Elemental sulfur occurs as octatomic molecules, S8. What mass of fluorine gas is needed to react completely with 19.0g of sulfur to form sulfur hexafluoride?
first you need a balanced equation, so:
24F2+S8 --> 8SF6
then find the no. of moles of s8 (which is 19g divided by molar mass of s8)
then use the reaction ratio of 24:1 to multiply your answer to get number of moles of fluorine
then convert from moles to mass using m=n*M
19.0/256.56 multiply by 24 mol F2 multiply by 38g F2 after calculation will give you the mass in grams of F2.
To determine the mass of fluorine gas needed to react completely with 19.0g of sulfur to form sulfur hexafluoride, we need to use the balanced chemical equation for the reaction between sulfur and fluorine:
S8 + 24F2 -> 8SF6
From the equation, we can see that it takes 24 moles of fluorine gas to react with 1 mole of sulfur.
First, calculate the molar mass of sulfur (S), which is 32.06 g/mol.
Next, calculate the number of moles of sulfur in 19.0g of sulfur. We'll use the formula:
moles = mass / molar mass
moles of sulfur = 19.0g / 32.06 g/mol = 0.593 mol (approximately)
Since the molar ratio between sulfur and fluorine is 1:24, we can determine the number of moles of fluorine gas needed:
moles of fluorine = moles of sulfur x 24
= 0.593 mol x 24
= 14.232 mol
Finally, calculate the mass of fluorine gas needed using the molar mass of fluorine (F), which is 19.00 g/mol:
mass of fluorine = moles of fluorine x molar mass
= 14.232 mol x 19.00 g/mol
= 270.648 g (approximately)
Therefore, approximately 270.648 grams of fluorine gas is needed to react completely with 19.0g of sulfur to form sulfur hexafluoride.
To find out the mass of fluorine gas needed to react completely with sulfur to form sulfur hexafluoride, we need to follow these steps:
Step 1: Write the balanced chemical equation for the reaction between sulfur and fluorine to form sulfur hexafluoride (SF6).
S8 + 24 F2 → 8 SF6
From the balanced equation, we can see that 1 mole of sulfur (S8) reacts with 24 moles of fluorine (F2) to produce 8 moles of sulfur hexafluoride (SF6).
Step 2: Calculate the molar mass of sulfur (S8) and fluorine (F2).
S8: The molar mass of sulfur (S) is approximately 32.06 g/mol.
To calculate the molar mass of sulfur (S8), we multiply the molar mass of sulfur by 8:
Molar mass of S8 = 32.06 g/mol × 8 = 256.48 g/mol
F2: The molar mass of fluorine (F) is approximately 18.998 g/mol.
Since we have 2 fluorine atoms in 1 fluorine molecule (F2), we multiply the molar mass of fluorine by 2:
Molar mass of F2 = 18.998 g/mol × 2 = 37.996 g/mol
Step 3: Calculate the moles of sulfur (S8) using its given mass.
Given: Mass of sulfur = 19.0 g
To convert the mass of sulfur to moles, we divide the mass by the molar mass:
Moles of sulfur = Mass of sulfur / Molar mass of sulfur (S8)
Moles of sulfur = 19.0 g / 256.48 g/mol ≈ 0.074 moles
Step 4: Use the mole ratio from the balanced equation to calculate the moles of fluorine (F2) required.
From the balanced equation, we know that 8 moles of SF6 are produced from 24 moles of F2.
So, the mole ratio of F2 to SF6 is 24:8 or 3:1.
Moles of fluorine (F2) = Moles of sulfur (S8) × (Moles of F2 / Moles of S8)
Moles of fluorine (F2) = 0.074 moles × (3 moles F2 / 1 mole S8) = 0.222 moles
Step 5: Convert the moles of fluorine (F2) to grams using its molar mass.
Mass of fluorine (F2) = Moles of fluorine (F2) × Molar mass of fluorine (F2)
Mass of fluorine (F2) = 0.222 moles × 37.996 g/mol ≈ 8.42 g
Therefore, approximately 8.42 grams of fluorine gas is needed to react completely with 19.0 grams of sulfur to form sulfur hexafluoride.