If a tablet of TUMS contains 500mg of the active ingredient, CaCO3, how many tablets would it take to neturalize the 1.5g of HCl?

From balanced equation: CaCO3 + 2HCl = CaCl2 + H2O + CO2

500 mg = 0.500g

mols HCl = g/molar mass = 1.5/30.0416.5 = approximately 0.041 but you need to do it more accurately.
mols CaCO3 = 0.041 mols HCl x (1 mol CaCO3/2 mol HCl) = 0.041 x 1/2 = approx 0.02 mols CaCO3.
g CaCO3 = mols x molar mass = approx 0.02 x 100 = approx 2 g CaCO3.
Then (0.500 g CaCO3/tab) x # tab = 2g.
Solve for # tabs.

To determine the number of tablets required to neutralize 1.5g of HCl using TUMS tablets, we need to calculate the quantity of calcium carbonate (CaCO3) required to neutralize this amount of HCl.

From the balanced equation provided: CaCO3 + 2HCl = CaCl2 + H2O + CO2, we can see that one mole of CaCO3 reacts with two moles of HCl.

First, we need to calculate the number of moles of HCl in 1.5g. We can do this using the molecular weight of HCl, which is 36.46 g/mol:
Moles = Mass / Molecular weight
Moles = 1.5g / 36.46 g/mol
Moles = 0.041 moles

According to the balanced equation, 1 mole of CaCO3 is required to react with 2 moles of HCl. Therefore, we need double the number of moles of HCl in terms of CaCO3:
Moles of CaCO3 = 2 * 0.041 moles
Moles of CaCO3 = 0.082 moles

The molar mass of CaCO3 is 100.09 g/mol. Now, we can calculate the mass of CaCO3 required in grams:
Mass of CaCO3 = Moles * Molecular weight
Mass of CaCO3 = 0.082 moles * 100.09 g/mol
Mass of CaCO3 = 8.208 g

Since each TUMS tablet contains 500mg (0.5g) of CaCO3, we can calculate the number of tablets needed:
Number of tablets = Mass of CaCO3 required / Mass per tablet
Number of tablets = 8.208 g / 0.5 g per tablet
Number of tablets = 16.416 tablets

Therefore, it would take approximately 16 tablets of TUMS to neutralize 1.5g of HCl.