### 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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Fe O3(s) + 3CO(g) → 2Fe(s) + 3CO;g); AH® = -26.8 kJ %3D FeO(s) + CO(g) -Fe(s) + CO2(g); AH° = -16.5 kJ determine AH for the following thermochemical equation. Fe O(s)+ CO(g) 2FEO(s) + CO;(g) 6.2 kJ O 22.7 kJ O 10.3 kJ 2433KJ 2-103KJ
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
(b) Calculate the enthalpy change for the reaction C(graphite) + 2 H2(g) → CH4(g) with the help of the enthalpy changes of the following reactions: C(graphite) + O2(g) → CO2(g) ∆H= -393.5 kJmol−1 H2(g) +1/2O2(g) → H2O(l) ∆H = -285.8 kJmol−1 CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) ∆H = -890.4 kJmol−1 The temperature is 25 ◦C in all instances.
Calculate the standard enthalpies of formation of (a) KCIO3(s) with the following information: K(s) + 1/2 Cl₂(g) KCI(s) 2 KCIO3(s)→2 KCl(s) + 3 O₂(g) ArH=-436.75 kJ mol-¹ A,H-89.4 kJ mol-¹ (b) NaHCO3(s) with the following information: Na(s) + 1/2 O₂(g) + 1/2 H₂(g) → NaOH(s) C(s) + O₂(g) → CO₂(g) NaOH(s) + CO₂(g)→→NaHCO3(s) A,H-425.61 kJ mol-¹ ArH=-393.51 kJ mol-¹ A,H= -127.5 kJ mol-¹
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)
What is the standard enthalpy change for the reaction: 2C5H10(1) + 15O2(g) → 10CO2(g) + 10H20(1); where C5H10(1) AH°f = –605.0 kJ/mol; CO2(g) AH°f = -393.5 kJ/mol; H2O(1) AH°F - 285.8 kJ/mol. O a. -5583 kJ O b. -5783 kJ O C. -5383 kJ O d. -5183 kJ e. -4983 kJ
A chemist measures the enthalpy change AH during the following reaction: 4 Fe(s) + 3 02(g)→2 Fe,O3(s) AH =-320. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction ΔΗ x10 Fe(s) + 0,6) - Fe,0,(1) O kJ 2Fe,0; (s) – 4Fe(s) + 30, (3) O kJ 4Fe,0, (s) - 8Fe(s) + 60, (3)
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15. Use the following reactions for which the reaction enthalpies are given to determine the reaction enthalpy of: Given: N₂H40) + 2 H₂O2(1)→ N2(g) + 4H₂O N₂H4(1) + 3 O2(g) → 2 NO2(g) + 2 H₂O(g) H₂O(1) + 1/2O2(g) → H₂O2(1) 1/2 N2(g) + O2(g) → NO₂(g) H₂O → H₂O ΔΗ° = _466 kJ AH°= 98.0 kJ AH° = 34.0 kJ AH° = 44.0 kJ
Find the enthalpy change for this reaction using the data below. Clearly show how you got the answer. 2 Al(s) + 3 Cl2 (g) → 2 AlCl3 (s) Data: (a) 2 Al(s) + 6 HCl(aq) → 2 AlCl3 (aq) + 3 H2 (g) H = −1049 kJ (b) AlCl3 (s) → AlCl3 (aq) H = −323 kJ (c) H2 (g) + Cl2 (g) → 2 HCl(g) H = −185 kJ (d) HCl(aq) → HCl(g) H = +74.8 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
（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?