Solution of 50g AgNO3 is mixed with 50g NaCl.
a) What mass of AgCl will you get?
b) which substance is in redundancy?
Another limiting reagent problem See you Hg + I2 problem above. This is done the same way.
To find the mass of AgCl (silver chloride) that will be formed, we need to determine which reactant will limit the amount of AgCl that can be produced. This is known as the limiting reactant.
a) To find the limiting reactant, we need to calculate the number of moles of each reactant:
1. Calculate the number of moles of AgNO3 (silver nitrate):
moles of AgNO3 = mass (AgNO3) / molar mass (AgNO3)
The molar mass of AgNO3 can be found using the periodic table. It consists of one silver (Ag) atom, one nitrogen (N) atom, and three oxygen (O) atoms. The atomic masses are: Ag = 107.87 g/mol, N = 14.01 g/mol, O = 16.00 g/mol.
molar mass (AgNO3) = (1 × 107.87) + (1 × 14.01) + (3 × 16.00) g/mol
2. Calculate the number of moles of NaCl (sodium chloride):
moles of NaCl = mass (NaCl) / molar mass (NaCl)
The molar mass of NaCl can be found using the periodic table. It consists of one sodium (Na) atom and one chlorine (Cl) atom. The atomic masses are: Na = 22.99 g/mol, Cl = 35.45 g/mol.
molar mass (NaCl) = (1 × 22.99) + (1 × 35.45) g/mol
3. Calculate the ratio of moles of AgNO3 to moles of NaCl. This will give us the stoichiometric ratio between the reactants:
stoichiometric ratio = moles of AgNO3 / moles of NaCl
4. Determine the limiting reactant:
The reactant with the smaller stoichiometric ratio will be the limiting reactant. Suppose the stoichiometric ratio is x:1, where x represents the smaller stoichiometric ratio.
5. Calculate the moles of AgCl that can be formed based on the limiting reactant:
moles of AgCl = x × moles of NaCl
6. Calculate the mass of AgCl using the moles of AgCl and the molar mass of AgCl:
mass of AgCl = moles of AgCl × molar mass (AgCl)
The molar mass of AgCl can be found using the periodic table. It consists of one silver (Ag) atom and one chlorine (Cl) atom. The atomic masses are: Ag = 107.87 g/mol, Cl = 35.45 g/mol.
molar mass (AgCl) = (1 × 107.87) + (1 × 35.45) g/mol
b) To determine which substance is in excess or redundancy, we compare the stoichiometric ratio obtained in step 3 to the actual ratio of the reactants. If the actual ratio is greater than the stoichiometric ratio, it means that substance is present in excess.
Now, let's calculate the mass of AgCl and determine the substance in redundancy:
1. Calculate the moles of AgNO3:
moles of AgNO3 = 50 g / molar mass (AgNO3)
2. Calculate the moles of NaCl:
moles of NaCl = 50 g / molar mass (NaCl)
3. Calculate the stoichiometric ratio:
stoichiometric ratio = moles of AgNO3 / moles of NaCl
4. Compare the stoichiometric ratio to the actual ratio of the reactants:
If the stoichiometric ratio is less than the actual ratio, AgNO3 is in excess.
If the stoichiometric ratio is greater than the actual ratio, NaCl is in excess.
By following these steps, you will find the mass of AgCl and determine which substance is in redundancy.