Question

TUMS is a popular remedy for acid indigestion. A typical TUMS tablet contains calcium carbonate plus some inert substances. When ingested, it reacts with the gastric juice (hydrochloric acid) in the stomach to give off carbon dioxide gas. When a 1.367−g tablet reacted with 40.00 mL of hydrochloric acid (density = 1.140 g/mL), carbon dioxide gas was given off, and the resulting solution weighed 46.699 g. Calculate the number of liters of carbon dioxide gas released if its density is 1.81 g/L.

Answer 1

Answer:

0.333 L CO2

Explanation:

Hello,

I'm attaching the picture with the mathematical procedure for this exercise.

Don't forget to consider that the HCl is in excess because the resulting solution's weight is pretty much similar to the HCl's mass (40 mL*1.14 g/mL=45.6g), so we can say that it is by far in excess, thus, the resulting CO2 is computed based in the initial amount of calcium carbonate as is shown in the picture. One could say that the reaction is likely to be:

$CaCO_3+2HCl-->CO_2+H_2O+CaCl_2$

For us to know the stoichiometric relationship.

Best regards.