**Combustion Reaction of Ethanol**The equation represents the combustion of ethanol:\[ \text{C}_2\text{H}_5\text{OH} (l) + 3\text{O}_2 (g) \rightarrow 2\text{CO}_2 (g) + 3\text{H}_2\text{O} (g) \]**Reactants:**- Ethanol (\(\text{C}_2\text{H}_5\text{OH}\)), in its liquid form.- Oxygen (\(\text{O}_2\)), in gaseous form.**Products:**- Carbon dioxide (\(\text{CO}_2\)), in gaseous form.- Water (\(\text{H}_2\text{O}\)), in gaseous form.**Description:**- This balanced chemical equation describes the complete combustion of ethanol, a type of alcohol, with oxygen.- The process results in the formation of carbon dioxide and water vapor.- The coefficients in the equation ensure that the number of each type of atom is the same on both sides, maintaining the principle of conservation of mass. **Calculation of Standard Molar Enthalpy for Ethanol Combustion**To calculate the standard molar enthalpy for the complete combustion of liquid ethanol (\( \text{C}_2\text{H}_5\text{OH} \)), you will need to use the standard enthalpies of formation for both the reactants and products. This information can be typically found in Appendix 4 at the back of your textbook. **Step-by-Step Instructions:**1. **Write the Balanced Chemical Equation:** The balanced equation for the combustion of ethanol is: \[ \text{C}_2\text{H}_5\text{OH}_{(l)} + 3\text{O}_2_{(g)} \rightarrow 2\text{CO}_2_{(g)} + 3\text{H}_2\text{O}_{(g)} \]2. **Identify the Standard Enthalpies of Formation:** Refer to Appendix 4 for the standard enthalpies of formation (\( \Delta H_f^\circ \)) of the following: - Ethanol (\( \text{C}_2\text{H}_5\text{OH} \)) - Oxygen (\( \text{O}_2 \)), typically zero as it is in its elemental state - Carbon dioxide (\( \text{CO}_2 \)) - Water (\( \text{H}_2\text{O} \))3. **Apply Hess’s Law:** Use Hess's Law to find the total enthalpy change of the reaction: \[ \Delta H_{rxn}^\circ = \sum (\Delta H_f^\circ \text{ of products}) - \sum (\Delta H_f^\circ \text{ of reactants}) \]4. **Calculate the Standard Molar Enthalpy:** Plug in the values from Appendix 4 to compute the enthalpy change. **Understanding the Result:**The result represents the energy change when one mole of ethanol undergoes complete combustion under standard conditions. This value is crucial in studying the energy efficiency of fuels.Remember, for precise values and further instruction, refer to the relevant appendix in your textbook.

Answered: Image /qna-images/answer/f2763c59-91f0-4dff-9971-a1fd6aac608c.jpg

Calculate the standard molar enthalpy for the complete combustion of liquid ethanol (C2H5OH) using the standard enthalpies of formation of the reactants and products (see Appendix 4 in the back of the textbook).

Calculate the standard molar enthalpy for the complete combustion of liquid ethanol (C2H5OH) using the standard enthalpies of formation of the reactants and products (see Appendix 4 in the back of the textbook).

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...

See similar textbooks

Similar questions

OH 1. NaOH, EtOH 2. n-BuBr A nucleophilic substitution reaction is a frequently used method to convert one functional group into another. A nucleophile is mixed with an electrophile and the nucleophile replaces the leaving group to produce a new compound. In this experiment, a weak nucleophile (2-naphthol) is converted into a strong nucleophile by deprotonation with sodium hydroxide. Then this strong nucleophile, now with a negative charge, reacts with alkyl halide to yield an ether, 2-butoxynaphthalene. 2-butoxynaphthalene is a flavoring agent that has strong fruit smell like raspberry and strawberry.
A scientist measures the standard enthalpy change for the following reaction to be 561.1 k : 2BrFy(g)Br:(g) +3 F2(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of BrF(g) is kJ/mol.
None
Given the standard enthalpies of formation for the following substances, determine the reaction enthalpy for the following reaction. AGran =? kJ 4A (g) + 2B (3) → 1C (g)+ 7D (g) AGi in kJ/mol Substance A (g) B (g) C(g) D (g) 76.34 + 5.24 - 55.86 - 14.55 O - 452.59 kJ/mol O + 452.59 kJ/mol O + 137.17 kJ/mol O - 141.51 kJ/mol O - 137.17 kJ/mol
A chemist measures the enthalpy change AH during the following reaction: COC1₂(9) + 4 NH3(9)→ CO(NH₂),(s) + 2NH4Cl(s) Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. esc COC₁₂ (8) + 2NH₂(g) → CO(NH₂), (s) + NH₂Cl(s) 1 1 ẩCO(NH,),() + ≈NH,C() → † COCI,(8) + NH, (8) CO(NH₂)₂ (s) + 2NH₂Cl(s) → COCL, (g) + 4NH, (g) Explanation THE Check reaction I > AH=-559. kJ Costa ΔΗ kJ ☐ kJ KJ MacBook Pro x10 X S © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Acc You MOSISO L
The first step in the production of nitric acid from ammonia involves the oxidation of NH3. 4 NH3(g) + 5 O₂ (g) → 4 NO(g) + 6 H₂O(g) 2 a Use standard enthalpies of formation from the table below to calculate the standard enthalpy change for this reaction. Species AfH (kJ/mol) NH3(g) -45.90 NO(g) +90.29 H₂O(g) -241.83 Standard enthalpy change Submit = kJ/mol-rxn
Using the standard enthalpies of formation, what is the standard enthalpy of reaction? CO(g) + H,O(g) –→ CO,(g) + H,(g) AHân = kJ
1. The change in internal energy of the combustion of solid naphthalene (C10H8) was determined to be equal to -5151 kJ/mol. Calculate its enthalpy of combustion. 2. What is the change in internal energy of a system if the system evolves 525 J of heat and has 1.25 kJ of work done on it
1. Methanol CH3OH is a potential source of fuel. An experiment was conducted to determine the enthalpy of combustion of methanol. 2.00 g of methanol was used to heat 150 g of water. The temperature of the water increased from 25°C to 87 °C. (Given that the specific heat capacity of water is 4.18 J K-1 g-1) Define the term standard enthalpy of combustion with reference to methanol. Use the data above to determine the enthalpy of combustion of methanol (show solutions). 2. Calculate the e.m.f of the following cell in the image (show solutions).
A scientist measures the standard enthalpy change for the following reaction to be 184.8 kJ:Fe3O4(s) + 4 H2(g) 3Fe(s) + 4 H2O(g)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of Fe3O4(s) is kJ/mol.
3. Write a balanced chemical reaction for the synthesis of methane (CH4) and liquid water from hydrogen and acetic acid (CH3COOH) and calculate the standard enthalpy of the reaction by using the appropriate enthalpies of formation on page 308 or Appendix 4 in the textbook.
A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy available from foods. Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter. In the laboratory a student burns a 0.461-g sample of 2-naphthylacetic acid (C12H1002) in a bomb calorimeter containing 1150. g water. The temperature increases from 24.70 °C to 27.20 °C. The specific heat capacity of water is 4.184 J g1 oC-1. The combustion enthalpy is -5779 kJ/mol 2-naphthylacetic acid. C12H1002(s) + 27/2 02(g) –→12 CO2(g) + 5 H20(1) A,H° -5779 kJ/mol Calculate the heat capacity of the calorimeter. heat capacity of calorimeter= orc J/C