**Chemical Reactions and Yield Calculations**1. **Percent Yield Calculation:** In the reaction \( \text{Mg (s)} + \text{I}_2 \text{(s)} \rightarrow \text{MgI}_2 \text{(s)} \), if 10.0 g of Mg reacts with 60.0 g of \( \text{I}_2 \) and 57.14 g of \( \text{MgI}_2 \) is produced, what is the percent yield?2. **Aspirin Production Calculation:** What mass of aspirin (\( \text{C}_9\text{H}_8\text{O}_4 \)) is produced from 88.5 g of \( \text{C}_7\text{H}_6\text{O}_3 \) assuming a 95.0% yield from the reaction below? \( \text{C}_7\text{H}_6\text{O}_3 \text{(s)} + \text{C}_4\text{H}_6\text{O}_3 \text{(s)} \rightarrow \text{C}_9\text{H}_8\text{O}_4 \text{(s)} + \text{HC}_2\text{H}_3\text{O}_2 \text{(aq)} \) **Explanation:**- The first problem involves calculating the percent yield of a reaction by comparing the actual yield (57.14 g of \( \text{MgI}_2 \)) to the theoretical yield obtained from stoichiometry. - The second problem involves determining the mass of aspirin produced, factoring in a 95.0% yield, when starting with 88.5 g of a reactant \( \text{C}_7\text{H}_6\text{O}_3 \). This requires stoichiometric calculations based on the balanced chemical equation provided.

Given, Mass of Mg = 10.0 g Mass of I2 = 60.0 g Actual yield of MgI2 = 57.14 g

Answered: In this reaction: Mg (s) + I2 (s) →…

In this reaction: Mg (s) + I2 (s) → Mgl2 (s), if 10.0 g of Mg reacts with 60.0 g of l2, and 57.14 g of Mgl, form, what is the percent vield?

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

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**Chemical Reactions and Yield Calculations**

1. **Percent Yield Calculation:**

In the reaction \( \text{Mg (s)} + \text{I}_2 \text{(s)} \rightarrow \text{MgI}_2 \text{(s)} \), if 10.0 g of Mg reacts with 60.0 g of \( \text{I}_2 \) and 57.14 g of \( \text{MgI}_2 \) is produced, what is the percent yield?

2. **Aspirin Production Calculation:**

What mass of aspirin (\( \text{C}_9\text{H}_8\text{O}_4 \)) is produced from 88.5 g of \( \text{C}_7\text{H}_6\text{O}_3 \) assuming a 95.0% yield from the reaction below?

\( \text{C}_7\text{H}_6\text{O}_3 \text{(s)} + \text{C}_4\text{H}_6\text{O}_3 \text{(s)} \rightarrow \text{C}_9\text{H}_8\text{O}_4 \text{(s)} + \text{HC}_2\text{H}_3\text{O}_2 \text{(aq)} \)

**Explanation:**

- The first problem involves calculating the percent yield of a reaction by comparing the actual yield (57.14 g of \( \text{MgI}_2 \)) to the theoretical yield obtained from stoichiometry.

- The second problem involves determining the mass of aspirin produced, factoring in a 95.0% yield, when starting with 88.5 g of a reactant \( \text{C}_7\text{H}_6\text{O}_3 \). This requires stoichiometric calculations based on the balanced chemical equation provided.

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