sulfur 17.8g S8 x 1 mol S8/256.56g S8 (the 256.56 is the molar mass of S8) this gives you .06938. multiply that by 24 mols F2/1 mol S8. which is 1.67 mols of F2. 1.67 mols F2 x 38.00g F2/1 mol F2. (38.00g F2 is the molar mass of F2) your answer is 63.2 g F2 :D
445 g
The balanced chemical equation for the reaction between F2 and NH3 is: 3 F2 + 4 NH3 -> 6 HF + N2 From the equation, we can see that 3 moles of F2 react with 4 moles of NH3. To find the moles of F2 required to react with 3.50 moles of NH3, we can set up a proportion: 3 moles F2 / 4 moles NH3 = x moles F2 / 3.50 moles NH3 Solving for x, we find that 2.625 moles of F2 are required. To convert this to grams, we use the molar mass of F2 which is approximately 38.00 g/mol. 2.625 moles F2 x 38.00 g/mol = 99.75 grams of F2 required to react with 3.50 moles of NH3.
To calculate the number of moles of F2 molecules in 38g, we first need to determine the molar mass of F2, which is 38 grams/mol. Next, we can use the formula: moles = mass / molar mass. Therefore, the number of moles in 38g of F2 is 1 mole.
To find the grams of F2 required for the reaction, first calculate moles of NH3: 69.3 g NH3 / 17.03 g/mol = 4.07 moles NH3. From the balanced equation, 5 moles of NH3 react with 2 moles of F2, so you need 4.07 moles NH3 * (2 moles F2 / 5 moles NH3) * 38.0 g/mol = 30.6 g of F2 for complete reaction.
To find the mass of 5.20 x 10^22 molecules of F2, first calculate the molar mass of F2 (38.00 g/mol). Then, convert the number of molecules to moles by dividing by Avogadro's number (6.022 x 10^23). Finally, multiply the moles by the molar mass to get the mass in grams, which is approximately 3.1 grams.
1 mole F2 = 37.996g F2 = 6.022 x 1023 molecules F2 85g F2 x 6.022 x 1023 molecules F2/37.996g F2 = 1.3 x 1024 molecules F2
The balanced reaction for converting 1 mol of C2H4 to C2H4F2 using F2 gas is: C2H4 + 2 F2 -> C2H4F2 First, calculate the moles of C2H4 in 100g. Then, using the mole ratio from the balanced equation, determine how many moles of F2 are needed. Finally, convert the moles of F2 to liters using the ideal gas law (PV = nRT) at the given conditions.
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F2 < F2- < F2+. This is because F2 has no extra electrons or missing electrons, while F2- has an extra electron making it more stable than F2. F2+ is the least stable as it has lost an electron, creating an electron deficiency.
F2 means that there are two flourines usually a gas is a diatomic molecule. Since a fluorine molecule has an atomic mass of 18.998 that molar mass of F2 would be 18.9998 *2 = 37.996 except in molar mass the units change so instead of being g/mol it would just be grams. so 37.996 grams
To determine the number of moles of fluorine present in 2.67 grams of nitrogen trifluoride (NF3), we first need to calculate the molar mass of NF3, which is 71.0 g/mol. Then we find the moles of NF3 in 2.67 g by dividing the mass by the molar mass: 2.67 g / 71.0 g/mol ≈ 0.038 moles. As there are three fluorine atoms in each molecule of NF3, there are 3 times more moles of fluorine: 0.038 moles NF3 x 3 = 0.114 moles of fluorine.