Question

Calcium carbonate, CaCO3, reacts with stomach acid (HCl, hydrochloric acid) according to the following equation: CaCO3(s)+2HCl(aq)→ CaCl2(aq)+H2O(l)+CO2(g)

One tablet of Tums, an antacid, contains 500.0 mg of CaCO3.

a) If one tablet of Tums is added to 34.5 mL of a 0.250 M HCl solution how many liters of CO2 gas are produced at STP?

Express your answer with the appropriate units.

Answer 1

CaCO3(s)+2HCl(aq)→ CaCl2(aq)+H2O(l)+CO2(g)

a. no of moles of HCl = molarity * volume in L

                                     = 0.25*0.0345   = 0.008625 moles

from balanced equation

2 moles of HCL react with CaCo3 to gives 1 mole of CO2

2 moles of HCL react with CaCo3 to gives 22.4L of CO2

0.008625 moles of HCl react with CaCo3 to gives = 22.4*0.008625/2   = 0.0966 L of CO2