How many grams of AgBr are produced from 2.50g of cobalt II bromide?
Using this chemical reaction:
AgNO3+CoBr->CoNO3
You need to work on the equation. An oxidation state of +1 is unusual for Co.
To find out how many grams of AgBr are produced from 2.50g of cobalt II bromide, we need to use stoichiometry.
1. Start by writing the balanced chemical equation:
CoBr + AgNO3 -> CoNO3 + AgBr
2. Determine the molar mass of cobalt II bromide (CoBr):
Cobalt (Co) has a molar mass of 58.93 g/mol.
Bromine (Br) has a molar mass of 79.90 g/mol.
So, the molar mass of CoBr is 58.93 + 79.90 = 138.83 g/mol.
3. Convert the given mass of CoBr (2.50g) into moles:
Number of moles = Mass / Molar mass
Number of moles of CoBr = 2.50g / 138.83 g/mol
4. Use the balanced equation to find the moles of AgBr produced.
From the balanced equation, we see that 1 mole of CoBr reacts with 1 mole of AgBr.
This means that the mole ratio is 1:1.
5. Convert the moles of CoBr to moles of AgBr:
Since the mole ratio is 1:1, the number of moles of AgBr produced is the same as the number of moles of CoBr.
6. Finally, calculate the mass of AgBr produced:
Mass = Number of moles x Molar mass
Mass of AgBr = Number of moles of AgBr x Molar mass of AgBr
To find the molar mass of AgBr:
Silver (Ag) has a molar mass of 107.87 g/mol.
Bromine (Br) has a molar mass of 79.90 g/mol.
So, the molar mass of AgBr is 107.87 + 79.90 = 187.77 g/mol.
Substituting the given values into the equation:
Mass of AgBr = Number of moles of AgBr x Molar mass of AgBr
Mass of AgBr = Number of moles of CoBr x Molar mass of AgBr
Now, you can calculate the mass of AgBr produced.