3. When hydrogen sulfide (MW = 34.08 g/mol) gas is bubbled into a solution of sodium hydroxide (40.00 g/mol), their reaction forms sodium sulfide (78.05 g/mol) and water (18.02 g/mol) according to the following reaction. H2S(g) a. Write the properly balanced chemical equation b. What is the theoretical yield of sodium sulfide, if 1.50 g of hydrogen sulfide is reacted with a solution containing 1.65 g of sodium hydroxide, assuming the limiting reagent is completely consumed? C. What is the limiting reactant? N2OH(aq) Nazsłaq) H2O() ----> d. If the actual yield of sodium sulfide is determined to be 1.00 g. what is the percent yield.

3. When hydrogen sulfide (MW = 34.08 g/mol) gas is bubbled into a solution of sodium hydroxide (40.00 g/mol), their reaction forms sodium sulfide (78.05 g/mol) and water (18.02 g/mol) according to the following reaction. H2S(g) a. Write the properly balanced chemical equation b. What is the theoretical yield of sodium sulfide, if 1.50 g of hydrogen sulfide is reacted with a solution containing 1.65 g of sodium hydroxide, assuming the limiting reagent is completely consumed? C. What is the limiting reactant? N2OH(aq) Nazsłaq) H2O() ----> d. If the actual yield of sodium sulfide is determined to be 1.00 g. what is the percent yield.

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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