Solid lead(ii) iodide was prepared by reacting 65.0 ml of a solution containing 0.218 m lead(ii) ions with 80.0 ml of a solution containing 0.265 m iodide ions. if the actual yield of the reaction was 3.26 g, which choice is closest to the %yield of the reaction?

The balanced chemical reaction will be as follows:

To determine the % yield, first calculate the theoretical yield.

Molairty and volume of is 0.218 M and 65 mL respectively. Convert it into number of moles as follows:

Here, volume should be in L thus,

Similarly, calculate number of moles of iodide ion,

Now, from the balanced chemical equation, 1 mole of   gives 1 mol of , thus, 0.01417 mol will give 0.01417 mol of .

Also, 2 mole of will give 1 mole of thus, 0.0212 mol will give,

Molar mass of is 461.01 g/mol calculating mass of obtained from   and as follows:

From :

Similarly, for :

Here, is limiting reactant as it produced less amount of    as compared with .

Theoretical yield is amount of product obtained from limiting reactant thus, theoretical yield will be 4.8867 g.

Percentage yield can be calculated as follows:

Actual yield is 3.26 g thus, percentage yield will be:

=66.7%

Therefore, % yield will be 66.7%

i believe you are right for all except the 3rd ( look at sqdancefan his answer is much better)

the correct option is c.

isotopes refers to different forms of the same element with the same atomic number but different mass number as a result of difference in their neutron numbers. isotopes have different relative atomic mass but share the same chemical properties.