How many Ca +2 ions in 40.08g of CaCO3 (Calcium Carbonate)
I'm unsure on how to approach this problem and set it up.
How many moles in 40.08 g CaCO3.
moles = grams/molar mass
How many molecules of CaCO3 are in that many moles. Remember there are 6.02 x 10^23 molecules per mole of anything.
Now that you know the number of CaCO3 molecules, how many Ca^+2 ions per molecule. There is 1.
I think the molar mass CaCO3 = about 100 grams/mole but you can look it up exactly.
40.08 g CaCO3 x (1 mole CaCO3/100 g CaCO3) x (6.02 x 10^23 molecules CaCO3/1 mole CaCO3) x (1 Ca^+2/1 CaCO3 molecule) = ?? Ca^+2 ions.
Check my thinking.
To determine the number of Ca+2 ions in 40.08g of CaCO3 (Calcium Carbonate), you need to first calculate the number of moles of CaCO3 using its molar mass. Then, you can use the mole ratio between CaCO3 and Ca+2 to find the number of Ca+2 ions.
1. Calculate the molar mass of CaCO3:
- Calcium (Ca) has a molar mass of 40.08 g/mol.
- Carbon (C) has a molar mass of 12.01 g/mol.
- Oxygen (O) has a molar mass of 16.00 g/mol.
So, the molar mass of CaCO3 is:
(1 * 40.08) + (1 * 12.01) + (3 * 16.00) = 100.09 g/mol.
2. Use the molar mass of CaCO3 to calculate the number of moles:
Number of moles = Mass / Molar mass
Number of moles = 40.08 g / 100.09 g/mol
Number of moles = 0.4005 mol
3. Apply the mole ratio from the balanced chemical equation of CaCO3:
CaCO3 dissociates into one Ca+2 ion and one CO3-2 ion.
Therefore, for every 1 mole of CaCO3, you have 1 mole of Ca+2 ions.
4. Calculate the number of Ca+2 ions in 0.4005 moles of CaCO3:
Number of Ca+2 ions = Number of moles of CaCO3 * (Avogadro's number)
Number of Ca+2 ions = 0.4005 mol * (6.022 x 10^23 ions/mol)
Number of Ca+2 ions ≈ 2.41 x 10^23 Ca+2 ions
So, in 40.08g of CaCO3, there are approximately 2.41 x 10^23 Ca+2 ions.