In one experiment you reacted 45.7 g of Alumin um with 182.8 g of Iron (III) oxide to produce AluminumOxide and Elemental iron (not diatomic).g)If you produced 5 grams of aluminum oxide, how many atoms of aluminum are in the 5 grams?h)The reaction required a lot of heat to begin and it did not release any heat? Was the reactionexothermic or endoth ermici)If the reaction required a lot of energy what can you infer from the activation energy?

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Asked Oct 29, 2019
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In one experiment you reacted 45.7 g of Alumin um with 182.8 g of Iron (III) oxide to produce Aluminum
Oxide and Elemental iron (not diatomic).
g)
If you produced 5 grams of aluminum oxide, how many atoms of aluminum are in the 5 grams?
h)
The reaction required a lot of heat to begin and it did not release any heat? Was the reaction
exothermic or endoth ermic
i)
If the reaction required a lot of energy what can you infer from the activation energy?
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In one experiment you reacted 45.7 g of Alumin um with 182.8 g of Iron (III) oxide to produce Aluminum Oxide and Elemental iron (not diatomic). g) If you produced 5 grams of aluminum oxide, how many atoms of aluminum are in the 5 grams? h) The reaction required a lot of heat to begin and it did not release any heat? Was the reaction exothermic or endoth ermic i) If the reaction required a lot of energy what can you infer from the activation energy?

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Expert Answer

Step 1

Reaction involved is:

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2AFe Al,0312Fe(

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Step 2

Molecular weight of iron oxide = (56×2) + (16×3) = 160 g.

Moles of aluminum = 45.7/27 = 1.7 moles.

Moles of aluminum oxide produces =0.5 × 1.7 = 0.85 moles.

Mass of alum...

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