### Understanding Enthalpy Changes in Chemical ReactionsGiven the reactions:1. \( \text{X}(s) + \frac{1}{2} \text{O}_2(g) \rightarrow \text{XO}(s) \) \( \Delta H = -651.7 \, \text{kJ} \)2. \( \text{XCO}_3(s) \rightarrow \text{XO}(s) + \text{CO}_2(g) \) \( \Delta H = +413.3 \, \text{kJ} \)The task is to determine \( \Delta H \) for the following reaction:\[ \text{X}(s) + \frac{1}{2} \text{O}_2(g) + \text{CO}_2(g) \rightarrow \text{XCO}_3(s) \]### Solution:To find \( \Delta H \) for the target reaction, we apply Hess's Law, which states that the total enthalpy change is the same no matter how a reaction is carried out in steps, provided the initial and final conditions are the same.1. Reverse the direction of reaction 2 to match the formation of \( \text{XCO}_3(s) \): \[ \text{XO}(s) + \text{CO}_2(g) \rightarrow \text{XCO}_3(s) \] The enthalpy change for the reverse reaction is the negative of the forward reaction: \[ \Delta H = -413.3 \, \text{kJ} \]2. Add this reversed reaction with reaction 1: \[ \text{X}(s) + \frac{1}{2} \text{O}_2(g) \rightarrow \text{XO}(s) \] \[ \text{XO}(s) + \text{CO}_2(g) \rightarrow \text{XCO}_3(s) \]3. The net equation becomes: \[ \text{X}(s) + \frac{1}{2} \text{O}_2(g) + \text{CO}_2(g) \rightarrow \text{XCO}_3(s) \]4. Sum the enthalpy changes: \[ \Delta H = (-651.7 \, \text{kJ}) +

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Answered: wen the reactions, X(s) + O₂(g) →→→…

wen the reactions, X(s) + O₂(g) →→→ XO(s) XCO3(s) XO(s) + CO₂(g) at is AH for this reaction? X(s) + O₂(g) + CO₂(g) 1 = AH = -651.7 kJ AH = +413.3 kJ XCO3(s) 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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