Question

One of the reactions that occurs in a blast furnace, where iron ore is converted to cast iron, is below. Fe2O3 + 3 CO → 2 Fe + 3 CO2 Suppose that 1.92 ✕ 103 kg of Fe are obtained from a 5.13 ✕ 103 kg sample of Fe2O3. Assuming that the reaction goes to completion, what is the percent purity of Fe2O3 in the original sample?

Answer 1

The answer to your question is: 53.46 % pure

Step-by-step explanation:

data

Fe = 1.92 ✕ 103 kg produced = 1920 kg

Fe2O3 = 5.13 ✕ 103 kg sample = 5130 kg

MW Fe2O3 = (56x2)+(16x3) = 160 kg

% of purity = ?

Fe2O3 + 3 CO → 2 Fe + 3 CO2

Convert mass to moles

Fe

56 kg --------------------- 1 mol

1920 kg --------------------- x moles x = 34.28 moles

From the reaction

1 mol of Fe2O3 --------------------- 2 moles of Fe

x moles of Fe2O3 --------------- 34.28 moles

x = 34.28/2 = 17.14 moles of Fe2O3

160 kg of FE2O3 ---------------- 1 mol

x kg of Fe2O3--------------- 17.14 moles

x = 17.14 x 160/1 = 2742,4 kg of Fe2O3 It's supposed to be the amount of Fe if it was 100% pure.

2742.4 kg of Fe2O3 ---------------- 100%

5130 kg of Fe2O3 ------------------- x

x = (2742.4x100)/5130 = 53.46 pure