# Chemistry

posted by .

A rock sample contains only Sb2S3 and FeS. If 835g of the sample contains 11.2% antimony, what is the mass percent of the Sb2S3 in the sample? What is the mass percent of the sulfur in the sample?

So far, I have determined that 11.2% of an 835g sample is 93.52g Sb, the molar mass of FeS is 87.92 g/mol and the molar mass of Sb2S3 is 339.73 g/mol. I have no idea where to go from here.

• Chemistry -

pretend you have 100 g of the sample
Then, you have 11.2 grams Sb. That is

moles Sb=11.2/molemassSb.

But you know the compound is Sb2S3, which means there are 1/2 * moles Sb of Sb2S3 (reason, if you have ten moles SB, you can make 5 moles Sb2S3).

Now, you know the moles Sb2S3. That means you have a mass of Sb2S3 of molesSb2S3*molmassSb2S3. So the percent of antomony sulide is then that mass divided by 100grams.

The remaining mass is Ferrous Sulfide, and you can determine its percent by dividing by 100

## Similar Questions

1. ### Chem problem- percent yield

Heating an ore of antimony (Sb2S3) in the presence of iron gives the element antimony and iron(II) sulfide. Sb2S3 (s) + 3Fe(s) ¨ 2Sb(s) + 3FeS(s) When 15.0 g Sb2S3 reacts with an excess of Fe, 9.84 g Sb is produced. What is the …
2. ### chemistry

A 1.10g- sample contains only glucose and sucrose . When the sample is dissolved in water to a total solution volume of 25.0ML , the osmotic pressure of the solution is 3.78atm at 298K a.What is the percent by mass of glucose in the …
3. ### chemistry

Heating an ore of antimony (Sb2S3) in the presence of iron gives the element antimony and iron(II) sulfide. Sb2S3(s) + 3 Fe(s) 2 Sb(s) + 3 FeS(s) When 10.9 g Sb2S3 reacts with an excess of Fe, 9.84 g Sb is produced. What is the percent …
4. ### chem

Heating an ore of antimony (Sb2S3) in the presence of iron gives the element antimony and iron(II) sulfide. Sb2S3(s) + 3 Fe(s) 2 Sb(s) + 3 FeS(s) When 10.9 g Sb2S3 reacts with an excess of Fe, 9.84 g Sb is produced. What is the percent …
5. ### Chemistry

Heating an ore of antimony (Sb2S3) in the presence of iron gives the element antimony and iron(II) sulfide. Sb2S3(s) + 3Fe(s) ==> 2Sb(s) + 3FeS(s) When 15.0g Sb2S3 reacts with an excess of Fe, 9.84g Sb is produced. What is the percent …
6. ### ap chemistry

A mixture contains only NaCl and Fe(NO3)3. A .456 gram sample of the mixture is dissolved in water and an excess of NaOH is added, producing a precipitate of Fe(OH)3. The precipitate is dried and filtered, and its mass is determined …
7. ### Chemistry

A 1.00-kg sample of Sb2S3(s) and a 10.0-g sample of H2(g) are allowed to react in a 25.0-L container at 713 K. At equilibrium, 72.6 g H2S(g) is present. What is the value of Kp at 713 K for this reaction?
8. ### Chemistry

Heating an ore of antimony (Sb2S3) in the presence of iron gives the element antimony and iron(II) sulfide. Sb2S3(s) + 3Fe(s) ---> 2Sb(s) + 3FeS(s) When 15.0 g Sb2Sb3 reacts with an excess of Fe, 9.84 g Sb is produced. What is the …
9. ### chem

Sb2S3(s) + 3 Fe(s) 2 Sb(s) + 3 FeS(s) When 14.7 g Sb2S3 reacts with an excess of Fe, 9.84 g Sb is produced. What is the percent yield of this reaction?
10. ### Chemistry

Heating an ore of antimony (Sb2S3) in the presence of iron yields antimony and iron (II) sulfide. Sb2S3 + 3 Fe = 2Sb + 3 FeS When 15g of Sb2S3 reacts with 10g of Fe in the lab 9.84g of Sb is produced. What is the limiting reactant …

More Similar Questions