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What chemical test is there to distinguish between a sample of iron(Fe) and a sample of iron sulphide(FeS)
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what are two characteristics shared by plants and green algae
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a chemical test to distinguish between a sample of iron and a sample of iron sulphide.
Top answer:
Which iron sulfide are you talking about? There are several. FeS2 looks like gold, and would not be
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still need to know what chemical tests you can perform to distinguish the difference between a sample of iron and a sample of
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The response from Dr Russ was to suggest you answer and we would critique your answer. He added a
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How do you diffirentiate between a sample of iron and a sample of iron sulfur by means of a chemical test
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This question has been answered twice already
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I have 3 I don't understand how to do.
A 33.2 g of iron ore is treated as follows. The iron in the sample is all converted by a
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Convert 12.63 g Fe2O3 to grams Fe. 12.63 x (2*atomic mass Fe/molar mass Fe2O3) = ? %Fe = (mass
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A 7.7 g sample of iron ore is treated as follows.
The iron in the sample is all converted by a series of chemical reactions to
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You end up with 25.4 g Fe2O3. 25.4g Fe2O3 x (2*atomic mass Fe/molar mass Fe2O3) = mass Fe. Piecemeal
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A 12 g sample of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to
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Check your numbers. Something is wrong with the problem.
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A 38 g sample of iron ore is treated as follows.
The iron in the sample is all converted by a series of chemical reactions to
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Another stoichiometry problem BUT there is a short cut that saves a lot of time; however, the
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A 7.6 g sample of iron ore is treated as follows.
The iron in the sample is all converted by a series of chemical reactions to
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Didn't I do this for you (or one similar to it) a couple of days ago. 12.9g x (1 mol Fe2O3/molar
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A 12.8 g sample of iron ore is treated as
follows. The iron in the sample is all converted by a series of chemical reactions to
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21.3 g Fe2O3 x (1 mol Fe2O3/molar mass Fe2O3) x (2 mol Fe/1 mol Fe2O3) x (atomic mass Fe/1 mol Fe) =
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A 37.5 g sample of iron ore is treated as
follows. The iron in the sample is all converted by a series of chemical reactions to
Top answer:
percent of iron in ore: 2*atomicmassFe/(formulamassFe2O3) now multiply that by 17.8 grams.
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A 25.2 g of iron ore is treated as follows. The
iron in the sample is all converted by a series of chemical reactions to Fe2O3.
A sample of 100 iron bars is said to be drawn from a large number of bars whose lengths are normally distributed with mean 4
