chemistry question. How many grams of silver sulfide can be produced by heating 45 grams of silver excess sulfer?
Here is a solve example stoichiometry problem. Just follow the steps. Post your work if you get stuck.
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To determine the number of grams of silver sulfide that can be produced, we need to consider the balanced chemical equation for the reaction between silver and sulfur.
The balanced chemical equation for the reaction between silver (Ag) and sulfur (S) can be represented as follows:
2 Ag + S → Ag2S
From the equation, we can see that 2 moles of silver react with 1 mole of sulfur to produce 1 mole of silver sulfide.
First, we need to calculate the moles of silver in 45 grams:
Molar mass of silver (Ag) = 107.87 g/mol
Moles of silver = Mass of silver / Molar mass of silver
Moles of silver = 45 g / 107.87 g/mol
Next, we need to determine the limiting reactant—whether silver or sulfur—since one of them is present in excess. In this case, sulfur is present in excess, so we will use the moles of sulfur to calculate the moles of silver sulfide.
Since the ratio of sulfur to silver sulfide in the balanced equation is 1:1, the moles of sulfur and the moles of silver sulfide produced will be the same.
Finally, we convert the moles of silver sulfide to grams:
Molar mass of silver sulfide (Ag2S) = (107.87 g/mol × 2) + 32.07 g/mol
Moles of silver sulfide = Moles of sulfur = Moles of silver
Mass of silver sulfide = Moles of silver sulfide × Molar mass of silver sulfide
Once you have the mass in grams, you will have the answer to your question.