Gchem Question

[D.D.S.]

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What percentage of iron is present in the ore, if a 1.120 g sample requires 25.00 ml of 0.050 M KMnO4 to fully oxidize all of the dissolved Fe2+?

8H+ + 5Fe2+ + MnO4- à 5Fe3+ + Mn2+ + 4H2O


I dont understand the explanation to this problem that someone told me 😉 so can someone explain this to me in simple terms??


Thanks

 

[DDS4tehwin]

I was just about to post this, lol. Isn't Achiever great?

 

[D.D.S.]

Ahhhhhh it has its ups and downs... good for practice i guess... anyone have a better solution to this question??

 

[Flipper405]

Is the answer 31%?

 

[DDS4tehwin]

Well, I think I got it. You have to calculate how much Fe is formed. So:

(5moles)(25ml\1000ml)(.05)(MM of Fe) = Fe formed = Z

(Z\1.12)(100%) = % of Fe

 

[Flipper405]

Well, I think I got it. You have to calculate how much Fe is formed. So:

(5moles)(25ml\1000ml)(.05)(MM of Fe) = Fe formed = Z

(Z\1.12)(100%) = % of Fe

That's also what I did.