An antacid tablet weighing 0.833 g contained calcium carbonate as the active ingredient, in addition to an inert binder. when an acid solution weighing 58.072 g was added to the tablet, carbon dioxide gas was released, producing a fizz. the resulting solution weighed 57.053 g. how many grams (g) of carbon dioxide were produced?

1.852 g of CO2 were produced in the chemical reaction

Explanation:

The problem is pretty simple. We can write down the chemical reaction that is involved to help us understand better what is going on in the process:

CaCO3 (aq) + HAc (aq) → CaAc (aq) + CO2 (g) + H2O (l)

Let's think this through: we have a tablet that has an active compound (CaCO3) and an inert substance that weighs 0.833 g. When we add 58.072 g of an acid solution (represented in the equation as HAc because we are not told specifically which acid is being added), CO2 is formed and released from solution as gas leaving us with an aqueous solution that weighs 57.053 g.

Having said that, we know that the only mass lost during the reaction is due to the formation of CO2 gas. Therefore, we sum the reactants (the tablet + the acid solution) and subtract the mass of the remnant solution. This value will indicate us the amount of CO2 formed:

0.833 g of the Tablet + 58.072 g from the Acid solution = 58.905 g

58.905 g of reactants - 57.053 g of remnant solution = 1.852 g of produced CO2.