She tells you that instead of titrating metal carbonates, it should be possible to react them with an excess of acid and collect the carbon dioxide gas that is generated by the reaction in a eudiometer. From the volume of carbon dioxide, you can calculate the moles of metal carbonate that reacted and use this information to determine the molar mass of the metal carbonate. She gives you a sample of another unknown metal carbonate to test this approach. You weigh out 0.1836 g of the unknown sample and react it with an excess of hydrochloric acid inside a eudiometer at 18.4 °C and 0.956 atm. Once the reaction is complete, you find that 17.20 mL of carbon dioxide gas were produced. a) How many moles of metal carbonate reacted? mol b) What is the molar mass of the metal carbonate? g/mol c) What is the chemical symbol of the metal cation?
She tells you that instead of titrating metal carbonates, it should be possible to react them with an excess of acid and collect the carbon dioxide gas that is generated by the reaction in a eudiometer. From the volume of carbon dioxide, you can calculate the moles of metal carbonate that reacted and use this information to determine the molar mass of the metal carbonate. She gives you a sample of another unknown metal carbonate to test this approach. You weigh out 0.1836 g of the unknown sample and react it with an excess of hydrochloric acid inside a eudiometer at 18.4 °C and 0.956 atm. Once the reaction is complete, you find that 17.20 mL of carbon dioxide gas were produced. a) How many moles of metal carbonate reacted? mol b) What is the molar mass of the metal carbonate? g/mol c) What is the chemical symbol of the metal cation?
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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She tells you that instead of titrating metal carbonates, it should be possible to react them with an excess of acid and collect the carbon dioxide gas that is generated by the reaction in a eudiometer. From the volume of carbon dioxide, you can calculate the moles of metal carbonate that reacted and use this information to determine the molar mass of the metal carbonate. She gives you a sample of another unknown metal carbonate to test this approach. You weigh out 0.1836 g of the unknown sample and react it with an excess of hydrochloric acid inside a eudiometer at 18.4 °C and 0.956 atm. Once the reaction is complete, you find that 17.20 mL of carbon dioxide gas were produced.
a) How many moles of metal carbonate reacted?
mol
b) What is the molar mass of the metal carbonate?
g/mol
c) What is the chemical symbol of the metal cation?
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