Consider this reaction Fe + 2 HCI Fe Cl2 + H2 If 30.0 g of FeCl, was recovered after the reaction between 16.0 g of Fe and 18.0 g of HCI, find 1. Theoretical yield 2. Percent yield

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Chapter1: Chemical Foundations
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### Consider this Reaction

\[ \text{Fe} + 2 \text{HCl} \rightarrow \text{FeCl}_2 + \text{H}_2 \]

If 30.0 g of FeCl\(_2\) was recovered after the reaction between 16.0 g of Fe and 18.0 g of HCl, find:

1. Theoretical yield
2. Percent yield

---

### Explanation

This is a chemical equation where iron (Fe) reacts with hydrochloric acid (HCl) to produce iron(II) chloride (FeCl\(_2\)) and hydrogen gas (H\(_2\)).

**Theoretical Yield:** 

The theoretical yield is the maximum amount of product that can be produced in a chemical reaction, based on the amount of limiting reactant.

**Percent Yield:** 

The percent yield is a measure of the efficiency of a reaction, calculated by dividing the actual yield (amount of product obtained) by the theoretical yield, and then multiplying by 100.

You are tasked with computing these values using the given masses of the reactants and the recovered product.
Transcribed Image Text:### Consider this Reaction \[ \text{Fe} + 2 \text{HCl} \rightarrow \text{FeCl}_2 + \text{H}_2 \] If 30.0 g of FeCl\(_2\) was recovered after the reaction between 16.0 g of Fe and 18.0 g of HCl, find: 1. Theoretical yield 2. Percent yield --- ### Explanation This is a chemical equation where iron (Fe) reacts with hydrochloric acid (HCl) to produce iron(II) chloride (FeCl\(_2\)) and hydrogen gas (H\(_2\)). **Theoretical Yield:** The theoretical yield is the maximum amount of product that can be produced in a chemical reaction, based on the amount of limiting reactant. **Percent Yield:** The percent yield is a measure of the efficiency of a reaction, calculated by dividing the actual yield (amount of product obtained) by the theoretical yield, and then multiplying by 100. You are tasked with computing these values using the given masses of the reactants and the recovered product.
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