a) Calculate AH° (in kJ/mol) for the combustion of 1 mol of ethanol, C₂H5OH(I) with toform gaseous carbon dioxide and gaseous water using Hess's Law.C(s) + O₂ (g)H₂(g) + 1/2O₂ (g)2 C(s) + 3H₂(g) + 1/2 O₂(g)►CO₂ (g)→ H₂O (g)C₂H5OH (1)AHform-393.5-241.8-235.2b) Based on your results from a), calculate the amount of energy released in thecombustion of 500 g of ethanol.

Answered: Image /qna-images/answer/ac668426-bb74-4feb-b53f-0cd4574b4981.jpg

a) Calculate AH (in kJ/mol) for the combustion of 1 mol of ethanol, C₂H5OH(I) with to form gaseous carbon dioxide and gaseous water using Hess's Law. -CO₂ (g) H₂O (g) C(s) + O₂ (g) H₂(g) + 1/2O2 (g) 2 C(s) + 3H₂(g) + 12 O₂(g) C₂H5OH (1) AH form -393.5 -241.8 -235.2 b) Based on your results from a), calculate the amount of energy released in the combustion of 500 g of ethanol.

a) Calculate AH (in kJ/mol) for the combustion of 1 mol of ethanol, C₂H5OH(I) with to form gaseous carbon dioxide and gaseous water using Hess's Law. -CO₂ (g) H₂O (g) C(s) + O₂ (g) H₂(g) + 1/2O2 (g) 2 C(s) + 3H₂(g) + 12 O₂(g) C₂H5OH (1) AH form -393.5 -241.8 -235.2 b) Based on your results from a), calculate the amount of energy released in the combustion of 500 g of ethanol.

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

< Question 21 of 29 O Attempt 2 When 0.376 g of sodium metal is added to an excess of hydrochloric acid, 3910 J of heat are produced. What is the enthalpy of the reaction as written? 2 Na(s) + 2 HCI(aq) 2 NaCl(aq) + H2(g) Enthalpy of reaction: 478.35 kJ Incorrect
2 E6L14(s) + 19 A2(g) → 12 MA2(g) + 7 L₂A(g) AH = 1300 kJ/molrxn 21. What is the enthalpy of formation, AH, for the substance E6L14 shown in the reaction above? AH (kJ/mol) ??? со How Substance E6L14(S) A₂(g) De MA₂(g) L₂A (g) 0 100 50 B
A chemist measures the energy change AH during the following reaction: 2 Fe₂O3(s) 4 FeO(s) + O₂(g) 1 AH 560, kJ Use the information to answer the following questions. This reaction is... Suppose 25.9 g of Fe₂O3 react. Will any heat be released or absorbed? If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. Be sure your answer has the correct number of significant digits. endothermic exothermic OYes, absorbed. Yes, released. No. 0... X G
Given : CH4 (g) + 2 O2 (g) --> CO2 (g) + 2H2O (g) Δ H = -882 kJ/mol What is Δ H for the reaction below in kJ/mol. H2O (g)+ 1/2 CO2 (g) --> O2 (g) + 1/2 CH4 (g)
Write a balanced thermochemical expression depicting the formation of 1 mol of the compound below from it's elements. Note: ΔH∘fΔHf∘ for C6H12O6 (s) = -1274.4 kJ/mol 6 CO2 (g) + 6 H2O (l) ⟶⟶ C6H12O6 (s) + 6 O2 (g) ΔH∘ΔH∘ = -1274.4 kJ
A laboratory “volcano” can be made from ammonium dichromate (252.07 g/mol). When ignited, the compound decomposes in a fiery display: (NH4)2Cr2O7(s) ➜ N2(g) + 4H2O(g) + Cr2O3(s) If the decomposition produces 315 kJ of heat per mole of ammonium dichromate at constant pressure, how much heat energy would be produced by 28.3 g of the solid? Select one: a.+33.5 kJ b.+40.7 kJ c.–36.4 kJ d.–35.4 kJ
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300. g of water (see sketch at right). thermometer stirrer First, a 6.000 g tablet of benzoic acid (C,H,C0,H) is put into the "bomb" and burned completely in an excess of water oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is insulation observed to rise from 13.00 °C to 40.13 °C over a time of 10.0 minutes. Next, 5.200 g of ethane (C,H) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 13.00 °C to 53.96 °C. chemical reaction "bomb" Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. 2C,H,(g) + 70,(g) 4CO,(g) + 6 H,0 (g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced…
A 125 g piece of rock of unknown specific heat is heated to 93 degrees C. The rock is then dropped into 100 g of water at 19 degrees C. the water temperature rises to 31 degrees C. What is the specific heat of the rock? (3) O 0.65 J/(g °C) O 0.65 J O 0.71 J/g °C) O 1.14 J/g.
When ammonia reacts with dinitrogen oxide gas (ΔHf° = 82.05 kJ/mol), liquid water and nitrogen gas are formed. How much heat (in kJ) is liberated or absorbed by the reaction that produces 365 mL of nitrogen gas at 25°C and 743 mm Hg? ΔHf° (kJ/mol) NH3(g) –46.1 H2O(l) –285.8 N2(g) 0 N2O(g) 82.05
Do all and label question with problem
uestion 27 "A new element (Rr) has been synthesized and its properties analyzed. When 0.157g of RrO (s) is added to 125g of water at 22.2° C in a coffee cup calorimeter, the following reaction occurs. RrO(s) + H 20(1) – Rr(OH) 2 (aq) AH = -83.1k/mol Given the molar mass for RrO is 74g/mol calculate the following moles of Rro round answer to 4 decimal places omit trailing zeroes 9 rxn in joules round answer to the nearest whole number 9 water in joules round answer to the nearest whole number Final temperature round answer to 1 decimal place omit trailing zeroes " A Moving to another question will save this response.
Consider the reaction of ammonia gas with O2(g) according to the thermochemical equation given below: 4NH3(g) + 702(g) – 4NO2(g) + 6H2O(1) AH° = - 1132 kJ/mole I (a) Calculate the mass (g) NO2 produced together with the release of 226 J of heat. (b) Calculate the heat released when 3.75 g of NO2 are produced.