Iron is obtained commercially by the reaction of hematite $F e_{2} O_{3}$ $Fe_2O_3$ with carbon monoxide. How many grams of iron is produced when 25.0 mol of hematite reacts with 30.0 mol of carbon monoxide?

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Iron is obtained commercially by the reaction of hematite $F e_{2} O_{3}$ $Fe_2O_3$ with carbon monoxide. How many grams of iron is produced when 25.0 mol of hematite reacts with 30.0 mol of carbon monoxide?

The reaction is $F e_{2} O_{3} (s) + 3 C O (g) \to 2 F e (s) + 3 C O_{2} (g)$ $Fe_2O_3(s) + 3CO(g) -> 2Fe(s) + 3CO_2(g)$ .

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Answer 1 · 2018-03-30T16:28:59

1117 grams of iron

Explanation:

As can be seen from the chemical equation, each mole of $F e_{2} C O_{3}$ $Fe_2CO_3$ needs 3 moles of $C O$ $CO$ . If 30 moles of $C O$ $CO$ are used, only 10 moles of $F e_{2} C O_{3}$ $Fe_2CO_3$ can be reduced, generating 20 moles of $F e$ $Fe$ , corresponding to 1117 grams of iron.

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Iron is obtained commercially by the reaction of hematite $F e_{2} O_{3}$ $Fe_2O_3$ with carbon monoxide. How many grams of iron is produced when 25.0 mol of hematite reacts with 30.0 mol of carbon monoxide?

The reaction is $F e_{2} O_{3} (s) + 3 C O (g) \to 2 F e (s) + 3 C O_{2} (g)$ $Fe_2O_3(s) + 3CO(g) -> 2Fe(s) + 3CO_2(g)$ .

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Iron is obtained commercially by the reaction of hematite Fe2O3Fe_2O_3 with carbon monoxide. How many grams of iron is produced when 25.0 mol of hematite reacts with 30.0 mol of carbon monoxide?

The reaction is Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)Fe_2O_3(s) + 3CO(g) -> 2Fe(s) + 3CO_2(g).

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Iron is obtained commercially by the reaction of hematite $F e_{2} O_{3}$ $Fe_2O_3$ with carbon monoxide. How many grams of iron is produced when 25.0 mol of hematite reacts with 30.0 mol of carbon monoxide?

The reaction is $F e_{2} O_{3} (s) + 3 C O (g) \to 2 F e (s) + 3 C O_{2} (g)$ $Fe_2O_3(s) + 3CO(g) -> 2Fe(s) + 3CO_2(g)$ .