In the balanced double replacement reaction of calcium chloride CaCl2 and aluminum sulfate Al2(SO4)3, how many grams of calcium sulfate can be produced if you start the reaction with 18.97 grams of calcium chloride and the reaction goes to completion?

3CaCl2 + Al2(SO4)3 ==> 3CaSO4 + 2AlCl3

mols CaCl2 = grams/molar mass
Convert mols CaCl2 to mols CaSO4 using the coefficients in the balanced equation.
Convert mols CaSO4 to g. g = mols x molar mass.

the final answer is 7750.80/333.012= 23.27g CaSOa if you follow DrBob222 steps

To determine the number of grams of calcium sulfate produced in the reaction, we need to follow several steps:

1. Begin by writing the balanced chemical equation for the reaction:
CaCl2 + Al2(SO4)3 → CaSO4 + 2AlCl3

2. Calculate the molar mass of calcium chloride (CaCl2):
Ca: 1 atom x 40.08 g/mol = 40.08 g/mol
Cl: 2 atoms x 35.45 g/mol = 70.90 g/mol
Total: 40.08 g/mol + 70.90 g/mol = 110.98 g/mol

3. Use the molar mass to convert the given mass of calcium chloride to moles:
Moles of CaCl2 = Mass / Molar mass
Moles of CaCl2 = 18.97 g / 110.98 g/mol = 0.171 mol

4. Examine the balanced equation to determine the mole ratio between calcium chloride and calcium sulfate. From the equation, we see that 1 mole of CaCl2 reacts to produce 1 mole of CaSO4.

5. Determine the moles of calcium sulfate produced:
Moles of CaSO4 = Moles of CaCl2 (since the ratio is 1:1)
Moles of CaSO4 = 0.171 mol

6. Finally, convert the moles of calcium sulfate to grams using its molar mass:
Molar mass of CaSO4: Ca: 1 atom x 40.08 g/mol = 40.08 g/mol,
S: 1 atom x 32.07 g/mol = 32.07 g/mol,
O: 4 atoms x 16.00 g/mol = 64.00 g/mol
Total: 40.08 g/mol + 32.07 g/mol + 64.00 g/mol = 136.15 g/mol

Mass of CaSO4 = Moles of CaSO4 x Molar mass
Mass of CaSO4 = 0.171 mol x 136.15 g/mol ≈ 23.30 grams

Therefore, approximately 23.30 grams of calcium sulfate can be produced if the reaction goes to completion starting with 18.97 grams of calcium chloride.