If Tums is added to 55.0 {\rm mL} of 0.750 {\rm M}{\rm HCl}, how many grams of {\rm CO}_{2} gas are produced?
To calculate the grams of CO2 gas produced when Tums is added to HCl, we first need to determine the chemical reaction between these two substances.
The active ingredient in Tums is calcium carbonate (CaCO3), while HCl is hydrochloric acid. The reaction between calcium carbonate and hydrochloric acid can be represented as:
CaCO3 + 2HCl → CaCl2 + CO2 + H2O
From the balanced chemical equation, we can see that for each mole of calcium carbonate, 1 mole of CO2 is produced.
Next, we need to determine the number of moles of HCl in 55.0 mL of 0.750 M HCl solution.
First, convert the volume of the solution to liters:
55.0 mL = 55.0 mL * (1 L / 1000 mL) = 0.055 L
Next, we use the molarity (M) and volume (V) to calculate the number of moles of HCl:
moles of HCl = Molarity * Volume
= 0.750 M * 0.055 L
= 0.04125 moles
According to the balanced chemical equation, 1 mole of HCl reacts with 1 mole of CO2. Therefore, the number of moles of CO2 produced will also be 0.04125 moles.
Finally, we can calculate the mass of CO2 using the molar mass of CO2:
Molar mass of CO2 = (12.01 g/mol) + (2 * 16.00 g/mol) = 44.01 g/mol
Mass of CO2 = number of moles * molar mass of CO2
= 0.04125 moles * 44.01 g/mol
= 1.82 grams
Therefore, when Tums is added to 55.0 mL of a 0.750 M HCl solution, approximately 1.82 grams of CO2 gas is produced.