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3.09 Molar Mass of Compounds Honors
Transcript of 3.09 Molar Mass of Compounds Honors
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.
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.
5.Convert the mass of water to moles of water.
6.Convert the mass of dehydrated compound to moles of the compound.
7.Divide by the lowest mole value to get a whole number mole ratio.
Heating a hydrate for a sufficient amount of time is real important. Over heating or under heating will ruin the whole experiment. If the hydrate was not heated long enough, i most likely agree that the final measured mass of the anhydrate would have been totally different. It would be different because it would have still been wet if it was not heated long enough and that would cause it to weigh more than the dehydrate.
The purpose of the experiment is to determine the formula of a Copper Sulfate hydrate by heating it up.
Crucible, Balance, Hydrate, Dehydrate, Bunsen Burner, Scale
1.Measure the mass of the clean, empty crucible, record the mass.
2.Fill the crucible about 1/2 to 2/3 full with the hydrate (3 to 5 scoops), record the mass.
3.Heat the crucible and hydrate above a Bunsen burner for at least ten minutes to make sure that all of the water evaporates.
4.Let the crucible cool and then mass the crucible with dehydrated solid inside, record the mass.
5.Calculate the formula of the hydrate.
Mass of empty crucible
Mass of crucible and hydrate
Mass of hydrate
Mass of crucible and dehydrate
Mass of dehydrate
2.Heat the hydrate. After heating, record the mass of the crucible and the dehydrated compound.
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.