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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 for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter4: Stoichiometry
Section: Chapter Questions
Problem 4.69PAE: 4.69 The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to...
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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) + 0₂ 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(s) collected from the 23.0 g sample was 12.3 g, what is the percent yield of the reaction? g The exact neutralization of 15.00 mL of 0.2500 M H₂SO4 (aq) requires 19.50 mL of the NaOH titrant. a. Balance the chemical equation for the reaction between H₂SO4(aq) and NaOH(aq) H₂SO4(aq) + NaOH(aq) → Na₂SO4(aq) + H₂O(1) b. What is the molarity of the NaOH titrant solution? c. If 5.000 mL of the NaOH solution is diluted to 250.0 mL, what is the new concentration of the NaOH solution? Write your answer in decimal form. Molarity of diluted NaOH solution: M M
Transcribed Image Text: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) + 0₂ 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(s) collected from the 23.0 g sample was 12.3 g, what is the percent yield of the reaction? g The exact neutralization of 15.00 mL of 0.2500 M H₂SO4 (aq) requires 19.50 mL of the NaOH titrant. a. Balance the chemical equation for the reaction between H₂SO4(aq) and NaOH(aq) H₂SO4(aq) + NaOH(aq) → Na₂SO4(aq) + H₂O(1) b. What is the molarity of the NaOH titrant solution? c. If 5.000 mL of the NaOH solution is diluted to 250.0 mL, what is the new concentration of the NaOH solution? Write your answer in decimal form. Molarity of diluted NaOH solution: M M
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