I am trying to find the theoretical yield for this lab I am working on. The steps to finidng it would be great.
In my lab I took 40mls of H2O + 4g of AgNO3+ 8g of NaCL then I stirred it and filtered in a buchner funnel to be left with 6.7496g of silver chloride (AgCL)
The question I am asked is to find the percent yield which I know how to do, and since I have the actual yield I just cannot recall how to get the theoretical yield, do I do something with moles???
I assume your actual yield is 6.7496 g AgCl.
Theoretical yield:
AgNO3 + NaCl ==> AgCl + NaNO3.
Convert AgNO3 to moles. moles = g/molar mass.
Convert NaCl to moles.
Now you must determine which reagent (AgNO3 or NaCl0 is in excess. Since the reaction shows a 1:1 ratio for moles AgNO3 vs moles NaCl, the one with the fewer moles will be the limiting reagent. My guess is that will be AgNO3.
Then convert moles AgNO3 to moles AgCl and go from there to grams AgCl. That will be the theoretical yield. I did a quick calculation (but you need to check it out) and came out with about 3.4 g AgCl as theoretical yield. If I didn't goof, then you have something extra in your product for you have over 100% yeild and that's a no, no. My guess would be you didn't wash all of the NaNO3 and excess NaCl out of the product.
In my math I took 8g of AgNo3/1.69.8731 g/mol=.0471 mol of AgNo3
Then since there is only one AgNO3 and one AgCL, then AgCl's has a mol of .0471, multiply that by its molecular weight of 143.321 and I receive 6.75 grams. not 3.4, where did I did I do something wrong?
Disregard this question I figured it out, THanks for all the help Bob
To find the theoretical yield, you need to calculate it based on the balanced chemical equation for the reaction. Here are the steps to find the theoretical yield:
1. Write the balanced chemical equation for the reaction:
AgNO3 + NaCl -> AgCl + NaNO3
2. Determine the molar masses of the reactants and products:
- Molar mass of AgNO3 = atomic mass of Ag (107.87 g/mol) + atomic mass of N (14.01 g/mol) + (3 * atomic mass of O (16.00 g/mol)) = 169.87 g/mol
- Molar mass of NaCl = atomic mass of Na (22.99 g/mol) + atomic mass of Cl (35.45 g/mol) = 58.44 g/mol
- Molar mass of AgCl = atomic mass of Ag (107.87 g/mol) + atomic mass of Cl (35.45 g/mol) = 143.32 g/mol
3. Calculate the number of moles of each reactant used in the reaction:
- Moles of AgNO3 = mass of AgNO3 (4g) / molar mass of AgNO3 (169.87 g/mol)
- Moles of NaCl = mass of NaCl (8g) / molar mass of NaCl (58.44 g/mol)
4. Determine the limiting reactant:
Since the reaction is stoichiometrically balanced, we can compare the moles of each reactant to determine the limiting reactant. The reactant that produces the least amount of product is the limiting reactant.
- Moles of AgCl produced from AgNO3 = Moles of AgNO3 * (1 mole of AgCl / 1 mole of AgNO3)
- Moles of AgCl produced from NaCl = Moles of NaCl * (1 mole of AgCl / 1 mole of NaCl)
The limiting reactant will be the one that produces the smaller amount of AgCl. Let's assume the limiting reactant is AgNO3.
5. Calculate the theoretical yield of AgCl:
- Theoretical yield of AgCl = Moles of AgCl produced (from AgNO3) * molar mass of AgCl (143.32 g/mol)
6. Convert the theoretical yield to grams:
Theoretical yield (in grams) = Theoretical yield of AgCl * molar mass of AgCl (143.32 g/mol)
By following these steps, you will be able to calculate the theoretical yield of AgCl.