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3.09 Honors Chem Online

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3.09 Honors Chem Online
3.09 Honors:

Here is sample data and how you would do the calculations. Of course, you will need to use your data, but you can follow along step-by-step.

In the lab, you must record the following measurements: mass of your empty crucible mass of your crucible and the hydrate (the original chemical) mass of the crucible and chemical after heating(which is the dehydrate)

The other two in the data table are calculated (mass of hydrate and mass of dehydrate)
SAMPLE DATA – YOU MUST USE YOUR DATA FOR CREDIT!!!!

Mass of empty crucibleMass of crucible and hydrateMass of hydrateMass of crucible and dehydrateMass of dehydrate
Mass, grams15.00020.0005.00019.5000.500 Calculations: (Remember, you must use YOUR data!)
1. Obtain the mass of the empty crucible. Obtain the mass of the crucible and the hydrate. Subtraction of the mass of the empty crucible from the mass of the hydrate and crucible gives the mass of the CuSO4 hydrate.
Mass of hydrate = (mass of crucible + hydrate) - (mass of empty crucible) Mass of hydrate = (20.000g) – (15.000g) Mass of hydrate = 5.000g

2. Heat the hydrate. After heating, record the mass of the crucible and the dehydrated compound.
No calculations for this step
3. Subtracting the mass of the empty crucible from the mass of the crucible and dehydrated CuSO4 gives you the mass of the dehydrated compound.
Mass of dehydrate = (mass of the crucible and dehydrate) - (mass of empty crucible)
Mass of dehydrate = (19.500g) – (15.000)
Mass of dehydrate = 4.500g

4. Subtract the mass of the dehydrated compound from the mass of the hydrate to determine the mass of water that was present in the hydrate.
Mass of water = (Mass of hydrate) – (mass of dehydrate)
Mass of water = (answer to #1) – (answer to #3)
Mass of water = (5.000g) – (4.500g)
Mass of water = 0.500g
5. Convert the mass of water to moles of water.
To do this, we need the molar mass (from 2.04 and 3.09-molar mass is the mass, in grams, of one mole of your
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