|Solid silver oxide, Ag2O(s), decomposes at tempera- | tures in excess of 300 °C, yielding metallic silver and |oxygen gas. A 3.13 g sample of impure silver oxide |yields 0.187 g O2(g). What is the mass percent Ag20 in the sample? Assume that Ag2O(s) is the only |source of O2g)- [Hint: Write a balanced equation for |the reaction.

|Solid silver oxide, Ag2O(s), decomposes at tempera- | tures in excess of 300 °C, yielding metallic silver and |oxygen gas. A 3.13 g sample of impure silver oxide |yields 0.187 g O2(g). What is the mass percent Ag20 in the sample? Assume that Ag2O(s) is the only |source of O2g)- [Hint: Write a balanced equation for |the reaction.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter4: Reactions In Aqueous Solution

Section: Chapter Questions

Problem 62QAP: Ten mL of concentrated H3PO4 (91.7% by mass, d=1.69g/mL) was accidentally poured into a beaker...

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Iodine can be prepared by allowing an aqueous solution of hydrogen iodide to react with manganese dioxide, MnO2. The reaction is 2I(aq)+4H+(aq)+MnO2(s)Mn2+(aq)+2H2O+I2(s) If an excess of hydrogen iodide is added to 0.200 g of MnO2, how many grams of iodine are obtained, assuming 100% yield?
On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
Ten mL of concentrated H3PO4 (91.7% by mass, d=1.69g/mL) was accidentally poured into a beaker containing 20.0 g of NaOH. Not all the NaOH was consumed. How many grams of NaOH were left unreacted? The equation for the reaction is H3PO4(aq)+3OH(aq)3H2O+PO43(aq)
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