How many moles of KCIO3 must be reacted according to the following balanced chemical reaction to transfer -34.2 kJ of heat? 2 KCIO3(s) → 2 KC((s) + 3 O2(g) AH = -89.4 kJ %3D
How many moles of KCIO3 must be reacted according to the following balanced chemical reaction to transfer -34.2 kJ of heat? 2 KCIO3(s) → 2 KC((s) + 3 O2(g) AH = -89.4 kJ %3D
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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![**Question 14 of 15:**
**Problem Statement:**
How many moles of \( \text{KClO}_3 \) must be reacted according to the following balanced chemical reaction to transfer \(-34.2 \, \text{kJ}\) of heat?
**Chemical Reaction:**
\[ 2 \, \text{KClO}_3(s) \rightarrow 2 \, \text{KCl}(s) + 3 \, \text{O}_2(g) \]
**Enthalpy Change (ΔH):**
\[ = -89.4 \, \text{kJ} \]
**Calculation Setup:**
- **Starting Amount Box:** An input section for entering initial quantities.
- **Calculation Factor:** A boxed multiplication expression, indicating that the input amount will be multiplied by a ratio.
- **Answer Box:** Placeholder for the result of the calculation.
- **Reset Button:** Option to clear entries and reset the workspace.
**Input Options:**
Buttons with numeric values:
- \(1\), \(0.001\), \(3\), \(0.383\)
**Instructions:**
1. Enter the starting amount of moles of \( \text{KClO}_3 \) in the provided box.
2. Use the calculation factor to find how many moles of \( \text{KClO}_3 \) are needed.
3. Input values can be selected from the options provided or manually entered.
4. The result will appear in the answer box after performing the calculations.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F743e1204-284e-4787-9cb1-b6fdc93e0afd%2F8fa57fd9-0808-4286-aac6-751008c98c9b%2Ffjkqn_processed.png&w=3840&q=75)
Transcribed Image Text:**Question 14 of 15:**
**Problem Statement:**
How many moles of \( \text{KClO}_3 \) must be reacted according to the following balanced chemical reaction to transfer \(-34.2 \, \text{kJ}\) of heat?
**Chemical Reaction:**
\[ 2 \, \text{KClO}_3(s) \rightarrow 2 \, \text{KCl}(s) + 3 \, \text{O}_2(g) \]
**Enthalpy Change (ΔH):**
\[ = -89.4 \, \text{kJ} \]
**Calculation Setup:**
- **Starting Amount Box:** An input section for entering initial quantities.
- **Calculation Factor:** A boxed multiplication expression, indicating that the input amount will be multiplied by a ratio.
- **Answer Box:** Placeholder for the result of the calculation.
- **Reset Button:** Option to clear entries and reset the workspace.
**Input Options:**
Buttons with numeric values:
- \(1\), \(0.001\), \(3\), \(0.383\)
**Instructions:**
1. Enter the starting amount of moles of \( \text{KClO}_3 \) in the provided box.
2. Use the calculation factor to find how many moles of \( \text{KClO}_3 \) are needed.
3. Input values can be selected from the options provided or manually entered.
4. The result will appear in the answer box after performing the calculations.
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