Question 3 Continued (d) The following table contains standard enthalpy changes of combustion AcombH®. Use the tabulated values (Table 1) to calculate standard enthalpy change for fermentation reaction Glucose(s) → 2 Ethanol (1) + 2C02(g) Species AcombH®/ kJ mol-" Sucrose (s) (C12H22O11) -5645 Glucose (s) (C,H1206) -2808 Ethanol (1) (C2H50H) -1368 Carbon monoxide (CO) -283 (i) Write balanced chemical equations for combustion reactions of sucrose, glucose, ethanol and carbon monoxide. (ii) Using Hess's Law and relevant equations and their enthalpies, in part (i), calculate the standard enthalpy change for the fermentation reaction.

Question 3 Continued (d) The following table contains standard enthalpy changes of combustion AcombH®. Use the tabulated values (Table 1) to calculate standard enthalpy change for fermentation reaction Glucose(s) → 2 Ethanol (1) + 2C02(g) Species AcombH®/ kJ mol-" Sucrose (s) (C12H22O11) -5645 Glucose (s) (C,H1206) -2808 Ethanol (1) (C2H50H) -1368 Carbon monoxide (CO) -283 (i) Write balanced chemical equations for combustion reactions of sucrose, glucose, ethanol and carbon monoxide. (ii) Using Hess's Law and relevant equations and their enthalpies, in part (i), calculate the standard enthalpy change for the fermentation reaction.

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions

Section: Chapter Questions

Problem 64PS: The enthalpy change for the oxidation of styrene. C8H8, is measured by calorimetry. C8H8() + 10...

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Question 2:The standard enthalpies of formation, at 25.00 oC, of methane (CH4(g)), water (H2O(l)), and carbon dioxide (CO2(g)) are -74.6 kJ/mol, -285.8 kJ/mol, and -393.5 kJ/mol respectively. Calculate the heat released (in kJ) during combustion of 18.84 L of methane under a constant pressure of 1,000 atm at 25.00 oC (N.B., combustion is the reaction of a substance with molecular oxygen to produce water and carbon dioxide).
Please answer the following question: The combustion of isoctane reaction produces -5099.5 kJ of heat per mole of C8H18(g) consumed, under standard conditons. The enthalpy of formation (DHf) for CO2(g) and H2O(g) are -393.5 kJ/mol and -241.8 kJ/mol, repspectively. Find the standard enthalpy of formation (DHf) of this isomer of C8H18(g)? (Show work) C8H18(g) + O2(g) -> 8CO2(g) + 9H2O(g) DHrxn = -5099.5 kJ
Question 2: The standard enthalpies of formation, at 25.00 °C, of methane (CH4(g)), water (H,O(1)), and carbon dioxide (CO-(g)) are respectively -74.6 kJ/mol, -285.8 kJ/mol, and -393.5 kJ/mol. Calculate the heat released (in kJ) during the combustion of 17.70 L of methane under a constant pressure of 1.000 atm at 25.00 °C (N.B. combustion is the reaction of a substance with molecular oxygen to produce water and carbon dioxide).
H2O = -285.5 CO2 = -393 C2H6 = -83.6 enthalpy cycle and enthalpy of combustion
Liquid pentane is burned with dry air and products are measured on a dry basis: CO2 10.1%, CO 0.2%, O2 9.5% remaining. N2 Find the enthalpy of formation for fuel and the true equivalence ratio.
2C4H10 + 13O2 -> 8 CO2 + 10 H2O Heat= -5314kJ, heat of combustion per gram?
The standard enthalpy change of combustion [to CO2(g) and H2O()] at 25°C of the organic solid isophthalic acid, C8H6O4(s), is determined to be -3185.8 kJ mol-1. What is the Hf° of C8H6O4(s) based on this value?
The standard enthalpy change of combustion [to CO2(g) and H2O()] at 25°C of the organic solid 9,10-phenanthrenediol, C14H10O2(s), is determined to be -6482.1 kJ mol-1. What is the Hf° of C14H10O2(s) based on this value? Use the following data: Hf° H2O () = -285.83 kJ mol-1 ; Hf° CO2(g) = -393.51 kJ mol-1
A student performed the procedure described in the lab manual using 48.9 mL of 1.0 M HCl and 49.9 mL of 1.0 M NaOH. Reaction caused the temperature inside the calorimeter to increase from 17.9 oC to 24.7 oC. What is the value of the enthalpy change for this reaction (ΔHaqueous) in units of kJ/mol? (Enter your answer as a number without units.)
Which of the following is FALSE regarding the lab experiment on Calorimetry? a.The specific heat of the calorimeter was calculated in the calibration step. b.The reactions utilized in the calibration step and in the measurement of enthalpy of reaction are both exothermic. c.The enthalpy of reaction for a strong acid-strong base system was calculated in the experiment. d.The ΔHrxn of the reactions used in (1) calibration and (2) in the measurement of ΔHrxn are theoretically equal.
The enthalpy change for the oxidation of styrene. C8H8, is measured by calorimetry. C8H8() + 10 O2(g) 8 CO2(g) + 4 H2O() rH = 4395.0 kJ|/mol-rxn Use this value, along with the standard enthalpies of formation of CO2(g) and H2O(), to calculate the enthalpy of formation of styrene. in kJ/mol.
The enthalpy of combustion of isooctane (C8H18(l)) is -5461 kJ/mol. From data found in appendix G, calculate the enthalpy of formation of C8H18(l): C8H18(l) + 12.5 O2(g) → 8 CO2(g) + 9 H2O(l) ∆Hrxn = -5461 kJ ∆Hf = ___ kJ/mol Correct answer is not 259.2