A 5.00 g sample of impure Ag₂O (MM-231.739 g/mol) is decomposed at 300°C to yield metallic silver (MM-107.87 g/mol) and oxygen gas (MM-31.998 g/mol). The unbalanced chemical equation is given below: Ag₂0 (s) → Ag(s) + O₂ a. What is the mass percent of Ag2O(s) in the sample if its decomposition yields 2.91 g Ag(s)? b. How much Ag(s) and O2(g) (in grams) is produced in the decomposition of 23.0 g of sample? Mass Ag(s): g Mass O₂(g) c. If the actual mass of Ag(3) collected from the 23.0 g sample was 12.3 g, what is the percent yield of the reaction? g %

A 5.00 g sample of impure Ag₂O (MM-231.739 g/mol) is decomposed at 300°C to yield metallic silver (MM-107.87 g/mol) and oxygen gas (MM-31.998 g/mol). The unbalanced chemical equation is given below: Ag₂0 (s) → Ag(s) + O₂ a. What is the mass percent of Ag2O(s) in the sample if its decomposition yields 2.91 g Ag(s)? b. How much Ag(s) and O2(g) (in grams) is produced in the decomposition of 23.0 g of sample? Mass Ag(s): g Mass O₂(g) c. If the actual mass of Ag(3) collected from the 23.0 g sample was 12.3 g, what is the percent yield of the reaction? g %

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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