Percent Composition and Finding Formula - Chemistry

Click For Summary

Discussion Overview

The discussion revolves around determining the percent composition and empirical formula of a sulfide formed from a reaction between sulfur and iron. Participants explore the calculations involved in finding the molar ratios of the reactants based on the mass of unreacted iron.

Discussion Character

  • Homework-related

Main Points Raised

  • One participant presents a scenario involving 50.0g of sulfur and 100.0g of iron, noting that 12.5g of iron remains unreacted, and seeks to find the formula of the sulfide formed.
  • Another participant confirms the unreacted mass of iron and suggests calculating the mass of iron that reacted by subtracting the unreacted mass from the initial mass.
  • A third participant agrees with the approach and emphasizes dividing the mass reacted by the respective atomic masses to find the ratio.
  • There is a discussion about how to express the ratios in a suitable form for determining the empirical formula.

Areas of Agreement / Disagreement

Participants generally agree on the method of calculating the mass of reacted iron and the subsequent steps to find the molar ratios, but there is no consensus on the final formula or the exact ratio form to be used.

Contextual Notes

Some assumptions about the completeness of the reaction and the definitions of the terms used in the calculations may not be fully articulated, and the discussion does not resolve the final empirical formula.

Who May Find This Useful

Students studying chemistry, particularly those focusing on stoichiometry and empirical formula calculations, may find this discussion relevant.

Larrytsai
Messages
222
Reaction score
0
% Composition and Finding Formula - Chemistry

50.0g of Sulphur is mixed with 100.0g of iron and heated strongly. When the reaction is complete 12.5g of iron remains. What is the formula of the sulphide formed?

What i have done so far is i got the 2 mols of each element.

Fe=1.79
S=1.56

i divided biggest/smallest and i get 1.41
now i need to know how to put it in ratio form and what to do to find the formula for Sulphide
 
Physics news on Phys.org
it said 12.5g of Fe was unreacted!
 
Kushal said:
it said 12.5g of Fe was unreacted!

hmm so i should go 100-12.5 then find the mol then find the ratio?
 
yeah... this is it...

you divide the mass reacted by the respective atomic mass. then you find the ratio.
 

Similar threads

Percent Composition & Finding Formula - Chemistry
  • · Replies 3 ·
Replies
3
Views
2K
Chemistry Find Empirical Formula of Unknown Substance
  • · Replies 5 ·
Replies
5
Views
2K
Chemistry What is the percentage of KClO3 in a mixture after removing oxygen?
  • · Replies 12 ·
Replies
12
Views
2K
Redox titration and mass percent composition calculations.
  • · Replies 9 ·
Replies
9
Views
17K
Chemistry Finding the molecular formula of an unknown hydrocarbon
  • · Replies 4 ·
Replies
4
Views
3K
Chemistry How can I find the molecular formula in this problem?
  • · Replies 10 ·
Replies
10
Views
3K
Calculate Mass Percent of Fe in Ore Sample
  • · Replies 2 ·
Replies
2
Views
3K
Finding composition of mixture of Fe3O4 and Fe2O3
  • · Replies 5 ·
Replies
5
Views
3K
Calculating Percent Yield of PbI2 in 2CsI + Pb(NO3)2 Reaction
  • · Replies 7 ·
Replies
7
Views
3K
How Do You Calculate the Mass Percent of Fe3+ in Iron Ore Using Stoichiometry?
  • · Replies 28 ·
Replies
28
Views
4K