rasen58 Posted January 8, 2014 Share Posted January 8, 2014 (edited) A 98 gram sample of silver oxide is heated in an open container until all the oxygen has been driven off. What is the total mass of silver remaining in the container? I used to know how to do such problems, but I'm not sure where to start. I know the mass of silver is 107.9 and oxygen's is about 16, so the molar mass of AgO would be 123.9 g/mol, but I'm not sure what to do after that. Edited January 8, 2014 by rasen58 Link to comment Share on other sites More sharing options...
hypervalent_iodine Posted January 8, 2014 Share Posted January 8, 2014 You can do it a couple of ways, but the simplest is probably by looking at the mass percentage of silver in AgO. Are you familiar with how to do this? Link to comment Share on other sites More sharing options...
rasen58 Posted January 9, 2014 Author Share Posted January 9, 2014 No, not really. Link to comment Share on other sites More sharing options...
hypervalent_iodine Posted January 9, 2014 Share Posted January 9, 2014 Alright, well you should know that the mass of a compound is the sum of the mass of its components. NaCl, for example has a molar mass of 58.45 g / mol, of which 35.45 g / mol is Cl and 23 g / mol comes from the Na. We can also express these values as a percentage of the total mass (this is the mass %) and use those numbers to work out the mass of each component of a compound in a given sample. For example: Does that make sense? See if you can try that approach with your question, or otherwise I can show you how to do it using number of moles and stoicheometric ratios. Link to comment Share on other sites More sharing options...
rasen58 Posted January 9, 2014 Author Share Posted January 9, 2014 Ohh, I see! Thank you! Link to comment Share on other sites More sharing options...
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