How many atoms of silver are there in 2.639g of Ag2O?
how many moles?
double that, since Ag2O has two atoms for every molecule.
multiply by Avogadro's Number
Well, silver may be shiny, but counting atoms is no laughing matter! To answer your question, we need to do a little bit of math.
First, let's figure out the molar mass of Ag2O. The atomic mass of silver (Ag) is 107.87 g/mol, and oxygen (O) is 16.00 g/mol. So, the molar mass of Ag2O is (2 x 107.87) + (1 x 16.00) = 231.74 g/mol.
Next, we need to determine how many moles are present in 2.639 g of Ag2O. We divide the mass by the molar mass: 2.639 g / 231.74 g/mol = 0.0114 mol.
Since there are two silver atoms in one Ag2O molecule, we can multiply the number of moles by Avogadro's number (6.022 x 10^23), and then multiply that by 2. Thus, we get: 0.0114 mol x 6.022 x 10^23 atoms/mol x 2 = 1.376 x 10^22 atoms of silver.
So, there are approximately 1.376 x 10^22 atoms of silver in 2.639 g of Ag2O. That's quite a lot of tiny shiny particles if you ask me!
To determine the number of atoms of silver (Ag) in 2.639g of Ag2O, you need to follow these steps:
Step 1: Find the molar mass of Ag2O.
The molar mass of silver (Ag) is approximately 107.87 g/mol, and the molar mass of oxygen (O) is approximately 15.999 g/mol. Since Ag2O contains two Ag atoms and one O atom, we can calculate its molar mass as follows:
Molar mass of Ag2O = (2 * molar mass of Ag) + (1 * molar mass of O)
= (2 * 107.87 g/mol) + (1 * 15.999 g/mol)
= 216.74 g/mol
Step 2: Calculate the number of moles of Ag2O.
To calculate the number of moles, use the formula:
Number of moles = Mass / Molar mass
Number of moles of Ag2O = 2.639g / 216.74 g/mol
≈ 0.01215 mol
Step 3: Determine the number of moles of Ag.
Since there are two Ag atoms in one molecule of Ag2O, the number of moles of Ag is twice the number of moles of Ag2O. Therefore,
Number of moles of Ag = 2 * 0.01215 mol
≈ 0.0243 mol
Step 4: Calculate the number of atoms of Ag.
To calculate the number of atoms, use Avogadro's number, which is approximately 6.022 x 10^23 atoms/mol. Multiply the number of moles of Ag by Avogadro's number:
Number of atoms of Ag = Number of moles of Ag * Avogadro's number
= 0.0243 mol * 6.022 x 10^23 atoms/mol
≈ 1.46 x 10^22 atoms
Therefore, there are approximately 1.46 x 10^22 atoms of silver (Ag) in 2.639g of Ag2O.
To determine the number of atoms of silver in 2.639g of Ag2O, you'll need to follow these steps:
1. Determine the molar mass of Ag2O:
The molar mass of Ag (silver) is 107.87 g/mol, and O (oxygen) is 16.00 g/mol. Since there are two silver atoms in Ag2O, you'll need to multiply the molar mass of Ag by 2, and add the molar mass of O.
Molar mass of Ag2O = (2 * molar mass of Ag) + molar mass of O
= (2 * 107.87 g/mol) + 16.00 g/mol
= 232.74 g/mol
2. Convert the given mass of Ag2O to moles:
Use the formula: Moles = Mass / Molar mass
Moles of Ag2O = 2.639g / 232.74 g/mol
≈ 0.0113 mol (rounded to four decimal places)
3. Determine the number of moles of silver (Ag):
Since there are two silver atoms in one molecule of Ag2O, the number of moles of Ag will be twice the number of moles of Ag2O.
Moles of Ag = 2 * Moles of Ag2O
= 2 * 0.0113 mol
= 0.0226 mol
4. Calculate the number of atoms of silver:
The Avogadro's number states that 1 mol of any substance contains 6.022 x 10^23 entities (atoms, molecules, etc.). Therefore, to find the number of atoms of Ag, you need to multiply the number of moles of Ag by Avogadro's number.
Number of atoms of Ag = Moles of Ag * Avogadro's number
= 0.0226 mol * (6.022 x 10^23 atoms/mol)
= 1.36 x 10^22 atoms (rounded to two significant figures)
Therefore, there are approximately 1.36 x 10^22 atoms of silver in 2.639g of Ag2O.