what mass of AgBr is formed when a solution containing 3.45 g of KBr is mixed with a solution containing 7.28 g AgNO3?
mols AgNO3 = g/molar mass = ?
mols KBr = g/molar mass = ?
Determine limiting reagent and product.
To find the mass of AgBr formed when a solution containing 3.45 g of KBr is mixed with a solution containing 7.28 g AgNO3, we need to determine the limiting reactant.
1. Write the balanced chemical equation for the reaction:
2 AgNO3 + KBr → 2 AgBr + KNO3
2. Calculate the number of moles for each compound:
Number of moles of KBr = 3.45 g / molar mass of KBr
Number of moles of AgNO3 = 7.28 g / molar mass of AgNO3
3. Determine the limiting reactant:
The limiting reactant is the one that is completely consumed in the reaction. To find it, compare the moles of each compound using the stoichiometry of the balanced equation. The stoichiometric ratio between KBr and AgNO3 is 1:2.
Moles of KBr × 1 / 1 = Moles of AgNO3 × 2 / 2
4. Calculate the stoichiometric amount of AgBr formed from the limiting reactant:
The amount of AgBr formed is directly proportional to the limiting reactant. Use the stoichiometry of the balanced equation to find the moles of AgBr.
Moles of AgBr = Moles of limiting reactant × 2 / 1
5. Calculate the mass of AgBr formed:
Mass of AgBr = Moles of AgBr × molar mass of AgBr
By following these steps, you should be able to find the mass of AgBr formed in the given reaction.