a sample of Ag2S has a mass of 62.4g. what mass of each element could be obtained by decomposing this sample?
Well, breaking up is never easy, especially when it comes to chemical compounds. But let's give it a shot and decompose Ag2S. Ag2S consists of silver (Ag) and sulfur (S).
Given that the sample has a mass of 62.4g, we need to find the mass of each element.
Ag2S is composed of two silver atoms (Ag) and one sulfur atom (S). So, using the atomic masses of silver and sulfur, we can determine the weight of each element.
The atomic mass of silver (Ag) is 107.9 g/mol and the atomic mass of sulfur (S) is 32.1 g/mol.
In Ag2S, we have two Ag atoms, so the mass of Ag is 2 x 107.9 g/mol = 215.8 g/mol.
The mass of Sulfur (S) is 32.1 g/mol.
So, in our 62.4g sample of Ag2S, we could obtain approximately 215.8g of silver (Ag) and 32.1g of sulfur (S).
Remember, this is just an estimate, and in reality, it may not be as simple as it sounds. Chemical reactions can be quite complex, so decomposition might not yield the exact amounts we calculate. But hey, nothing wrong with a little bit of humor and estimation, right?
To find the mass of each element obtained by decomposing a sample of Ag2S (silver sulfide), we need to calculate the amount of each element present in the compound.
The molar mass of Ag2S can be calculated as follows:
Ag = 107.87 g/mol (atomic mass of silver)
S = 32.07 g/mol (atomic mass of sulfur)
The molar mass of Ag2S can be calculated as:
(2 * Ag) + S = (2 * 107.87 g/mol) + 32.07 g/mol = 245.81 g/mol
Now, we can calculate the mass of each element in the sample using the concept of molar mass.
Let's suppose the mass of Ag2S is 62.4g.
To find the mass of silver (Ag), use the following calculation:
(2 * Ag) / Ag2S * 62.4g = (2 * 107.87 g/mol) / 245.81 g/mol * 62.4g = 54.47g
To find the mass of sulfur (S), use the following calculation:
S / Ag2S * 62.4g = 32.07 g/mol / 245.81 g/mol * 62.4g = 8.93g
Therefore, the mass of silver obtained by decomposing the sample is approximately 54.47g, and the mass of sulfur is approximately 8.93g.
To determine the mass of each element obtained by decomposing the Ag2S sample, we need to use the molar mass and stoichiometry of the compound.
1. Calculate the molar mass of Ag2S:
- Molar mass of one Ag atom = 107.87 g/mol
- Molar mass of one S atom = 32.06 g/mol
- Ag2S consists of two Ag atoms and one S atom.
- Molar mass of Ag2S = (2 x Ag atomic mass) + (1 x S atomic mass)
Therefore, Molar mass of Ag2S = (2 x 107.87 g/mol) + (1 x 32.06 g/mol) = 273.76 g/mol
2. Determine the stoichiometry in the compound:
- Ag2S contains two Ag atoms and one S atom.
- This means, in the compound, the ratio of Ag to S is 2:1.
3. Calculate the mass of each element:
- Given mass of Ag2S = 62.4 g
- To find the mass of Ag, we can use the ratio of Ag to Ag2S:
- Mass of Ag = (mass of Ag2S / molar mass of Ag2S) x (2 x molar mass of Ag)
- Substituting the known values:
Mass of Ag = (62.4 g / 273.76 g/mol) x (2 x 107.87 g/mol)
Mass of Ag = 30.8 g (rounded to one decimal place)
- To find the mass of S, we can use the ratio of S to Ag2S:
- Mass of S = (mass of Ag2S / molar mass of Ag2S) x (1 x molar mass of S)
- Substituting the known values:
Mass of S = (62.4 g / 273.76 g/mol) x (1 x 32.06 g/mol)
Mass of S = 14.4 g (rounded to one decimal place)
Therefore, by decomposing a sample of Ag2S weighing 62.4 g, approximately 30.8 g of Ag and 14.4 g of S could be obtained.
What is %Ag in Ag2S?
What is %S in Ag2S.
%Ag x 62.4 = g Ag
%S x 62.4 = g S.