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Topic: Mass Percent  (Read 5952 times)

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Offline bigmoe70

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Mass Percent
« on: December 12, 2007, 05:43:59 AM »
Impurified nickel can be purified by first forming the compound Ni2(SO4)3, which is then decomposed by heating to yield very pure nickel. Metallic nickel reacts directly with concentrated sulfuric acid according to this equation:

2Ni + 3H2SO4 yields Ni2(SO4)3 + H2

Other metals present do not react. If 94.2g of a metal mixture produces 98.4g Ni2(SO4)3, what is the mass percent of nickel in the original sample?

Offline AWK

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Re: Mass Percent
« Reply #1 on: December 12, 2007, 06:49:17 AM »
I do not believe concentrated H2SO4 react with nickel that way
(I mean Ni(III) in the presence of H2)

But assuming that, it is a simple stoichiometry problem. Show your attempt (according to forum rules)
AWK

Offline Montemayor

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Re: Mass Percent
« Reply #2 on: December 12, 2007, 01:19:21 PM »

Moe:

When is this homework assignment due?


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