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Given the standard enthalpy changes for the following two reactions: ΔΗ° – 434.6 kJ (1) 2Pb(s) + O2(g) → 2PbO(s) (2) Pb(s) + Cl2(g) → PbCl2(s) -- – 359.4 kJ ΔΗ° what is the standard enthalpy change for the reaction: (3) 2PbCl2(s) + O2(g) → 2PbO(s) + 2Cl2(g) ΔΗ° =? = ΔΗ° kJ =

Given the standard enthalpy changes for the following two reactions: ΔΗ° – 434.6 kJ (1) 2Pb(s) + O2(g) → 2PbO(s) (2) Pb(s) + Cl2(g) → PbCl2(s) -- – 359.4 kJ ΔΗ° what is the standard enthalpy change for the reaction: (3) 2PbCl2(s) + O2(g) → 2PbO(s) + 2Cl2(g) ΔΗ° =? = ΔΗ° kJ =

Chemistry
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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**Understanding Standard Enthalpy Changes** Given the standard enthalpy changes for the following two reactions: 1. \( \text{2Pb}(s) + \text{O}_2(g) \rightarrow \text{2PbO}(s) \) \[ \Delta H^\circ = -434.6 \, \text{kJ} \] 2. \( \text{Pb}(s) + \text{Cl}_2(g) \rightarrow \text{PbCl}_2(s) \) \[ \Delta H^\circ = -359.4 \, \text{kJ} \] --- **Goal:** Determine the standard enthalpy change for the following reaction: 3. \( \text{2PbCl}_2(s) + \text{O}_2(g) \rightarrow \text{2PbO}(s) + \text{2Cl}_2(g) \) \[ \Delta H^\circ = \, \text{?} \] Fill in the box with the calculated standard enthalpy change: \[ \Delta H^\circ = \boxed{\,\,} \, \text{kJ} \] --- **Explanation for Educators:** This problem involves calculating the standard enthalpy change for a reaction using known values from related reactions. It applies principles from Hess’s Law, which states that if a reaction is the sum of two or more other reactions, the total enthalpy change is the sum of the enthalpy changes for the individual reactions. Students are tasked with rearranging and manipulating given reactions to derive the enthalpy change of the target reaction, highlighting skills in thermochemistry and stoichiometry.
Transcribed Image Text:**Understanding Standard Enthalpy Changes** Given the standard enthalpy changes for the following two reactions: 1. \( \text{2Pb}(s) + \text{O}_2(g) \rightarrow \text{2PbO}(s) \) \[ \Delta H^\circ = -434.6 \, \text{kJ} \] 2. \( \text{Pb}(s) + \text{Cl}_2(g) \rightarrow \text{PbCl}_2(s) \) \[ \Delta H^\circ = -359.4 \, \text{kJ} \] --- **Goal:** Determine the standard enthalpy change for the following reaction: 3. \( \text{2PbCl}_2(s) + \text{O}_2(g) \rightarrow \text{2PbO}(s) + \text{2Cl}_2(g) \) \[ \Delta H^\circ = \, \text{?} \] Fill in the box with the calculated standard enthalpy change: \[ \Delta H^\circ = \boxed{\,\,} \, \text{kJ} \] --- **Explanation for Educators:** This problem involves calculating the standard enthalpy change for a reaction using known values from related reactions. It applies principles from Hess’s Law, which states that if a reaction is the sum of two or more other reactions, the total enthalpy change is the sum of the enthalpy changes for the individual reactions. Students are tasked with rearranging and manipulating given reactions to derive the enthalpy change of the target reaction, highlighting skills in thermochemistry and stoichiometry.
**Enthalpy Change in Chemical Reactions** **Given the standard enthalpy changes for the following two reactions:** 1. \(2\text{C}(s) + 2\text{H}_2(g) \rightarrow \text{C}_2\text{H}_4(g)\)     \(\Delta H^\circ = 52.3\, \text{kJ}\) 2. \(2\text{C}(s) + 3\text{H}_2(g) \rightarrow \text{C}_2\text{H}_6(g)\)     \(\Delta H^\circ = -84.7\, \text{kJ}\) **What is the standard enthalpy change for the following reaction?** 3. \(\text{C}_2\text{H}_4(g) + \text{H}_2(g) \rightarrow \text{C}_2\text{H}_6(g)\)     \(\Delta H^\circ =?\) **Standard enthalpy change = \_\_\_ kJ**
Transcribed Image Text:**Enthalpy Change in Chemical Reactions** **Given the standard enthalpy changes for the following two reactions:** 1. \(2\text{C}(s) + 2\text{H}_2(g) \rightarrow \text{C}_2\text{H}_4(g)\)     \(\Delta H^\circ = 52.3\, \text{kJ}\) 2. \(2\text{C}(s) + 3\text{H}_2(g) \rightarrow \text{C}_2\text{H}_6(g)\)     \(\Delta H^\circ = -84.7\, \text{kJ}\) **What is the standard enthalpy change for the following reaction?** 3. \(\text{C}_2\text{H}_4(g) + \text{H}_2(g) \rightarrow \text{C}_2\text{H}_6(g)\)     \(\Delta H^\circ =?\) **Standard enthalpy change = \_\_\_ kJ**
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