1. Record and calculate the following about the copper sulfate pentahydrate (a)

Question

1. Record and calculate the following about the copper sulfate pentahydrate (a) mass of CuSO4*5H2O (g) (b) Molecular weight of CuSO4*5H2O (c)Moles of CuSO4*5H2O (d)Moles of Cu in the copper sulfate salt:
2.Calculate the following for the oxygen: (a)The initial mass of copper in the moles of copper from the copper sulfate salt (MW of Cu= 63.55 g/mole) (g) (b)The mass of copper oxide obtained (g) (the mass of the copper oxide in the test tube after heating over Bunsen burner to remove water) (c) The gain in mass, equal to the added mass of oxygen (g) (d) The number of moles of oxygen in the copper oxide, given a molecular weight of oxygen (O) equal to 16.00 g/mole
3. Calculate the molar ratio of copper to oxygen from: (moles copper) / (moles of oxygen in the copper oxide) 4. According to this molar ratio, what is the empirical formula of copper oxide? 5. Calculate the yield of copper oxide: (a) Expected number of moles of copper oxide (using the empirical formula of copper oxide and the starting moles of Cu) (b) Actual mass of copper oxide (c) Actual moles of copper oxide (dividing the mass by the MW of the copper oxide)
6. Calculate the percent difference between the expected and actual values for the moles of copper oxide, according to the following equation: % difference= |expected moles - actual moles| / expected moles * 100 7. Is there a percent difference between your actual and expected? If there was a difference, what could account for this difference?
Materials Used -50 mL beaker -balance - 5 g Copper sulfate pentahydrate -30 mL of water test tube Method 2 1.Place empty beaker on balance and record mass: 85.000 g 2.Take empty beaker off balance, place on lab area and then add 5 g of Copper sulfate pentahydrate 3.Place beaker and copper sulfate pentahydrate unto balance and record mass: 90.00 0 g 4.Dissolve copper sulfate pentahydrate by adding 30 mL of water 5.Then add 10 mL of 6M sodium hydroxide Reaction: Color change from blue to transparent 6. Transfer the liquid content to a new beaker and the hard material in the old beaker 7. Place a test tübe on the balance and record mass: 27.400 g Place on top of Bunsen bumer ang then allow to cool on workbench before recording n ew mass: 28.993 g

Explanation / Answer

Multiple questions in the same post. Post your questions per separate so you will have a better and faster answer. I'll answer 1 and part of 2.

1a. Mass is 5 g as it appears in the procedure.

1b. Molecular weight would be:
Cu = 63.55 g/mol; O = 16 g/mol; S = 32 g/mol; H = 1 g/mol
MW CuSO4*5H2O = (63.55)+(32)+(4*16)+(10*1)+(5*16) = 233.55 g/mol

1c. to get the moles, you'll need the MW and the mass so:
moles = 5 / 233.55 = 0.0214 moles

1d. To get the moles of Cu:
In 233.55 ------------ 63.5
in 5 ----------------------X
x = 63.5 * 5 / 233.55 = 1.3595 g (Answer for part a of 2)
moles of Cu = 1.3595 / 63.5 = 0.0214 moles

Post your other question in another question thread.

Hope this helps

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