how many atoms of chlorine are ther in 87.56 milligrams of barium chlorite?
Barium chlorite is Ba(ClO2)2.
moles Ba(ClO2)2 in 87.56 mg (0.08756 grams) = grams/molar mass.
There will be 6.022 x 10^23 atoms Ba(ClO2) in 1 mole Ba(ClO2)2.
There are two atoms Cl per mole Ba(ClO2)2. Post your work if you get stuck.
ok. so i have:
Ba 137.33
2Cl 70.9
2O 32
= 240.23
2Cl 70.9/240.23 Xs 100= 29.51%
i need mg not g so i convert it 29.51 in mg =0.02951 correct?
if so i have 0.02951mgCl X 1mol/35.45 X 6.022 X 10 to the 23= 0.00083244 X 6.022= 0.005 X 10 to the 23 power. am i on the correct path?
disregard the last post i meade. i submitted it and i realized i forget to add the87.56 into the work!
Ba 137.33
2Cl 70.9
2O 32
= 240.23
2Cl 70.9/240.23 Xs 100= 29.51%
0.2951 X 87.56mg= 25.84mgCl
25.84 Xs 1mol/35.45= 0.729 X 6.022= 4.39 X 10 to the 23 power. is that correct?
Megan
I'm in Mr. Hartzell's class are you?
yes paul i am. im having a blast trying to do this extra credit. how its it going for you?
I have the molar mass of Ba(ClO2)2 = 272.23
mols Ba(ClO2)2 = 0.08756/272.23 = 3.216 x 10^-4 moles.
6.022 x 10^23 molecules/mole x (3.216 x 10^-4 moles) = 1.937 x 10^20 molecules Ba(ClO2)2. There are 2 atoms Cl for each molecule of Ba(ClO2)2 so the number of Cl atoms will be just twice the amount of molecules Ba(ClO2)2.
To determine the number of atoms of chlorine in 87.56 milligrams of barium chlorite, we need to use the concept of molar mass, Avogadro's number, and stoichiometry.
1. Calculate the molar mass of barium chlorite: Barium (Ba) has a molar mass of 137.33 g/mol, chlorine (Cl) has a molar mass of 35.45 g/mol, and oxygen (O) has a molar mass of 16.00 g/mol. The formula of barium chlorite is Ba(ClO2)2, so the molar mass can be calculated as follows:
Molar mass of Ba(ClO2)2 = Molar mass of Ba + 2 × (Molar mass of Cl) + 4 × (Molar mass of O)
= 137.33 + 2 × 35.45 + 4 × 16.00
= 241.33 g/mol
2. Convert milligrams to grams: Since the molar mass is given in grams per mole, we need to convert milligrams to grams. There are 1000 milligrams in a gram, so:
87.56 milligrams = 87.56 / 1000 = 0.08756 grams
3. Use the molar mass to determine the number of moles: Divide the mass of barium chlorite by its molar mass:
Number of moles = Mass / Molar mass
= 0.08756 grams / 241.33 g/mol
≈ 0.000363 moles
4. Apply stoichiometry to determine the number of moles of chlorine: From the balanced chemical equation of barium chlorite, we know that there are two moles of chlorine for every one mole of barium chlorite.
Number of moles of chlorine = Number of moles of barium chlorite × 2
≈ 0.000363 moles × 2
≈ 0.000726 moles
5. Use Avogadro's number to determine the number of atoms: Avogadro's number, 6.022 × 10^23 atoms/mol, tells us the number of atoms per mole. Multiply the number of moles of chlorine by Avogadro's number:
Number of atoms of chlorine = Number of moles of chlorine × Avogadro's number
≈ 0.000726 moles × (6.022 × 10^23 atoms/mol)
≈ 4.374 × 10^20 atoms of chlorine
Therefore, there are approximately 4.374 × 10^20 atoms of chlorine in 87.56 milligrams of barium chlorite.