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atroni [7]
3 years ago
14

The following two reactions are important in the blast furnace production of iron metal from iron ore (Fe2O3):2C(s) + O2(g) -&gt

; 2CO(g)Fe2O3 + 3CO(g) -> 2Fe + 3CO2Using these balanced reactions, how many moles of O2 are required for the production of 5.00 kg of Fe?A) 67.1 molesB) 29.8 molesC) 7.46 molesD) 89.5 molesE) 16.8 moles
Chemistry
1 answer:
Inga [223]3 years ago
3 0

Answer: A) 67.1 moles

Explanation:

The balanced reaction is :

2C(s)+O_2(g)\rightarrow 2CO(g)

Fe_2O_3+3CO(g)\rightarrow 2Fe+3CO_2

To calculate the moles, we use the equation:

\text{Number of moles of iron}=\frac{\text{Given mass}}{\text {Molar mass}}=\frac{5.00\times 1000g}{56g/mol}=89.3moles

According to stoichiometry;

2 moles of iron is produced by 3 moles of carbon monoxide

89.3 moles of iron is produced by=\frac{3}{2}\times 89.3=134 moles of carbon monoxide

2 moles of carbon monoxide is produced by = 1 mole of oxygen

Thus 134 moles of carbon monoxide is produced by = \frac{1}{2}\times 134=67.1 moles of oxygen

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1. In this case, according to the reaction, we can infer that 799 kJ of energy are evolved (given off, released) it means that the enthalpy of reaction is negative as the reactants have more energy than the products; which means this is an exothermic reaction.

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