**Aim: What is a thermochemical equation?****Do Now:** Determine the ΔH and ΔS of the system:\[ 2H_2(g) + O_2(g) \rightarrow 2H_2O(g) \] \( \Delta H \) \( \Delta S \)**Example 1:**- How much energy is released to produce 1.0 mole \( H_2O(g) \)?- How much energy is released to produce 4.0 mole \( H_2O(g) \)?**Example 2:**\[ CH_4(g) + 2O_2(g) \rightarrow CO_2(g) + 2H_2O(l) \]- How much energy is released to produce 1.0 mole \( H_2O(g) \)?- How much energy is released to produce 3.0 mole \( CO_2(g) \)?**Discussion Question:**How is a thermochemical equation similar to a chemical equation? Different?

Note: We are authorized to answer one question at a time, since you have not mentioned which…

DO NOW: Determine the AH and AS of the system: ΔΗ 2H₂(g) + O₂(g) → 2H₂O(g) Example 1: ΔS • How much energy is released to produce 1.0 mole H₂O(g)? How much energy is released to produce 4.0 mole H₂O(g)? Example 2: CH,(g) +20₂(g) → CO₂(g) + 2H₂O(l)- How much energy is released to produce 1.0 mole H₂O(g)? How much energy is released to produce 3.0 mole CO₂(g)? How is a thermochemical equation similar to a chemical equation? Different?

DO NOW: Determine the AH and AS of the system: ΔΗ 2H₂(g) + O₂(g) → 2H₂O(g) Example 1: ΔS • How much energy is released to produce 1.0 mole H₂O(g)? How much energy is released to produce 4.0 mole H₂O(g)? Example 2: CH,(g) +20₂(g) → CO₂(g) + 2H₂O(l)- How much energy is released to produce 1.0 mole H₂O(g)? How much energy is released to produce 3.0 mole CO₂(g)? How is a thermochemical equation similar to a chemical equation? Different?

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

**Aim: What is a thermochemical equation?**

**Do Now:** Determine the ΔH and ΔS of the system:

\[ 2H_2(g) + O_2(g) \rightarrow 2H_2O(g) \] \( \Delta H \) \( \Delta S \)

**Example 1:**

- How much energy is released to produce 1.0 mole \( H_2O(g) \)?
- How much energy is released to produce 4.0 mole \( H_2O(g) \)?

**Example 2:**

\[ CH_4(g) + 2O_2(g) \rightarrow CO_2(g) + 2H_2O(l) \]

- How much energy is released to produce 1.0 mole \( H_2O(g) \)?
- How much energy is released to produce 3.0 mole \( CO_2(g) \)?

**Discussion Question:**
How is a thermochemical equation similar to a chemical equation? Different?

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Step 2: Determine the enthalpy change of the system

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Step 3: Determine the entropy change of the reaction

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Step 4: Determine the energy released to produce 1 mol H2O (g)

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Step 5: Determine the energy released to from 4 mol H2O(g)

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