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If you have 215.8g of silver and 32.1g of sulfide how much silver sulfide do you have?
Wiki User
∙ 6y ago
215.8 g Ag x 1 mol Ag/196.9 = 1.096 moles Ag32.1 g S x 1 mol S/32 g = 1 moles
Since Ag and S combine in a ratio of 2:1 (2 Ag to 1 S), the most Ag2S you can form is limited by moles of Ag. 1.096 moles Ag will react with 0.548 moles S ==> Ag2S. So the rest of the S will be left over and not used because there isn't enough Ag. Thus, the mass of resultant salt would be 197 g + 17.5 g = 214.5 g.
Wiki User
∙ 6y ago
Wiki User
∙ 6y agoTheoretical you have247,8 g Ag2S.
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Tarnish on silver is predominantly silver oxide and/or silver sulfide, both of which are insoluble in water. Magnesium, in accordance with its position in the electromotive series much higher than silver, displaces metallic silver from these compounds back onto the surface of the silverware. leaving behind oxides and/or sulfides of magnesium, which are sufficiently soluble in water to be easily washed away. This reaction is greatly facilitated if the tarnished silver and the magnesium are placed in contact with one another in an electrolyte solution in water.
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