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?
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).
Calculate the masses of. AG2. and sulfur. Produced.
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.
To find the number of moles of silver (Ag) and sulfur (S) in the compound Ag2S, we need to consider the subscripts in the compound's formula.
Ag2S has a subscript of 2 for silver (Ag) and a subscript of 1 for sulfur (S).
The molar mass of Ag is 107.87 g/mol, and the molar mass of S is 32.07 g/mol.
To calculate the number of moles, we can use the following formula:
Number of moles = mass of the substance / molar mass
First, let's calculate the moles of silver (Ag):
Molar mass of Ag = 107.87 g/mol
Mass of silver (Ag) in Ag2S = 0.250 g
Number of moles of Ag = 0.250 g / 107.87 g/mol
Number of moles of Ag ≈ 0.00232 moles
Therefore, you have approximately 0.00232 moles of silver (Ag).
Next, let's calculate the moles of sulfur (S):
Molar mass of S = 32.07 g/mol
Mass of sulfur (S) in Ag2S = 0.250 g
Number of moles of S = 0.250 g / 32.07 g/mol
Number of moles of S ≈ 0.00779 moles
Therefore, you have approximately 0.00779 moles of sulfur (S).
In summary:
- Moles of silver (Ag): Approximately 0.00232 moles
- Moles of sulfur (S): Approximately 0.00779 moles