suppose that you could decompose 0.250 mole of Ag2s into its elements
a.How many moles of silver would you have? how many moles of sulfur would you have?
b. how many moles of ag2s are there in 38.8 g of AG2S? how many moles of silver and sulfur would be produced from this amount of Ag2S?
c. caculate the masses of silver and sulfur produced in(b)
Ag2S ==> 2Ag^+ + S^-2
0.250 moles Ag2S will give you 2x0.250 moles Ag because the formula tells you there are 2 Ag ions for each Ag2S molecule. The moles of sulfur will be 1x0.250 because there is 1 atom S for each molecule of Ag2S.
See my previous response for moles from 38.8 g.
Part three is a stoichiometry problem. Post your thoughts and what you don't understand if you get stuck and we can help you through.
Ag2S==> 2Ag^+ + S^-2
Convert grams Ag2S to moles Ag2S.
Convert moles Ag2S to moles Ag.
Convert moles Ag2S to moles S^-2
Convert moles Ag to grams. grams = moles x molar mass.
Convert moles S to grams. grams = moles x molar mass.
Post your work AND EXPLAIN FULLY any step you don't understand.
Wow, almost 13 years later
pH? 40.0ml of 0.100M when 20.0ml of 0.250M
a. If you could decompose 0.250 mole of Ag2S, you would have 0.500 moles of silver. Since Ag2S contains two silver atoms, when it decomposes, it will release two moles of silver.
As for sulfur, since Ag2S contains one sulfur atom, when it decomposes, you would have 0.250 moles of sulfur.
b. To find the number of moles of Ag2S in 38.8 g, we need to use its molar mass. The molar mass of Ag2S is 247.8 g/mol. Therefore, the number of moles of Ag2S is:
38.8 g / 247.8 g/mol = 0.1567 mol
Since Ag2S contains two moles of silver per mole of Ag2S, you would have:
0.1567 mol Ag2S * 2 mol Ag/mol Ag2S = 0.3134 mol Ag
Similarly, Ag2S contains one mole of sulfur per mole of Ag2S, so you would have:
0.1567 mol Ag2S * 1 mol S/mol Ag2S = 0.1567 mol S
c. To calculate the masses of silver and sulfur produced, we need to multiply the number of moles by their respective molar masses. The molar mass of silver (Ag) is 107.87 g/mol and the molar mass of sulfur (S) is 32.06 g/mol.
Mass of silver produced = 0.3134 mol Ag * 107.87 g/mol Ag = 33.78 g Ag
Mass of sulfur produced = 0.1567 mol S * 32.06 g/mol S = 5.02 g S
So, from 38.8 g of Ag2S, you would produce approximately 33.78 g of silver and 5.02 g of sulfur.
To answer these questions, we need to use the molar ratio between Ag2S, Ag, and S.
a. The formula of Ag2S indicates that for every 1 mole of Ag2S, there are 2 moles of Ag and 1 mole of S. Since we have 0.250 moles of Ag2S, we can calculate the number of moles of Ag and S by multiplying the given amount by the respective ratios:
Number of moles of Ag = 0.250 moles Ag2S * 2 moles Ag / 1 mole Ag2S
= 0.500 moles Ag
Number of moles of S = 0.250 moles Ag2S * 1 mole S / 1 mole Ag2S
= 0.250 moles S
b. To find the number of moles of Ag2S in 38.8 g, we need to convert the mass of Ag2S to moles by using its molar mass. The molar mass of Ag2S is calculated by summing the atomic masses of the elements:
Molar mass of Ag2S = (2 * atomic mass of Ag) + atomic mass of S
= (2 * 107.87 g/mol) + 32.06 g/mol
= 107.74 g/mol + 32.06 g/mol
= 139.80 g/mol
Number of moles of Ag2S = 38.8 g Ag2S * (1 mol / 139.80 g)
= 0.2779 mol
Using the same molar ratios as in part (a):
Number of moles of Ag = 0.2779 mol Ag2S * 2 moles Ag / 1 mole Ag2S
= 0.5558 moles Ag
Number of moles of S = 0.2779 mol Ag2S * 1 mole S / 1 mole Ag2S
= 0.2779 moles S
c. To calculate the masses of silver and sulfur produced, we can multiply the respective number of moles by their molar masses:
Mass of Ag = 0.5558 moles Ag * 107.87 g/mol
= 59.96 g
Mass of S = 0.2779 moles S * 32.06 g/mol
= 8.918 g
Therefore, in part (b), 38.8 g of Ag2S would produce approximately 59.96 g of Ag and 8.918 g of S.