The active ingredient in Tums antacid tablets is calcium carbonate, which neutralizes stomach acid according to...

 

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The active ingredient in Tums® antacid tablets is calcium carbonate, which neutralizes stomach acid according to the following reaction: CaCO3(s) + 2HCl(aq) → H₂O(1) +CaCl₂(aq) + CO₂(g) a. Stomach acid is approximately 0.160 M. How many grams of CaCO3 would you need to neutralize 880 mL of stomach acid? b. Many acid/base reactions are exothermic. Use the following data to calculate the AH for the above reaction. AH°, (kJ/mol) -1207.6 -167.2 CaCO3(s) HCl(aq) H₂O(l) -285.8 CaCl₂(aq) -877.3 CO₂(g) -393.5 c. Using your value for the heat of the reaction from (b) calculate the heat (in kJ) associated with the reaction of 45.0 mL of HCI (density = 1.04 g/mL). xn The active ingredient in Tums® antacid tablets is calcium carbonate, which neutralizes stomach acid according to the following reaction: CaCO3(s) + 2HCl(aq) → H₂O(1) +CaCl₂(aq) + CO₂(g) a. Stomach acid is approximately 0.160 M. How many grams of CaCO3 would you need to neutralize 880 mL of stomach acid? b. Many acid/base reactions are exothermic. Use the following data to calculate the AH for the above reaction. AH°, (kJ/mol) -1207.6 -167.2 CaCO3(s) HCl(aq) H₂O(l) -285.8 CaCl₂(aq) -877.3 CO₂(g) -393.5 c. Using your value for the heat of the reaction from (b) calculate the heat (in kJ) associated with the reaction of 45.0 mL of HCI (density = 1.04 g/mL). xn

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Cace s 2HCl aa H0 1 Caclaq COg moker of Mcl X volume L x molarity moL1 Mcl 12 088 Lx 0160m b Ho... View the full answer