a sample of silver chromate has a mass of 78.6 grams?
Nice. Is this a question?
yes it isa question
You need to explain it. It doesn't appear to be a question to me.
To determine the molar mass of silver chromate, we first need to know the chemical formula of silver chromate. The formula for silver chromate is Ag2CrO4.
To calculate the molar mass, we need to add up the atomic masses of each element in the formula.
The atomic mass of silver (Ag) is approximately 107.87 grams per mole.
The atomic mass of chromium (Cr) is approximately 52.00 grams per mole.
The atomic mass of oxygen (O) is approximately 16.00 grams per mole.
The formula Ag2CrO4 contains two silver atoms, one chromium atom, and four oxygen atoms.
To calculate the molar mass, we multiply the atomic mass of each element by the number of atoms and then add them up:
(2 * 107.87 g/mol) + (1 * 52.00 g/mol) + (4 * 16.00 g/mol) = 215.74 g/mol + 52.00 g/mol + 64.00 g/mol = 331.74 g/mol
Therefore, the molar mass of silver chromate (Ag2CrO4) is approximately 331.74 grams per mole.
The mass of the sample given is 78.6 grams. To find the number of moles in the sample, we divide the mass of the sample by the molar mass:
78.6 g ÷ 331.74 g/mol ≈ 0.237 moles
Therefore, the sample of silver chromate has approximately 0.237 moles.