Silver oxide is used in small batteries called button batteries (Figure below). It decomposes upon heating to form silver metal and oxygen gas.
2Ag2O(s) → 4Ag(s) + O2(g)
How many moles of silver are produced by the decomposition of 4.85 g of Ag2O?
mols Ag2O = grams/molar mass = ?
Using the coefficients in the balanced equation, convert mols Ag2O to mols Ag.
To calculate the number of moles of silver produced by the decomposition of Ag2O, you can use the molar mass of Ag2O and the given mass of Ag2O.
Step 1: Determine the molar mass of Ag2O.
The molar mass of Ag2O can be calculated by adding the atomic masses of silver (Ag) and oxygen (O).
Ag2O = (2 × Ag atomic mass) + (1 × O atomic mass)
The atomic masses of Ag and O are:
Ag = 107.87 g/mol
O = 16.00 g/mol
Substituting the values:
Ag2O = (2 × 107.87 g/mol) + (1 × 16.00 g/mol)
Ag2O = 215.74 g/mol + 16.00 g/mol
Ag2O = 231.74 g/mol
Step 2: Calculate the number of moles of Ag2O.
Given mass of Ag2O = 4.85 g
Number of moles of Ag2O = Given mass / Molar mass
Number of moles of Ag2O = 4.85 g / 231.74 g/mol
Calculating:
Number of moles of Ag2O = 0.0209 mol (rounded to four decimal places)
Step 3: Determine the number of moles of Ag produced.
From the balanced equation, 2 moles of Ag2O produce 4 moles of Ag.
So, 1 mole of Ag2O produces 2 moles of Ag.
Number of moles of Ag = Number of moles of Ag2O × (2 moles of Ag / 1 mole of Ag2O)
Calculating:
Number of moles of Ag = 0.0209 mol × (2 mol of Ag / 1 mol of Ag2O)
Number of moles of Ag = 0.0418 mol (rounded to four decimal places)
Therefore, the decomposition of 4.85 g of Ag2O produces 0.0418 moles of silver.
To determine the number of moles of silver produced by the decomposition of Ag2O, you need to use the molar mass of Ag2O and apply stoichiometry.
1. Find the molar mass of Ag2O:
The molar mass of silver (Ag) is 107.87 g/mol, and the molar mass of oxygen (O) is 16.00 g/mol.
Since Ag2O contains two silver atoms and one oxygen atom, the molar mass of Ag2O can be calculated as follows:
Molar mass of Ag2O = (2 * molar mass of Ag) + molar mass of O
= (2 * 107.87 g/mol) + 16.00 g/mol
= 231.74 g/mol
2. Convert the given mass of Ag2O to moles:
Moles of Ag2O = Mass of Ag2O / Molar mass of Ag2O
= 4.85 g / 231.74 g/mol
≈ 0.021 moles
3. Use the stoichiometry of the balanced chemical equation to determine the number of moles of silver produced:
From the balanced equation: 2Ag2O(s) → 4Ag(s) + O2(g)
For every 2 moles of Ag2O, 4 moles of Ag are produced.
Therefore, the number of moles of Ag produced can be calculated as:
Moles of Ag = (Moles of Ag2O) * (4 moles of Ag / 2 moles of Ag2O)
= 0.021 moles * (4 moles/2 moles)
= 0.042 moles
So, the decomposition of 4.85 g of Ag2O will produce approximately 0.042 moles of silver.