The following thermochemical equation is for the reaction of iron(II) oxide(s) with aluminum(s) to form aluminum oxide(s) and iron(s). Fe203(s) + 2Al(s) Al203(s) + 2Fe(s) AH = -852 kJ How many grams of Fe203(s) would have to react to produce 296 kJ of energy? grams

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Chapter6: Thermochemisty
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Problem 6.136QP: Sulfur dioxide gas reacts with oxygen, O2(g), to produce SO3(g). This reaction releases 99.0 kJ of...
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The reaction of nitrogen(g) with oxygen(g) to form dinitrogen monoxide(g) proceeds as follows:
2N2(g) + O2(g) 2N20(g)
When 10.5 grams of N2(g) react with sufficient O2(g), 30.7 kJ of energy are absorbed.
What is the value of AH for the chemical equation given?
kJ
Transcribed Image Text:The reaction of nitrogen(g) with oxygen(g) to form dinitrogen monoxide(g) proceeds as follows: 2N2(g) + O2(g) 2N20(g) When 10.5 grams of N2(g) react with sufficient O2(g), 30.7 kJ of energy are absorbed. What is the value of AH for the chemical equation given? kJ
The following thermochemical equation is for the reaction of iron(III) oxide(s) with aluminum(s) to form aluminum oxide(s) and iron(s).
Fe203(s) + 2AI(s) → Al203(s) + 2Fe(s)
ΔΗ--852 kJ
How many grams of Fe,03(s) would have to react to produce 296 kJ of energy?
grams
Transcribed Image Text:The following thermochemical equation is for the reaction of iron(III) oxide(s) with aluminum(s) to form aluminum oxide(s) and iron(s). Fe203(s) + 2AI(s) → Al203(s) + 2Fe(s) ΔΗ--852 kJ How many grams of Fe,03(s) would have to react to produce 296 kJ of energy? grams
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