TUMS®, a form of calcium carbonate often needed after final exams, neutralizes stomach acid according to this reaction: CaCO3(s) + 2HCI(aq) → CaCl2(aq) + H2O(1) + CO2(g) (a) What volume of CO2(g) is produced at 1.00 atm and 37.0 °C when an excess of CaCO3 completely reacts with 605 mg of HCl? (Mm of HCl = 36.461 g/mol) (0.211 L) (b) Suppose the CO2(g) in part (a) was collected over water. What change would be made in the pressure value in your calculation? The vapor pressure of water at 37°C is 45.5 mmHg. (0.94 atm)

TUMS®, a form of calcium carbonate often needed after final exams, neutralizes stomach acid according to this reaction: CaCO3(s) + 2HCI(aq) → CaCl2(aq) + H2O(1) + CO2(g) (a) What volume of CO2(g) is produced at 1.00 atm and 37.0 °C when an excess of CaCO3 completely reacts with 605 mg of HCl? (Mm of HCl = 36.461 g/mol) (0.211 L) (b) Suppose the CO2(g) in part (a) was collected over water. What change would be made in the pressure value in your calculation? The vapor pressure of water at 37°C is 45.5 mmHg. (0.94 atm)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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