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How much iron metal can be produced from #40*g# #"ferric oxide"#?

Answer 1

Mateo Aguilar

Approx.....#28*g# #"iron metal..............."#

A stoichiometric equation (i) that depicts the iron reduction is required.

#2Fe_2O_3(s) + 6CO(s) rarr 4Fe +6CO_2(g)uarr#

And (ii) the corresponding amount of "ferric oxide" that undergoes a reaction:

#=(40*g)/(159.69*g*mol^-1)=0.250*mol#

Given the equation, at most I can form #0.500*mol# #"iron metal"# #=# #0.500*molxx55.8*g*mol^-1=??g#

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Answer 2

Avery Adams

Use the molar masses to calculate the moles of ferric oxide, then determine the moles of iron produced using the balanced chemical equation. Finally, convert moles to grams using the molar mass of iron. The result is approximately 28.16 grams of iron.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.