Solution:
Step 1: Calculate the theoretical yield of the reaction.
Since Fe₂O₃ is the limiting reagent,
[tex]\text{theoretical yield = 0.94 mol Fe} × \frac{\text{55.85 g Fe}}{\text{1 mol Fe}}[/tex]
[tex]\text{theoretical yield = 52.5 g}[/tex]
Step 2: Calculate the actual yield of the reaction.
[tex]\text{percent yield} = \frac{\text{actual yield}}{\text{theoretical yield}} × 100[/tex]
[tex]\text{actual yield} = \frac{\text{percent yield}}{100} × \text{theoretical yield}[/tex]
[tex]\text{actual yield} = \frac{\text{84.5}}{100} × \text{52.5 g}[/tex]
[tex]\boxed{\text{actual yield = 44.36 g}}[/tex]
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