Pg. 973 #55, 57, 58, 61

Gas Variable Pogil

Pg. 926 #11-16

Boyle's Law Lab

Stoichiometry Lab #3

Purpose:

Determine the Percent Yield of multiple reactions.

Procedure:

1. Mass .5g NaOH

2. Mass 2.5g CuSO4*5H2O

3. Dissolve CuSO4*5H2O and NaOH separately, each in in 50mL H2O

4. Mix two solutions together

5. Heat very slowly

6. Filter with vacuum filtration

7. Rinse into pan and place in oven

Data:

Mass of NaOH: .50g

Mass of CuSO4*5H2O: 1.25g

Mass of Cu(OH2):

Calculations:

Limiting Reagent/Reactant in Excess:

Percent Yield:

Conclusion:

Penguins approve this message. We found that the percent yields of the following reactions were 77.87%. Determining the limiting reactions in excess we were able to find that there were only .005 moles of Copper Oxate in the reaction. Using the mass of the Copper Oxate and the theoretical yield of the same formula we were able to find the the the the percent yield of the reaction. This conclusion is brought to you by the Penguins International Sanctuary of Seas or better known as PISS. Thank You.

Stoichiometry Lab #2

BPurpose:

Determine the percent yield of a single replacement reaction.

Procedure:

1. Mass .5g Fe

2. Mass 2.5g CuSO4*5H2O

3. Dissolve CuSO4*5H2O in 100mL H2O

4. Heat to dissolve, then add Fe (don't boil)

5. After 15min. decant into yogurt container

6. Rinse into pan and place in oven

Data: 

Mass of Fe: .51g

Mass of CuSO4*5H2O: 2.50g

Mass of Cu: .45g

Calculations:

Determine limiting reagent and Reactant in excess:

Percent Yield:

Conclusion:

It's the End of the World as we know it! And I feel like I didn't do this lab. The percent yield of this single replacement reaction is 80.36%. First, we determined the penguins limiting reagent and reactant in excess. Then with the mass of copper and theoretical yield of copper, we found the percent yield. Then everybody everybody living now everybody everybody sucks

Stoichiometry Problems From Blog

Pg. 815 #28-33, 37, 38

Pg. 811 #26, 27

Stoichiometry Lab #1

Purpose:

Determine the percent yield of a double replacement reaction.

Procedure:

1. Mass evaporating dish.

2. Mass 2g Na2CO3.

3. Add HCl slowly until bubbling stops.

4. Heat until all water has evaporated

5. Mass NaCl

Data:

Mass of evaporating dish: 46.54g

Mass of Sodium Chloride: 2.00g

Mass of NaCl: 1.67g

Calculations:

Balanced Equation:

Theoretical Yield of NaCl:

Percent Yield:

1.67g/2.21g x100=75.57%yield

Conclusion:

This is the end. Just hold your breath and count to ten. Feel the earth move and bend. Just kidding. In this lab a chemical reaction produced saltwater which was then evaporated to find the mass or yield of salt. There was significant error because the amount in the lab was only 75.57% of the theoretical yield in this equation. Penguins.

Pg. 826 #45, 46

Pg. 802 #23

Pg. 793. #11-16