Question

What mass of co is needed to react completely with 55.0 g of fe2o3 in the reaction: fe2o3(s) + 3co(g) → 2fe(s) + 3co2(g)?

A) 4.82 g
B) 9.64 g
C) 14.5 g
D) 28.9 g

Answer 1

To find the mass of CO needed to react with 55.0 g of Fe2O3, we first calculate the mole of Fe2O3 and use the balanced equation to find the corresponding moles of CO. Multiplying by the molar mass of CO gives us the required mass, which is 28.9 g.

Step-by-step explanation:

To determine the mass of CO needed to completely react with 55.0 g of Fe2O3, we start with the balanced chemical reaction:

Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g).

First, we calculate the molar mass of Fe2O3 and CO. Using the periodic table, we obtain that the molar mass of Fe2O3 is 159.7 g/mol and for CO is 28.01 g/mol. Then, calculate the moles of Fe2O3 using its molar mass:

1. 55.0 g Fe2O3 × (1 mol Fe2O3 / 159.7 g Fe2O3) = 0.344 mol Fe2O3.
2. According to the balanced equation, 1 mol Fe2O3 reacts with 3 mol CO. Thus, 0.344 mol Fe2O3 will react with 3 × 0.344 mol CO = 1.033 mol CO.
3. Finally, calculate the mass of CO: 1.033 mol CO × (28.01 g CO / 1 mol CO) = 28.9 g CO.

Therefore, the mass of CO needed to react completely with 55.0 g of Fe2O3 is 28.9 g, which corresponds to choice D.