How Much Ore is Needed to Extract 47.0kg of Antimony?

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Discussion Overview

The discussion revolves around calculating the amount of ore needed to extract 47.0 kg of antimony (Sb) from stibnite (Sb2S3), focusing on the correct application of stoichiometry and molar mass in the context of a chemistry problem.

Discussion Character

  • Homework-related
  • Mathematical reasoning

Main Points Raised

  • One participant presents a calculation involving the percentage of stibnite in the ore and the desired mass of antimony, questioning the correctness of their thought process and significant figures.
  • Another participant acknowledges that the initial approach is not entirely wrong but points out an error in the molar mass of Sb2S3, suggesting it is incorrectly calculated.
  • There is a discussion about the need to multiply the mass of antimony by 2 due to its presence in the formula Sb2S3, with one participant confirming this approach.
  • Participants engage in clarifying how to calculate molar mass by considering the contributions of both antimony and sulfur in the compound.

Areas of Agreement / Disagreement

Participants do not reach a consensus on the correctness of the calculations, as there are differing views on the molar mass and significant figures. The discussion remains unresolved regarding the final accuracy of the calculations presented.

Contextual Notes

There are unresolved issues regarding the correct molar mass of Sb2S3 and how significant figures should be applied based on the data provided.

alicia113
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An Ore contains 19.6 %...

Question:

An ore contains 19.6% of the mineral stibnite, Sb2S3, which is a source of the element Sb. how much ore must be processed in order to obtain 47.0kg of Sb?My Work:

(47000g Sb)((153.825g Sb2S3/ 2 (121.76 g Sb)) (100g ore/19.6g Sb2S3)

which equals 151472.5983g
151.473 Kg
i just want to know if my though process is correct and if i am suppose to multiply the mass of Sb becasue it has 2 moles ! please let me know ! thanks ! and if my Sig Fig is correct in the final answer
 
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alicia113 said:
i just want to know if my though process is correct

(47000g Sb)((153.825g Sb2S3/ 2 (121.76 g Sb)) (100g ore/19.6g Sb2S3)

It is not entirely wrong.

if i am suppose to multiply the mass of Sb becasue it has 2 moles !

Yes for 2, but your molar mass of Sb2S3 is completely off. 153.8 would be a molar mass for SbS.

which equals 151472.5983g
151.473 Kg

if my Sig Fig is correct in the final answer

No. How many sig figs in the data?
 


Borek said:
It is not entirely wrong.



Yes for 2, but your molar mass of Sb2S3 is completely off. 153.8 would be a molar mass for SbS.





No. How many sig figs in the data?


oh ok.. so i multiply my sb by 2 and s by 3 .. (their masses and then add them together like normally)
 


alicia113 said:
oh ok.. so i multiply my sb by 2 and s by 3 .. (their masses and then add them together like normally)

That's how you calculate molar mass, yes.
 

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