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 (NaCL.

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???

excuse me the product was AgCl not NaCl, that probably does not change the step but thought I would correct myself.

Answered above.

To calculate the theoretical yield in this lab experiment, you need to determine the limiting reagent first. The limiting reagent is the reactant that is completely consumed and determines the maximum amount of product that can be formed.

Here's how to find the theoretical yield step by step:

1. Write the balanced chemical equation for the reaction occurring in the lab:
AgNO3 + NaCl → AgCl + NaNO3

2. Determine the moles of each reactant used:
- H2O: Since it is a solvent, we can ignore it for the stoichiometry calculation.
- AgNO3: Convert the mass given (4g) into moles using the molar mass of AgNO3 (169.87 g/mol).
- NaCl: Convert the mass given (8g) into moles using the molar mass of NaCl (58.44 g/mol).

3. Use stoichiometry to find the moles of product formed:
- Based on the balanced equation, the mole ratio between AgNO3 and AgCl is 1:1. So, the number of moles of AgCl formed is the same as the number of moles of AgNO3 used.

4. Convert the moles of AgCl formed into grams:
- Multiply the moles of AgCl by the molar mass of AgCl (143.32 g/mol) to find the theoretical yield in grams.

5. Compare the theoretical yield with the actual yield:
- Calculate the percent yield by dividing the actual yield (6.7496g) by the theoretical yield (calculated in step 4), then multiplying by 100. This will give you the percentage of the theoretical yield that you obtained.

Note: It's important to ensure that the stoichiometric coefficients in the balanced equation are correct and that the reaction proceeds as expected.