**Chemical Reaction Problem**2. ____ KClO₃ → ____ KCl + ____ O₂a. Balance the reactionb. What is the reaction type? ____________________c. What is the theoretical yield in moles of oxygen that are produced by the reaction of 6 moles of potassium chlorate?d. If 11 moles of oxygen are actually produced, what is the percent yield?e. What is the percent error?---**Explanation and Solution Steps:**1. **Balancing the Reaction:** - The unbalanced equation is: KClO₃ → KCl + O₂ - Balance each element: - K: 1 K on both sides - Cl: 1 Cl on both sides - O: There are 3 O on the left and 2 O on the right, so you need to adjust to make them equal. - Balanced Equation: 2 KClO₃ → 2 KCl + 3 O₂2. **Reaction Type:** - It is a decomposition reaction because KClO₃ breaks down into KCl and O₂.3. **Theoretical Yield Calculation:** - From the balanced equation, 2 moles of KClO₃ produce 3 moles of O₂. - Calculate the yield for 6 moles of KClO₃ using the ratio (6 moles KClO₃ x 3 moles O₂ / 2 moles KClO₃ = 9 moles O₂).4. **Percent Yield:** - If actually 11 moles of O₂ are produced: - Percent Yield = (Actual Yield / Theoretical Yield) x 100% - Percent Yield = (11 moles / 9 moles) x 100% = 122.22%5. **Percent Error:** - Percent Error = | (Actual - Theoretical) / Theoretical | x 100% - Percent Error = | (11 moles - 9 moles) / 9 moles | x 100% = 22.22%

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Answered: 2. KCIO3 _KCI +_O2 a. Balance the…

2. KCIO3 _KCI +_O2 a. Balance the reaction b. What is the reaction type?. C. What is the theoretical yield in moles of oxygen that are produced by the reaction of 6 moles c potassium chlorate?

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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Concept explainers

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

**Chemical Reaction Problem**

2. ____ KClO₃ → ____ KCl + ____ O₂

a. Balance the reaction

b. What is the reaction type? ____________________

c. What is the theoretical yield in moles of oxygen that are produced by the reaction of 6 moles of potassium chlorate?

d. If 11 moles of oxygen are actually produced, what is the percent yield?

e. What is the percent error?

---

**Explanation and Solution Steps:**

1. **Balancing the Reaction:**
- The unbalanced equation is: KClO₃ → KCl + O₂
- Balance each element:
- K: 1 K on both sides
- Cl: 1 Cl on both sides
- O: There are 3 O on the left and 2 O on the right, so you need to adjust to make them equal.

- Balanced Equation: 2 KClO₃ → 2 KCl + 3 O₂

2. **Reaction Type:**
- It is a decomposition reaction because KClO₃ breaks down into KCl and O₂.

3. **Theoretical Yield Calculation:**
- From the balanced equation, 2 moles of KClO₃ produce 3 moles of O₂.
- Calculate the yield for 6 moles of KClO₃ using the ratio (6 moles KClO₃ x 3 moles O₂ / 2 moles KClO₃ = 9 moles O₂).

4. **Percent Yield:**
- If actually 11 moles of O₂ are produced:
- Percent Yield = (Actual Yield / Theoretical Yield) x 100%
- Percent Yield = (11 moles / 9 moles) x 100% = 122.22%

5. **Percent Error:**
- Percent Error = | (Actual - Theoretical) / Theoretical | x 100%
- Percent Error = | (11 moles - 9 moles) / 9 moles | x 100% = 22.22%

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