An alum hydrate sample was analyzed by decomposition and gave the following data: mass of beaker and watchglass + alum hydrate 102.218
mass of beaker and watchglass 101.286
mass of beaker and watchglass + anhydrous compound 101.798
Does the experimental result agree with the theoretical value?

No, the experimental result is different from the theoretical value.

Explanation:

Based on the given information, the mass of beaker and watchglass plus alum hydrate is 102.218 grams, and the mass of beaker and watchglass is 101.286 grams. Therefore, the mass of alum hydrate is:  

= 102.218 grams - 101.286 grams

= 0.932 grams

Now the mass of anhydrous compound is,  

= 102.218 grams - 101.798 grams

= 0.42 grams

Thus, the mass of water present is,  

= 0.932 grams - 0.42 grams

= 0.512 grams

The mass percent of water is,  

= mass of water/Total mass of hydrate * 100

= 0.512 grams / 0.932 grams * 100

= 54.93 %

Hence, the experimental result in not similar to the theoretical result.  

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