**Given the thermochemical equations:**\[\begin{align*}\text{1.} & \quad \text{X}_2 + 3\text{Y}_2 \rightarrow 2\text{XY}_3 \quad \Delta H_1 = -370 \, \text{kJ} \\\text{2.} & \quad \text{X}_2 + 2\text{Z}_2 \rightarrow 2\text{XZ}_2 \quad \Delta H_2 = -130 \, \text{kJ} \\\text{3.} & \quad 2\text{Y}_2 + \text{Z}_2 \rightarrow 2\text{Y}_2\text{Z} \quad \Delta H_3 = -220 \, \text{kJ} \\\end{align*}\]**Calculate the change in enthalpy for the reaction:**\[4\text{XY}_3 + 7\text{Z}_2 \rightarrow 6\text{Y}_2\text{Z} + 4\text{XZ}_2\]\[\Delta H = \boxed{\phantom{- \text{kJ}}}\]**Explanation:**The problem provides three thermochemical equations, each associated with a given enthalpy change (\(\Delta H\)). Your task is to find the overall change in enthalpy for the given reaction by manipulating and combining these equations, typically using Hess's Law.

Answered: Image /qna-images/answer/3bfebe31-7b40-4146-acf3-73dbfdad833a.jpg

Macmillan Learning Given the thermochemical equations X₂ + 3 Y₂ → 2XY3 X₂ +2Z₂ → 2XZ₂ 2Y₂+Z₂2Y₂Z Calculate the change in enthalpy for the reaction. 4XY3 +7Z₂6Y₂Z + 4XZ₂ AH = AH₁ = -370 kJ AH₂ = -130 kJ AH3-220 kJ kJ

Macmillan Learning Given the thermochemical equations X₂ + 3 Y₂ → 2XY3 X₂ +2Z₂ → 2XZ₂ 2Y₂+Z₂2Y₂Z Calculate the change in enthalpy for the reaction. 4XY3 +7Z₂6Y₂Z + 4XZ₂ AH = AH₁ = -370 kJ AH₂ = -130 kJ AH3-220 kJ kJ

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

**Given the thermochemical equations:**

\[
\begin{align*}
\text{1.} & \quad \text{X}_2 + 3\text{Y}_2 \rightarrow 2\text{XY}_3 \quad \Delta H_1 = -370 \, \text{kJ} \\
\text{2.} & \quad \text{X}_2 + 2\text{Z}_2 \rightarrow 2\text{XZ}_2 \quad \Delta H_2 = -130 \, \text{kJ} \\
\text{3.} & \quad 2\text{Y}_2 + \text{Z}_2 \rightarrow 2\text{Y}_2\text{Z} \quad \Delta H_3 = -220 \, \text{kJ} \\
\end{align*}
\]

**Calculate the change in enthalpy for the reaction:**

\[
4\text{XY}_3 + 7\text{Z}_2 \rightarrow 6\text{Y}_2\text{Z} + 4\text{XZ}_2
\]

\[
\Delta H = \boxed{\phantom{- \text{kJ}}}
\]

**Explanation:**
The problem provides three thermochemical equations, each associated with a given enthalpy change (\(\Delta H\)). Your task is to find the overall change in enthalpy for the given reaction by manipulating and combining these equations, typically using Hess's Law.

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