To solve the problem of finding how many grams of fluorine (F2) are needed to generate 3.25 moles of carbon tetrafluoride (CF4), we can follow these steps:
1. Understand the Stoichiometry:
The balanced chemical equation is:
[tex]\[
C + 2 F_2 \rightarrow CF_4
\][/tex]
This equation tells us that 1 mole of CF4 requires 2 moles of F2.
2. Determine Moles of Fluorine (F2) Needed:
Since 1 mole of CF4 requires 2 moles of F2, to produce 3.25 moles of CF4, we need:
[tex]\[
2 \text{ (moles of F2)} \times 3.25 \text{ (moles of CF4)} = 6.5 \text{ (moles of F2)}
\][/tex]
3. Calculate the Mass of Fluorine (F2) Needed:
We know the molar mass of F2 is 38.00 g/mol. To find the mass of 6.5 moles of F2, we multiply the number of moles by the molar mass:
[tex]\[
6.5 \text{ (moles of F2)} \times 38.00 \text{ (g/mol)} = 247.0 \text{ g}
\][/tex]
Therefore, 247.0 grams of fluorine (F2) are needed to generate 3.25 moles of carbon tetrafluoride (CF4).
