[Dylanwhite116]

A compound of Tin Sulfate is decomposed in the lab to give 1.91g of Tin, 1.03 grams of Sulfur, and 2.06g Oxygen. Determine if this is a compound of Tin(II) Sulfate or Tin(IV) Sulfate.

[Dylanwhite116]

Determine the empirical formula for a compound that is 54.1% Calcium, 43.2% Oxygen, and 2.7% Hydrogen. Name the compound.

[Dylanwhite116]

How much (grams) of Copper is expected to be recovered when 7.50 grams of Copper(II) Chlorate is decomposed to give Copper, Chlorine, and Oxygen.

 A 5.00g sample of organic compound is decomposed in the laboratory to give 0.541g of Carbon, 0.135g of Hydrogen, and 4.324g Oxygen. The molecular mass of the compound is known to be 22g/mol. Determine the molecular formula for this compound.

[sjb]

A compound of Tin Sulfate is decomposed in the lab to give 1.91g of Tin, 1.03 grams of Sulfur, and 2.06g Oxygen. Determine if this is a compound of Tin(II) Sulfate or Tin(IV) Sulfate.

Where have you got stuck so far? Please check the Forum rules ( http://www.chemicalforums.com/index.php?topic=65859.0 ) and show your thoughts so far.

[Dylanwhite116]

I don't even know where to start!

[sjb]

I don't even know where to start!

What, for instance are the formulae of tin(II) and tin(IV) sulfates?

[Arkcon]

Dylanwhite116:, I hope you don't mind my merging all your questions, they all work around the same basic concept, and once you learn a bit, you should be able to tackle them.  Try starting problem #1, following sjb:'s suggestion.

[Stovn0611]

Determine the empirical formula for a compound that is 54.1% Calcium, 43.2% Oxygen, and 2.7% Hydrogen. Name the compound.

Consider what would happen if you have 100 g of the compound - convert the percentages into g of each element and then you should be able to find mole ratios in the empirical formula from this.

How much (grams) of Copper is expected to be recovered when 7.50 grams of Copper(II) Chlorate is decomposed to give Copper, Chlorine, and Oxygen.

 A 5.00g sample of organic compound is decomposed in the laboratory to give 0.541g of Carbon, 0.135g of Hydrogen, and 4.324g Oxygen. The molecular mass of the compound is known to be 22g/mol. Determine the molecular formula for this compound.

For the first problem, consider the chemical formula for Copper(II) Chlorate then try to write a reaction for the decomposition of it and use stoichiometry to solve.

For the second problem, find the empirical formula using the values given and then convert this empirical formula to the molecular formula using the molecular mass