Question

Table 4.1

Mask of flask + iodine: 77.443g

-Mass of empty flask: 75.41g

=Mass of iodine used: 2.032g

Mass of zinc used: 2.055g

Table 4.2

Mass of beaker + crystals: 110.014g

-Mass of beaker: 107.482g

=Mass of crystals formed: 2.532g

Table 4.3

Mask of flask + solid; 1st weighing: 76.845g

Mask of flask + solid; 2nd weighing: 76.844g

Mass of excess reactant recovered: ?

I solved questions 1-4

2. How many grams of excess reactant remained after reaction: 76.844g-75.41g = 1.434g

3. How many grams of zinc reacted: 0.621g

4. How many moles of zinc reacted: 0.009 mol

I'm stuck on the questions that come:

5. How many grams of Iodine, I2, reacted? Is it 2.532 or 1.911g

6. How many moles of Iodine2, reacted? (show calculations)

7. How many moles of iodine, I^-, reacted? (show calculations)

8. Using the moles of zinc and I^- that reacted, the empirical formula for zinc iodide is (show calculations):

9. What is the charge on a zinc ion in the ionic compound?

11. Using the moles of Iodine (i2) that reacted, calculate the theoretical yield of zinc iodide in your experiment. (show calculation)

12. What is the percentage yield of zinc iodide in your experiment? (show calculations)

Answer 1