Silver oxide (Ag2O\text{Ag}_2\text{O}Ag2O) decomposes upon heating to produce metallic silver (Ag\text{Ag}Ag) and oxygen gas (O2\text{O}_2O2), according to the following balanced chemical equation:
2Ag2O(s)→4Ag(s)+O2(g) 2\text{Ag}_2\text{O}\text{(s)} \rightarrow 4\text{Ag(s)} + \text{O}_2\text{(g)} 2Ag2O(s)→4Ag(s)+O2(g)A 11.60 g11.60\text{ g}11.60 g sample of silver oxide (Mr=232.0M_r = 232.0Mr=232.0) is completely decomposed.
Calculate the mass, in grams, of metallic silver (Ar=108.0A_r = 108.0Ar=108.0) formed.
