Lab: Empirical Formula of Copper Oxide
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Step 1 = 5g of copper sulfate pentahydrate added to 50mL beaker
Mass of beaker & contents = 90.000g
Step 2 = add 30mL water to copper sulfate pentahydrate
mass= 120.000g
Step 3 = Add 10mL 6M Sodium Hydroxide
Observed that the mass increased to 131.273g
Mass of empty test tube = 27.400g
Mass of test tube after heating = 28.993g
Need to know the following:
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, which is 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
E. Calculate the molar ratio of copper to oxygen from: (moles copper) / (moles of oxygen in the copper oxide)
F. According to this molar ratio, what is the empirical formula of copper oxide?
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This solution offers detailed step-wise calculations and chemical reactions associated with a lab experiment, to determine empirical formula.
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