2 NaHCO3 (s) → N22CO3 (s) + CO2 (g) + H2O (g)1. Calculate the moles of NaHCO3 in 3.00 g of NaHCO3.3,00842. Using your answer to question one, if 1 mole of Na2CO3 is produced for every 2 moles of NaHCO3, howmany moles of Na2CO3 would theoretically be produced in the reaction?3. How many grams of Na2CO3 would theoretically be produced in the reaction?4. If the actual mass of Na2CO3 produced is 1.25 g, what is the percent yield of Na2CO3?Actual yield (g)Theoretical yield (g)Percent yield =100%5. Calculate the theoretical mass of H2O produced from the decomposition of 3.00 g NaHCO3 using similarcalculations as above.

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the moles

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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Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

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