Aluminum and Silver Sulfate
By: Mason Prough
What type of reaction is this?
This is a Single Replacement reaction.
Balanced Equation WITH states of matter
Al2 + 3Ag2(SO4) ===> Al2(SO4)3 + 6Ag
IUPAC name for each reactant and product
Molar Mass for each reactant and product
Silver: Silver has a subscript of 2 thanks to the sulfate. Now, you multiply the atomic mass of silver, 107.9 g/mol, by 2 making the result 215.8 g/mol.
Sulfur: There is only one sulfur molecule, so the atomic mass is the molar mass. 32.06 g/mol.
Oxygen: There are 4 oxygen molecules so, you multiply the atomic mass by 4 making 63.99 g/mol.
Aluminum: This time, Aluminum has a subscript of 2. You just multiply the atomic mass by 2 making it 53.97 g/mol.
Sulfur: This part can be tricky, but it easy. The entire compound of Sulfate now has a subscript of 3 since Aluminum has a superscript of 3. This now makes 3 times the atomic mass which turns into 96.18 g/mol.
Oxygen: Like stated before, sulfate has a subscript of 3, so you multiply oxygen's atomic mass by 3, making it 191.9 g/mol.
Silver: Silver is all alone when replaced with Aluminum, so the molar mass is the atmoic mass of 107. 8 g/mol.
Mole to mole conversions
12.1 mol Ag x 3 Ag2(SO4) / 6 mol Ag = 6.05 mol Ag2(SO4)
Mass to Mass Conversion
Limiting and Excess reactans
12.18 g Ag2(SO)4 x 6 mol Ag x 107.87 g Ag / 311.82 g Ag2(SO4) x 3 mol Ag = 8.427 g Ag
Usually the smaller answer is the Limiting Reactant