Suppose that you could decompose. 0.250. Mall of AG2S into it. element. How many moles of silver do you have? And how many moles of Sulfur. will you have?

Answer 1

To determine the number of moles of silver (Ag) and sulfur (S) in 0.250 mol of Ag2S, we need to consider the ratio of atoms in the compound.

The chemical formula for silver sulfide (Ag2S) indicates that it consists of 2 silver atoms (Ag) for every 1 sulfur atom (S).

Thus, for 0.250 mol of Ag2S:
- The number of moles of silver (Ag) = 2 x (0.250 mol) = 0.500 mol
- The number of moles of sulfur (S) = 1 x (0.250 mol) = 0.250 mol

Therefore, you would have 0.500 moles of silver (Ag) and 0.250 moles of sulfur (S).

Answer 2

Calculate the masses of. AG2. and sulfur. Produced.

Answer 3

To calculate the masses of Ag2 and sulfur produced, we need to know the molar masses of silver (Ag) and sulfur (S).

The molar mass of silver (Ag) is approximately 107.87 g/mol.
The molar mass of sulfur (S) is approximately 32.06 g/mol.

For Ag2:
- The number of moles of Ag2 = 0.500 moles (as calculated earlier)
- The molar mass of Ag2 = 2 x molar mass of Ag
= 2 x 107.87 g/mol
= 215.74 g/mol

Therefore, the mass of Ag2 produced = (0.500 moles) x (215.74 g/mol)
= 107.87 g

For sulfur (S):
- The number of moles of S = 0.250 moles (as calculated earlier)
- The molar mass of S = 32.06 g/mol

Therefore, the mass of sulfur produced = (0.250 moles) x (32.06 g/mol)
= 8.02 g

Thus, the mass of Ag2 produced is approximately 107.87 g and the mass of sulfur produced is approximately 8.02 g.