Part a the following data was acquired by a group of...

Part A: The following data was acquired by a group of students trying to find the empirical formula of a cobalt chloride hydrate, CoCl2 - __H2O. The students weighed out a sample of the hydrated compound in a crucible, then heated the hydrate to remove the water. Below is the data that they acquired. Fill in the blanks in the table and find the empirical formula for the hydrate. Mass crucible: 22.0000 g Mass crucible + hydrate: 24.4580 g Mass crucible + anhydrous solid: 23.9330 g Mass hydrate solid: __ g Mass anhydrous solid: __ g MM anhydrous solid: 129.83 g/mol Moles anhydrous solid: __ mol Mass H2O: __ g MM H2O: 18 g/mol Moles H2O: __ mol Molar ratio H2O: anhydrous solid: __:__ Empirical Formula: CoCl2 - __H2O Part B: Is the following an example of a good hypothesis? Why or why not? "Hermit crabs do not like colorful shells.

Transcript

00:01 Hello students, so the question is to calculate the empirical formula of this and the mass and we have to first fill the blanks.

00:09 So, the first part of the first blank is the mass of the hydrate solid.

00:13 So, it can be calculated by the by subtracting the mass of crucible from the mass of the crucible plus hydrate mass.

00:23 So, it is given in the question.

00:25 So, the mass of crucible plus hydrate is 24 .4580 gram subtracting it with the mass of the crucible which is 22 gram.

00:36 So, it is equal to 2 .458 grams.

00:43 So, this is the mass of the hydrate.

00:45 Now, the second blank is to find the mass of the anhydrous.

00:50 So, this can be calculated by is by subtracting the mass of the crucible from the mass of the crucible plus anhydrous.

00:58 So, it is given and now putting the value will get.

01:02 So, the mass of the anhydrous plus the crucible is 23 .9330 gram and the mass of the crucible is 22 gram and by calculating it by solving it will get the mass of the anhydrous and it is equal to 1 .9330 gram.

01:27 Now the next blank is to calculate the moles of the anhydrous.

01:33 So, the number of moles which is n is equal to the weight of the anhydrous divided by its molar mass.

01:43 So, we have been given the molar mass of the anhydrous solid and it is equal to 129 .83 gram per mole.

01:57 So, by putting the value of weight which we have calculated in the second blank and divide by the molar mass will get the number of moles.

02:04 So, here the number of moles which is n is equal to the weight which is 1 .933 gram divide by the molar mass of the anhydrous solid which is 129 .83 gram per mole.

02:20 So, by calculating it will get 0 .0149 moles.

02:29 So, this is the moles of the anhydrous.

02:32 Now the fourth blank is to calculate the mass of water...

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