2.50 g Fe2O3 excess CO metal Fe ΔH° = –24.8 kJ
2.50 g Fe2O3와 과량 CO가 반응, metal Fe 생성.
Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) ... ΔH° = –24.8 kJ
How much heat in kJ is evolved or absorbed
in the reaction of 2.50 g of Fe2O3
with enough carbon monoxide to produce iron metal?
Is the process exothermic or endothermic?
Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) ... ΔH° = –24.8 kJ
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Fe2O3의 몰질량 = 159.69 g/mol 이므로,
2.50 g / (159.69 g/mol) = 0.0157 mol Fe2O3
( 참고 https://ywpop.tistory.com/7738 )
0.0157 mol × (–24.8 kJ/mol) = –0.389 kJ
---> 0.389 kJ 만큼의 열이 방출.
ΔH < 0 이므로, 발열 반응.
답: 0.389 kJ is evolved. exothermic.
[참고] 철광석의 제련은 발열 과정이다.
Smelting of iron ore is an exothermic process.
( 참고: 철의 제련 https://ywpop.tistory.com/4368 )
[키워드] How much heat in kJ is evolved or absorbed in the reaction of 2.50 g of Fe2O3 when reacted with an excess of carbon monoxide to produce iron metal? Is this reaction exothermic or endothermic?
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