AgNO3+FeCl3 --> AgCl+Fe(NO3)3
In an experiment, it was planned to mix a solution containing 25 g of AgNO3 with another solution containing 45 g of FeCl3.
a) What is the maximum number of moles of AgCl that could be obtained?
I already found the limiting reagent, I just need to know how to set this part up.
To determine the maximum number of moles of AgCl that could be obtained, we need to identify the limiting reagent between AgNO3 and FeCl3. The limiting reagent is the reactant that is completely consumed during the reaction and determines the maximum amount of product that can be formed.
To find the limiting reagent, we can compare the number of moles of each reactant with their respective stoichiometric coefficients. In this case, the balanced equation tells us that the stoichiometric coefficient of AgNO3 is 1, while the stoichiometric coefficient of FeCl3 is 3.
Let's calculate the number of moles of AgNO3 and FeCl3:
Moles of AgNO3 = mass / molar mass
Moles of AgNO3 = 25 g / (107.87 g/mol) (molar mass of AgNO3)
Moles of FeCl3 = mass / molar mass
Moles of FeCl3 = 45 g / (162.2 g/mol) (molar mass of FeCl3)
Now that we have the moles of each reactant, we can compare their ratios to determine the limiting reagent. To do this, we divide the moles of AgNO3 by its stoichiometric coefficient (1) and divide the moles of FeCl3 by its stoichiometric coefficient (3):
Moles of AgNO3 / stoichiometric coefficient = 25 g / (107.87 g/mol) / 1
Moles of FeCl3 / stoichiometric coefficient = 45 g / (162.2 g/mol) / 3
By comparing these ratios, we can determine which is smaller. The reactant with the smaller ratio will be the limiting reagent.
Once we have identified the limiting reagent, we can use its moles to calculate the maximum number of moles of AgCl that could be obtained. To do this, we use the stoichiometry of the balanced equation:
Moles of AgCl = Moles of limiting reagent x Stoichiometric coefficient of AgCl
In this case, the stoichiometric coefficient of AgCl is 1.
By following these steps, you will be able to calculate the maximum number of moles of AgCl that could be obtained.
To find the maximum number of moles of AgCl that could be obtained, we need to determine the limiting reagent. The limiting reagent is the reactant that is completely consumed and determines the maximum amount of product that can be formed.
First, let's convert the given masses of AgNO3 and FeCl3 into moles by using their respective molar masses:
AgNO3:
Molar mass of AgNO3 = 107.87 g/mol + 14.01 g/mol + (3 * 16.00 g/mol) = 169.87 g/mol
Moles of AgNO3 = Mass of AgNO3 / Molar mass of AgNO3
= 25 g / 169.87 g/mol
FeCl3:
Molar mass of FeCl3 = 55.85 g/mol + (3 * 35.45 g/mol) = 162.2 g/mol
Moles of FeCl3 = Mass of FeCl3 / Molar mass of FeCl3
= 45 g / 162.2 g/mol
Next, we can determine the stoichiometric ratio of AgNO3 to AgCl from the balanced chemical equation:
1 mol AgNO3 : 1 mol AgCl
Now, we can compare the moles of AgNO3 to AgCl to see which reactant is the limiting reagent.
The number of moles of AgCl that could be formed will be equal to the number of moles of the limiting reagent.
Therefore, the maximum number of moles of AgCl that could be obtained will be equal to the number of moles of the limiting reagent.