### Reaction Yield Calculation ProblemFor the following reaction, 5.69 grams of hydrogen sulfide are mixed with excess oxygen gas. The reaction yields 2.33 grams of water.\[ \text{2H}_2\text{S (g)} + 3\text{O}_2\text{ (g)} \rightarrow 2\text{H}_2\text{O (l)} + 2\text{SO}_2\text{ (g)} \]#### Questions:1. **What is the theoretical yield of water?** \( \_\_\_\_\_\_\_\_\_\_ \) grams 2. **What is the percent yield for this reaction?** \( \_\_\_\_\_\_\_\_\_\_ \) %---**Explanation:**- **Theoretical Yield:** This is the maximum amount of product (water in this case) that can be formed from the given amount of reactant (hydrogen sulfide) based on stoichiometric calculations. - **Percent Yield:** This represents the efficiency of the reaction and is calculated using the formula:\[ \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100 \]To solve these questions, you will need to perform stoichiometric calculations using the molar masses of hydrogen sulfide (H₂S) and water (H₂O) and the given chemical equation.

Given information: Mass of hydrogen sulfide = 5.69 g Actual yield of water = 2.33 g

For the following reaction, 5.69 grams of hydrogen sulfide are mixed with excess oxygen gas. The reaction yields 2.33 grams of water. 2H2S (g) + 302 (g) - 2H2O (1) + 2SO2 (g) (1) What is the theoretical yield of water? grams (2) What is the percent yield for this reaction? %

For the following reaction, 5.69 grams of hydrogen sulfide are mixed with excess oxygen gas. The reaction yields 2.33 grams of water. 2H2S (g) + 302 (g) - 2H2O (1) + 2SO2 (g) (1) What is the theoretical yield of water? grams (2) What is the percent yield for this reaction? %

Chemistry

10th Edition

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

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

### Reaction Yield Calculation Problem

For the following reaction, 5.69 grams of hydrogen sulfide are mixed with excess oxygen gas. The reaction yields 2.33 grams of water.

\[ \text{2H}_2\text{S (g)} + 3\text{O}_2\text{ (g)} \rightarrow 2\text{H}_2\text{O (l)} + 2\text{SO}_2\text{ (g)} \]

#### Questions:

1. **What is the theoretical yield of water?**
\( \_\_\_\_\_\_\_\_\_\_ \) grams

2. **What is the percent yield for this reaction?**
\( \_\_\_\_\_\_\_\_\_\_ \) %

---

**Explanation:**

- **Theoretical Yield:** This is the maximum amount of product (water in this case) that can be formed from the given amount of reactant (hydrogen sulfide) based on stoichiometric calculations.

- **Percent Yield:** This represents the efficiency of the reaction and is calculated using the formula:
\[ \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100 \]

To solve these questions, you will need to perform stoichiometric calculations using the molar masses of hydrogen sulfide (H₂S) and water (H₂O) and the given chemical equation.

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