2.50 g Fe2O3 excess CO metal Fe ΔH° = –24.8 kJ

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?