To verify the previous experiment, the chemistry student carried out the next experiment and recorded the data for you in the following Data Table. Directions: Place 100 mL of filtered, saturated PbCl2 in a 150 mL beaker and put it under a dryer to evaporate the water. Record the necessary data in the Data Table.

Complete the Data Table.

Since the data allows it, you should use 3 significant digits for all your answers.

Molecular weight of PbCl2 = 278 g/mole

Mass of beaker + PbCl2 = 62.19 g

Mass of beaker = 57.77 g

first, consult an activity series chart to determine if al is more reactive than fe. it is, so it will replace the fe. now, one can continue with the problem.

next, make sure you have a correctly balanced equation.

3feo + 2al ==> 3fe + al2o3

now, determine which reactant (feo or al) is in limiting supply.

moles feo present = 125 g x 1 mole/71.8 g = 1.74 moles

moles al present = 25.0 g x 1 mole/26.98 g = 0.927 moles

since from the balanced equation, it take 3 mol feo for every 2 mol al, al will be limiting.

you can determine this simply by dividing moles of each by their coefficient in the balanced equation. for example: 1.74/3 = 0.58 and 0.927/2 = 0.464. al is less, so it is limiting.

finally, using the stoichiometry in the balanced eq. determine mass of fe that can be produced from 0.927 moles of al.

0.927 moles al x 3 moles fe/2 moles al x 55.8 g/mole = 77.6 g

points

explanation:

b.false that your answer