### Calculating the Enthalpy Change (ΔH_rxn) for a ReactionTo determine the ΔH_rxn for the reaction:\[ 2\text{H}_2(g) + 2\text{CO}(g) \rightarrow 2\text{H}_2\text{O}(g) + 2\text{C}(s) \]We use the given enthalpy changes for the following reactions:1. \[ \text{H}_2\text{O}(g) + \text{CO}(g) \rightarrow \text{H}_2(g) + \text{CO}_2(g) \quad \Delta H_1 = -41.2 \, \text{kJ} \]2. \[ 3\text{H}_2(g) + \text{CO}(g) \rightarrow \text{H}_2\text{O}(g) + \text{CH}_4(g) \quad \Delta H_2 = -206 \, \text{kJ} \]3. \[ \text{CO}_2(g) + \text{CH}_4(g) \rightarrow 2\text{H}_2\text{O}(g) + 2\text{C}(s) \quad \Delta H_3 = -15.5 \, \text{kJ} \]### Explanation of Reactions and ΔH Values:- **Reaction 1:** Represents the conversion of water vapor and carbon monoxide to hydrogen gas and carbon dioxide, releasing 41.2 kJ of energy.- **Reaction 2:** Conveys the reaction of hydrogen gas and carbon monoxide to form water vapor and methane, releasing 206 kJ of energy.- **Reaction 3:** Describes the reaction between carbon dioxide and methane to produce water vapor and solid carbon, releasing 15.5 kJ of energy.### Task:**Express your answer in decimal notation rounded to three significant figures.**When presenting this material on an educational website, it is crucial to explain the context of each reaction, the significance of enthalpy changes, and the method of calculating the overall enthalpy change for the given reaction. This approach aids in comprehending chemical thermodynamics and energy transformations in chemical reactions.

Thermodynamics is branch of chemistry in which we deal with amount of heat evolved or absorbed by…

Calculate the A Hrxn for the reaction: 2H₂(g) + 2CO(g) → 2H₂O(g) + 2C(s) Given that: H₂O(g) + CO(g) → H₂(g) + CO₂(g) A H₁ = -41.2 kJ A H₂ = -206. KJ 3H₂(g) + CO(g) → H₂O(g) + CH4(g) CO2(g) + CH4(g) 2H₂O(g) + 2C(s) A H3 = -15.5 kJ Express your answer in decimal notation rounded to three signific

Calculate the A Hrxn for the reaction: 2H₂(g) + 2CO(g) → 2H₂O(g) + 2C(s) Given that: H₂O(g) + CO(g) → H₂(g) + CO₂(g) A H₁ = -41.2 kJ A H₂ = -206. KJ 3H₂(g) + CO(g) → H₂O(g) + CH4(g) CO2(g) + CH4(g) 2H₂O(g) + 2C(s) A H3 = -15.5 kJ Express your answer in decimal notation rounded to three signific

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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Determine the enthalpy change, AH, in kJ, for the following reaction: CS2 (1) + 302 (g) --> CO₂ (g) + 2SO2 (g) given the following thermochemical equations: C(s) + O₂ (g) --> CO₂ (g) ΔΗ = 91.2 kJ S (s) + O₂ (g) --> SO₂ (g) ΔΗ = -382 kJ C(s) + 2S (g) --> CS₂ (1) Do not report units in your answer. Report your answer to one decimal place and include the correct sign in your answer. AH = 82.6 kJ
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4) Given the data N2(8) + O2(8) 2 NO(8) AH = +180.7 kJ 2 NO(8) + O2(8) · 2 NO,(8) 2 N,0(8) – 2 N2(8) + O2(8) AH = -163.2 kJ AH = -113.1 kJ | use Hess's law to calculate AH for the reaction N20(8) + NO2(8) –→ 3 NO(8)
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The standard enthalpy change for the following reaction is -135 kJ at 298 K. 1/2 N2(g) + 1/2 H2(g) + 3/2 O2(g) HNO3(g) ΔH° = -135 kJ What is the standard enthalpy change for the reaction at 298 K? N2(g) + H2(g) + 3 O2(g)2 HNO3(g) kJ
A chemist measures the enthalpy change AH during the following reaction: 2 KCl(s) + 302(g) →2 KClO3(s) AH=78. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ. reaction ΔΗ ㅁ x10 2K C103 (s) → 2KC1(s) + 302(g) KCIO, (s)-KCI(s) + 0,(s) 3 KCI(s)+0, (g)KCIO, (s) kJ kJ 1 5
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Given the standard enthalpy changes for the following two reactions: (1) N2(g) + 202(g)N204(g) AH° = 9.2 kJ (2) 2N20(g)2N2(g) + O2(g) AH° = -164.2 kJ what is the standard enthalpy change for the reaction: (3) 2N½0(g) + 302(g)- →2N2O4(g) AH° = ? kJ
Given the standard enthalpy changes for the following two reactions: (1) Sn(s) + Cl½(g)–SnCl½(s) AH° = -325.1 kJ (2) Sn(s) + 2C12(g)– →SNCI4(1) AH° = -511.3 kJ what is the standard enthalpy change for the reaction: (3) SNC1,(s) + Cl2(g)SnCl4(1) AH° = ? kJ
From the following enthalpies of reaction: 2 H2(g) + O2(g) → 2 H2O(l) ΔH = -571.6 kJ/mol C3H4(g) + 4 O2(g) → 3 CO2(g) + 2 H2O(l) ΔH = -1937 kJ/mol C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(l) ΔH = -2220 kJ/mol Determine the heat of the hydrogenation reaction: C3H4(g) + 2 H2(g) → C3H8(g)
（1）Consider the reaction: 2A (g) + 3 B (g) → 2 C (g) ΔHrxn = +254.3 kJ What will be the enthalpy change (in kJ) if 0.471 mol B reacts in excess A? （2）Consider the reaction: C (s) + O2 (g) → CO2 (g) ΔHrxn = -393.5 kJ What mass of carbon (in g) must be reacted via this mechanism to release 581.2 kJ of heat?