The procedure of the lab. please calculate the stoichiometric amount of aluminum foil needed to use to finish the reacti

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The procedure of the lab. please calculate the stoichiometric
amount of aluminum foil needed to use to finish the reaction in
gram?
USO4 and Al
1. Measure 30mL of 1M CuSO4 in the 50mL graduated cylinder. Record
the volume to the
tenth’s place. Pour into a beaker.
2. Calculate the stoichiometric amount of aluminum foil needed to
completely react to your
CuSO4. Record this value. Subtract 10%. The Aluminum foil will be
limiting in this
reaction.
a. I.e. If 2.70g of Al is the stoichiometric amount of aluminum
foil needed, then:
2.70g - 10% (0.27g) = 2.43g Al would be used.
3. Measure out the amount of aluminum foil calculated in 2, above,
on the scale. Record
the exact mass used.
4. Tear the aluminum foil into small pieces to increase the surface
area of the reaction.
5. Place the aluminum foil into the beaker of CuSO4.
what is the amount of aluminum foil needed in this lab to
complete reaction?
2. Compare the results to see which reactant produces less product. The sodium will produce less product therefore the Sodium is the limiting reactant. "*remember the limiting reagent is ALWAYS a reactant 3. Identify the theoretical yield. The theoretical yield 0.494 g H2 4. Calculate the percent yield. The % yield (Actual yield/ Theoretical yield) 100- (0.4059/0 494g)*100=82.0% This lab will require you to take each calculation stepwise in order to show your understanding of what you are calculating Procedure CuSO4 and Al 1. Measure 30ml. of 1M CuSO4 in the 50ml graduated cylinder. Record the volume to the tenth's place. Pour into a beaker your 2. Calculate the stoichiometric amount of aluminum foil needed to completely react to CuSO. Record this value Subtract 10% The Aluminum foil will be limiting in this reaction a Le. If 2.70g of Al is the stoichiometric amount of aluminum foil needed, then

2.70g-10% (0.27g)=2.43g Al would be used. 3. Measure out the amount of aluminum foil calculated in 2, above, on the scale. Record the exact mass used. 4. Tear the aluminum foil into small pieces to increase the surface area of the reaction. 5. Place the aluminum foil into the beaker of CuSO4 6. Record observations. 7. Add a large pinch of NaCl to the beaker. (This acts as an electron bridge therefore the exact amount is NOT necessary to know.) 8. Take a picture of the reaction. Your ID should be in the picture. 9. Record observations 10. Mass a cone coffee filter and record the mass 11. When the reaction is complete, pour the solution and solids through the massed cone filter. The solids are being collected to be dried and massed 12. Rinse the solids with fresh water. The idea is to remove any residual ions so that all that is left is the solid a. I found that I could use a binder clip to hold the filter to the edge of a glass while the liquid drained. Alternatively, I suspended the filter over my beaker by using a binder clip to hold the filter on a chopstick that was balanced on two glasses. Be creative. Show me what you did