(10) Bacteria sour wines and beers by converting ethanol, C₂H5OH, into acetic acid, CH₂COOH. Assume that the reaction is C₂H5OH(1) + O₂(g) → CH₂COOH() + H₂O(1) The standard molar enthalpies of combustion of ethanol and acetic acid to produce liquid water are, respectively, -1367 kJ/mol and -875 kJ/mol. Write chemical equations for the combustions, and use Hess' law to determine the standard enthalpy change for the conversion of ethanol to acetic acid.

(10) Bacteria sour wines and beers by converting ethanol, C₂H5OH, into acetic acid, CH₂COOH. Assume that the reaction is C₂H5OH(1) + O₂(g) → CH₂COOH() + H₂O(1) The standard molar enthalpies of combustion of ethanol and acetic acid to produce liquid water are, respectively, -1367 kJ/mol and -875 kJ/mol. Write chemical equations for the combustions, and use Hess' law to determine the standard enthalpy change for the conversion of ethanol to acetic acid.

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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THERMODYNAMICS: A 1.09 g sample of acetic acid (HC2H2O2) was burned in excess oxygen in a bomb calorimeter. The calorimeter, which alone had a heat capacity of 2.67 KJ°C. contained 7g of water. The temperature of the calorimeter and its contents increased from 24.13°C to 27.95°C. What is AH (in kJ) for the combustion per 1.00 mol of acetic acid? MW of acetic acid is 60 gimol. (Round off the final answer to ONE decimal place. Do not include the unit.)
When methanol, CH, OH, is burned in the presence of oxygen gas, O,, a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the balanced, thermochemical equation CH, OH(g) + 0,(g) → CO,(g) + 2 H,O(1) ΔΗ --764 kJ How much methanol, in grams, must be burned to produce 837 kJ of heat?
4) Consider the thermochemical equation below. What mass of HgO must decompose to consume 400.0 kJ of heat? 2 HgO (s) → 2 Hg (1)+ O2(g) AH°rxn =+ 181.4 kJ (1) 5) Write the standard formation reaction for KAI(SO4)2(s). (1) 3 CO2 (g). (1) -393.5 kJ/mol 2 Cr (s) + 3 CO (ag) -110.5 kJ/mol Cr2O3 (s) 6) Consider the reaction 0.0 kJ/mol AH°f = -1139.7 kJ/mol Calculate AH°rxn.
A 1.615-g sample of benzoic acid, C7H6O2 (122.12 g/mol) was burned in a bomb calorimeter with excessoxygen. The temperature of the calorimeter and the water before combustion was 17.49 °C; after combustionthe calorimeter and the water had a temperature of 27.28 °C. The calorimeter had a heat capacity of 832 J/K,and contained 0.837 kg of water. Use these data to calculate the molar heat of combustion (in kJ) of benzoicacid.
Given the following two reactions:(1)Fe(s) + Cl2(g)->FeCl2(s) H(1) = -341.8 kJ(2)Hg(l) + Cl2(g)->HgCl2(s) H(2) = -224.3 kJcalculate the enthalpy change for the following reaction:(3) FeCl2(s) + Hg(l)-> Fe(s) + HgCl2(s) H(3) = kJ
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（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?
A sample of NaOH (MM = 40.00 g/mol) with a mass of 1.811 g was added to a solution of HNO3 in a coffee cup calorimeter for a final volume of 100.0 mL. If both solutions were initially at 24.5 °C and the temperature of the resulting solution was recorded as 27.0 °C, determine the AH°rxn (in units of kJ/mol NaOH) for the neutralization reaction between aqueous NaOH. Assume that the density and the heat capacity of the resulting solution are the same as water, 1.00 g/mL and 4.184 J/(g x °C) respectively. Your Answer: Answer units
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