CaCl2 reacts with AgNO3 in aqueous solutions to produce a precipitate of AgCl that can be filtered and

weighed. The balanced equation for the reaction is:
CaCl2 (aq) + 2 AgNO3 (aq) → 2 AgCl (s) + Ca(NO3)2 (aq)
I got 59.22%.

Good, however, something is missing here.

Suppose you have a mixture that contains CaCl2, plus other compounds that do not react with AgNO3. If 0.2918

g of the mixture yields 0.4462 g of AgCl, what is the percentage of CaCl2 in the mixture. Thats whats missing.

See my response above.

To calculate the percentage yield of a reaction, you need to compare the actual yield (the mass of AgCl obtained in this case) with the theoretical yield (the maximum possible mass of AgCl that could be obtained according to the balanced equation).

To calculate the theoretical yield, you need to determine the limiting reactant. The limiting reactant is the reactant that is completely consumed and determines the amount of product that can be formed. In this case, we have CaCl2 and AgNO3 as the reactants.

To find the limiting reactant, you need to compare the molar ratios of the reactants in the balanced equation with the actual amounts used. You didn't provide any information about the amounts used, so I'll assume you have an equal amount of both reactants.

According to the balanced equation, 1 mole of CaCl2 reacts with 2 moles of AgNO3. If you have equal amounts of both reactants, you can assume that the moles of CaCl2 and AgNO3 are the same.

Once you determine the limiting reactant, you can calculate the theoretical yield of AgCl. From the balanced equation, you can see that 1 mole of CaCl2 produces 2 moles of AgCl. So, the theoretical yield of AgCl can be calculated by multiplying the moles of the limiting reactant by the molar mass of AgCl (107.87 g/mol).

Next, you need to find the actual yield of AgCl that you obtained by filtering and weighing.

Finally, you can calculate the percentage yield by dividing the actual yield by the theoretical yield and multiplying by 100.

Since you didn't provide any information about the actual yield or the amounts used, it's not possible for me to calculate the percentage yield of 59.22% accurately. Please provide the necessary information for a more precise calculation.