You weigh out 0.2103 g of the unknown sample and react it with an excess of hydrochloric acid inside a eudiometer at 16.6 °C and 0.902 atm. Once the reaction is complete, you find that 55.39 mL of carbon dioxide gas were produced. a) How many moles of metal carbonate reacted? b) What is the molar mass of the metal carbonate?
You've thoroughly impressed your PI with your work, and she soon has a new challenge for you. 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 (a special glass tube for measuring the volumes of gases). 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 0.2103 g of the unknown sample and react it with an excess of hydrochloric acid inside a eudiometer at 16.6 °C and 0.902 atm. Once the reaction is complete, you find that 55.39 mL of carbon dioxide gas were produced.
a) How many moles of metal carbonate reacted?
b) What is the molar mass of the metal carbonate?
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