Copper (2) fluoride contains 37.42% F by mass. calculate the mass of fluorine (in grams) contained in 35.6 g of copper(2) fluoride.

37.42% of 35.6 g = ??

9513.g

You had 35.6 g CuF2 to start. Only part of that was F. How can you have more F than you started with? Did you multiply by percent OR did you convert percent to a decimal before multiplying. You should have converted percent to a decimal.

To calculate the mass of fluorine in copper (II) fluoride, you need to know the molar mass and the percentage composition of fluorine in the compound.

Step 1: Find the molar mass of copper (II) fluoride (CuF2).
The atomic mass of copper (Cu) is 63.55 g/mol, and the atomic mass of fluorine (F) is 18.998 g/mol. The molar mass of copper (II) fluoride is the sum of the molar masses of copper and twice the molar mass of fluorine.
Molar mass of CuF2 = (63.55 g/mol) + 2 * (18.998 g/mol) = 127.05 g/mol

Step 2: Calculate the mass of fluorine in copper (II) fluoride.
Since the compound contains 37.42% F by mass, that means 37.42 grams of the compound consists of fluorine.
Mass of F in 100 g of CuF2 = (37.42 g F / 100 g CuF2) * 100 g CuF2
Mass of F in 100 g of CuF2 = 37.42 g F

Step 3: Convert the mass of fluorine to the mass of F in 35.6 g of CuF2.
Use the proportion:
(37.42 g F) / (100 g CuF2) = X g F / 35.6 g CuF2

To solve for X (the mass of F in 35.6 g of CuF2), you can use cross-multiplication:
X g F = (37.42 g F / 100 g CuF2) * 35.6 g CuF2

Now, calculate X:
X g F = (37.42 g F * 35.6 g CuF2) / 100 g CuF2

X g F = 13.31 g F

Therefore, the mass of fluorine in 35.6 g of copper (II) fluoride is 13.31 grams.