Given 80g of Calcium reacts with Fluorine at STP, how many atoms of Fluorine are consumed?
Heres the formula:
Ca (s) + F(subscript 2) --> CaF(subscript 2)
How do i do this?
Thanks!
Jackie
How many mol is 80 g Ca? 80/40 = about 2
Convert mols Ca to mols F2.
2 mols Ca x (1 mol F2/1 mol Ca) = 2 x 1/1 = 2 mols F2.
1 mol F2 contains 6.022E23 molecules and 12.044E23 atoms F. So how many will 2 moles contain?
So do u multiply 12.044 by 2 again to get 2 moles?
Yes, but it's 12.044E23 x 2 = 24.1E23 = 2.4E24 to two significant figures.
To determine the number of atoms of fluorine consumed in the reaction, we need to follow these steps:
Step 1: Convert the mass of calcium (Ca) to moles.
- The molar mass of calcium is 40.08 g/mol. Therefore, 80g of calcium can be converted to moles using the equation: number of moles = mass / molar mass.
- In this case, number of moles of calcium (Ca) = 80g / 40.08 g/mol = 1.9975 moles.
Step 2: Use the balanced equation to determine the mole ratio between Ca and F₂.
According to the balanced equation: Ca (s) + F₂ → CaF₂
- The stoichiometric coefficient of calcium (Ca) is 1.
- The stoichiometric coefficient of fluorine (F₂) is 1.
This means that one mole of calcium (Ca) reacts with one mole of fluorine (F₂) to produce one mole of calcium fluoride (CaF₂).
Step 3: Determine the number of moles of fluorine (F₂) consumed.
Since the mole ratio between calcium and fluorine is 1:1, the number of moles of fluorine consumed is also 1.9975 moles.
Step 4: Convert the number of moles of fluorine (F₂) to the number of atoms.
- Avogadro's number (6.022 x 10²³) represents the number of atoms in one mole of any substance.
- Multiply the number of moles of fluorine (F₂) by Avogadro's number to get the number of atoms: number of atoms = number of moles x Avogadro's number.
Therefore, the number of fluorine atoms consumed in the reaction is:
- Number of atoms = 1.9975 moles x (6.022 x 10²³ atoms)/mole
Now you can calculate the result.