A 0. 600 g sample containing Ag₂O and inert material is heated, causing the silver oxide to decompose according to the following equation:
2Ag₂O(s) → 4Ag(s) + O₂(g)
If 13.8 mL of gas are collected over water at 27 °C and 1.001 bar external pressure, what is the percentage of silver oxide in the sample? The partial pressure of water is 26.7 mmHg at 27 °C.

Question

Quizplus · Accepted Answer

To find the percentage of Ag₂O, first calculate the moles of O₂ using the ideal gas law, considering the partial pressure of O₂ (subtracting water vapor pressure from total pressure). Then, use stoichiometry to find moles of Ag₂O and convert to grams. Finally, calculate the percentage by dividing the mass of Ag₂O by the total sample mass and multiplying by 100.

A 0 600 G Sample Containing Ag2O and Inert Material Is

A 0 600 G Sample Containing Ag₂O and Inert Material Is