In the reaction Fe2O3 + 3CO �¨ 2Fe + 3CO2
How much CO is used to produce 112 grams of iron?
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To determine the amount of CO used to produce 112 grams of iron in the given reaction, we need to first find the molar mass of CO (carbon monoxide).
The molar mass of carbon (C) is approximately 12.01 grams/mol, and the molar mass of oxygen (O) is approximately 16.00 grams/mol.
So, the molar mass of CO is:
(12.01 g/mol) + (16.00 g/mol) = 28.01 g/mol
Next, we need to find the molar mass of iron (Fe). The molar mass of iron is approximately 55.85 grams/mol.
Now, we can set up a proportion using the balanced equation for the reaction:
Fe2O3 + 3CO → 2Fe + 3CO2
From the equation, we can see that 3 moles of CO react with 2 moles of Fe. We want to find the amount of CO required to produce 112 grams of iron, so we need to convert 112 grams of iron to moles.
Using the molar mass of iron:
(112 g Fe) × (1 mol Fe / 55.85 g Fe) = 2 mol Fe
Now we can set up the proportion:
2 mol Fe / 3 mol CO = 112 g Fe / x
Cross-multiplying gives us:
2 mol Fe × x = 3 mol CO × 112 g Fe
Simplifying further:
2x = 3 × 112
2x = 336
x = 336 / 2
x = 168
Therefore, 168 grams of CO are used to produce 112 grams of iron in the reaction Fe2O3 + 3CO → 2Fe + 3CO2.