Copper (II) flouride contains 37.42% F by mass. Use this percentage to calculate the mass of flourine (in grams) contained in 35.6 g of copper (II)fluoride.
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How many grams of Cl are present in 55g of CFCl3?
You (or another anonymous) asked this question a couple of days ago. The answer is the same.
If CuF2 is 37.42% by mass of F, then 35.6 grams must contain 37.42% of 35.6 g. Don't forget to change percent to a decimal.
To calculate the mass of fluorine in 35.6 g of copper (II) fluoride, we first need to find the mass of copper (II) fluoride (CuF2) present in the given sample.
Given that copper (II) fluoride contains 37.42% F by mass, the remaining percentage must be from copper (II). Therefore, the mass percentage of copper (II) is 100% - 37.42% = 62.58%.
To calculate the mass of copper (II) fluoride in 35.6 g, we multiply the mass by its percentage:
Mass of CuF2 = 35.6 g × 62.58% = 22.27328 g
Now, since the compound is copper (II) fluoride (CuF2), the molar ratio of copper (II) to fluorine is 1:2. This means that for every mole of copper (II) fluoride, there are two moles of fluorine.
To calculate the mass of fluorine in 22.27328 g of copper (II) fluoride, we can use the molar mass of fluorine. The molar mass of F is 19 g/mol.
Number of moles of F = Mass of F / Molar mass of F
Number of moles of F = 22.27328 g / 19 g/mol = 1.171808421 moles
Since the molar ratio between copper (II) and fluorine is 1:2, the number of moles of fluorine is twice the number of moles of copper (II) fluoride.
Number of moles of F = 2 × Number of moles of CuF2 = 2 × 1.171808421 moles = 2.343616842 moles
Finally, to find the mass of fluorine in grams, we multiply the number of moles of F by its molar mass:
Mass of fluorine = Number of moles of F × Molar mass of F
Mass of fluorine = 2.343616842 moles × 19 g/mol = 44.522725 g
Thus, the mass of fluorine contained in 35.6 g of copper (II) fluoride is approximately 44.522725 g.
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To find the grams of chlorine (Cl) in 55 g of CFCl3, we need to determine the mass percentage of chlorine in CFCl3 (carbon tetrafluoride).
CFCl3 has a molecular formula of CCl2F2. From the formula, we can see that there are two chlorine atoms in one molecule of CFCl3.
The molar mass of chlorine (Cl) is 35.45 g/mol.
To calculate the mass percentage of chlorine in CFCl3, we can first find the molar mass of CFCl3:
Molar mass of CFCl3 = (1 × Molar mass of C) + (2 × Molar mass of Cl) + (3 × Molar mass of F)
Molar mass of CFCl3 = (12.01 g/mol) + (2 × 35.45 g/mol) + (3 × 19 g/mol)
Molar mass of CFCl3 = 12.01 g/mol + 70.9 g/mol + 57 g/mol
Molar mass of CFCl3 = 139.91 g/mol
The molar mass of CFCl3 is 139.91 g/mol.
Now, we can calculate the mass percentage of chlorine in CFCl3:
Mass percentage of Cl = (2 × Molar mass of Cl) / Molar mass of CFCl3 × 100%
Mass percentage of Cl = (2 × 35.45 g/mol) / 139.91 g/mol × 100%
Mass percentage of Cl = 70.9 g/mol / 139.91 g/mol × 100%
Mass percentage of Cl ≈ 50.66%
Therefore, in 55 g of CFCl3, the mass of chlorine would be:
Mass of Cl = Mass percentage of Cl × Total mass of CFCl3
Mass of Cl = 50.66% × 55 g
Mass of Cl = 0.5066 × 55 g
Mass of Cl ≈ 27.87 g
Thus, there are approximately 27.87 grams of chlorine (Cl) in 55 grams of CFCl3.
To calculate the mass of fluorine in copper (II) fluoride, we first need to determine the amount of fluorine present.
Step 1: Identify the given information
- Copper (II) fluoride contains 37.42% F by mass.
- You have 35.6 g of copper (II) fluoride.
Step 2: Calculate the mass of fluorine using the percentage
- If copper (II) fluoride contains 37.42% F by mass, it means that for every 100 g of the compound, 37.42 g is fluorine.
- To calculate the mass of fluorine in 35.6 g of copper (II) fluoride, we can set up a proportion:
(37.42 g F / 100 g CuF2) = (x g F / 35.6 g CuF2)
- Cross-multiplying, we find:
x g F = (37.42 g F * 35.6 g CuF2) / 100 g CuF2
Step 3: Calculate the mass of fluorine
- By substituting the given values, we get:
x g F = (37.42 g F * 35.6 g CuF2) / 100 g CuF2
- Evaluating this expression, we find:
x g F = 13.30152 g F
Therefore, the mass of fluorine contained in 35.6 g of copper (II) fluoride is 13.30152 grams.
Now, let's move on to the next question.
To calculate the mass of chlorine (Cl) in CFCl3, we need to know the percentage of Cl in the compound. Unfortunately, it is not provided in the question. Without the percentage, we cannot accurately determine the mass of Cl in CFCl3.