First, determine the maximum yield of Fe by converting the given mass of Fe3O4 to moles and using the mole ratio from the balanced chemical equation to convert to moles of Fe: 950 g Fe3O4 * (1 mol Fe3O4/231.5 g Fe3O4) = 4.10 mol Fe3O4
4.10 mol Fe3O4 * (3 mol Fe/1 mol Fe3O4) = 12.3 mol Fe
Next, convert the number of moles of Fe to grams to find the theoretical yield of Fe: 12.3 mol Fe * (55.845 g Fe/mol Fe) = 687 g Fe
Finally, divide the actual yield of Fe by the theoretical yield of Fe and multiply by 100% to find the percent yield: 533 g Fe / 687 g Fe * 100% = 77.6% yield.
Calculate the percent yield of iron if 950 g of Fe3O4 underwent the reaction shown in the chemical equation below and 533 g of Fe was isolated from the reaction mixture. Fe3O4 (s) + 2 C(s) ----> 2 CO2 (g) + 3 Fe(s)
1). 25.9%
2). 77.5%
3). 56.1%
4). None of the above.
Based on my calculations, the answer came out to be number 2. I used the formula %yeild = actual yield/theorical yield * 100
Please helpp!
You are correct. I found 687.4 g for the theoretical yield.
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