Posted by thao nguyen on Friday, February 19, 2010 at 2:20pm.
A 2.50 g sample of a hydrate of calcium sulphate losses 0.523 g of water when heated. Determine the mass percent of water in the hydrate and the formula of the hydrate.
- chemistry - bobpursley, Friday, February 19, 2010 at 3:37pm
find the mole ratio of water to CaSO4.
divide moles water by the moles CaSO4, that is X
- chemistry - DrBob222, Friday, February 19, 2010 at 3:40pm
percent water = (mass H2O/mass sample)*100= (0.523/2.50)*100 = 20.92 which I would round to 20.9%.
To find the formula, take a 100 gram sample which provides
20.9 g H2O
100-20.9 = 79.1 g CaSO4
moles water = 20.9/18 = 1.16
moles CaSO4 = 79.1/136 = 0.582
Now find the ratio of water to 1 atom of the CaSO4. The easy way to do that is to divide 0.582 by 0.582 = 1.0000 CaSO4
Then 1.16/0.582 = ?? H2O
- chemistry - Chris, Saturday, February 16, 2013 at 12:30am
I believe it comes out to CaSO4 x 2H20
I think haha
Answer this Question
More Related Questions
- chem - a 2.50g sample of hydrate of calcium sulfate losses 0.523g of water when ...
- chemistry - A 2.500 gram sample of hydrate of calcium sulfate loses 0.532 grams ...
- chemistry - In the experiment, a hydrate is heated to form an anhydrate. The ...
- Chemistry - A 32.907-g sample of a hydrate of Au (CN)3 contains 5.406 g H2O What...
- chemistry - Cobalt(2) chloride is commonly obtained from chemical supply houses ...
- Chemistry - I need help with this lab. Write the equation for the decomposition ...
- Chemistry - Experiment 1 results: mass of crucible 88g mass of hydrate 93g mass ...
- chemistry - A 2.50g sample of a hydrate of calcium nitrate was heated, and only ...
- chemistry - I need help with this lab. Write the equation for the decomposition...
- chemistry - if 4.36g of a hydrate of the salt baCl2 is heated and in the process...