SHOW YOUR WORK (1) Consider the conversion of glucose to ethanol (and CO2): C6H12O6 → 2CH3CH2OH...
SHOW YOUR WORK
(1) Consider the conversion of glucose to ethanol (and CO2): C6H12O6 → 2CH3CH2OH + 2CO2 The heat of formation for glucose is -1273 kJ/mol, the heat of formation of ethanol is -277.7 kJ/mol, and the heat of formation for CO2 is -393.5 kJ/mol.
(a) What is the heat of formation for making ethanol and CO2 from glucose? ANSWER: -69.4 kJ/mol
(b) Is the reaction thermodynamically favorable? Why/why not?
(2) Calculate the specific enthalpy change when ethylene glycol is heated from 10°C to 20°C. The heat capacity for ethylene glycol is Cp=0.569 cal/g*°C. ANSWER: 5.69 cal/g
Homework Answers
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SHOW YOUR WORK
(1) Consider the conversion of glucose to ethanol (and CO2):
C6H12O6 → 2CH3CH2OH...
1) Calculate the specific enthalpy change when ethylene glycol is heated from 10°C to 20°C. The...
1) Calculate the specific enthalpy change when ethylene glycol is heated from 10°C to 20°C. The heat capacity for ethylene glycol is Cp=0.569 cal/g*°C. ANSWER: 5.69 cal/g
Calculate the standard enthalpy change for the fermentation process, in which glucose (C6H12O6) is converted into...
Calculate the standard enthalpy change for the fermentation process, in which glucose (C6H12O6) is converted into ethanol (C2H5OH) and carbon dioxide (CO2). Substance Enthalpy of Formation, CO2 (g) −393.5 kJ/mol CO2 (aq) −412.9 kJ/mol C2H5OH (l) −276.98 kJ/mol C6H12O6 (s) −1,274.5 kJ/mol H2O (g) −241.8 kJ/mol H2O (l) −285.8 kJ/mol O2 (g) 0 kJ/mol ______kJ/mol
Calculate the standard enthalpy change for the fermentation process, in which glucose (C6H12O6) is converted into...
Calculate the standard enthalpy change for the fermentation process, in which glucose (C6H12O6) is converted into ethanol (C2H5OH) and carbon dioxide (CO2). Substance Enthalpy of Formation, Δ H o f CO2 (g) −393.5 kJ/mol CO2 (aq) −412.9 kJ/mol C2H5OH (l) −276.98 kJ/mol C6H12O6 (s) −1,274.5 kJ/mol H2O (g) −241.8 kJ/mol H2O (l) −285.8 kJ/mol O2 (g) 0 kJ/mol
Given the following heat capacity data, calculate ΔH∘f of CO2(g) at 629 K. The standard enthalpy...
Given the following heat capacity data, calculate ΔH∘f of CO2(g) at 629 K. The standard enthalpy of formation of CO2(g) at 298.15 K is −393.5 kJ⋅mol−1. Assume that the heat capacities are independent of temperature. Substance C(graphite) O2(g) CO2(g) CP,m/J⋅mol−1⋅K−1 8.51 29.0 37.4
From the following heats of combustion, CH3OH(l) + 3/2O2(g) → CO2(g) + 2H2O(l) ΔHorxn = –726.4...
From the following heats of combustion, CH3OH(l) + 3/2O2(g) → CO2(g) + 2H2O(l) ΔHorxn = –726.4 kJ/mol C(graphite) + O2(g) → CO2(g) ΔHorxn = –393.5 kJ/mol H2(g) + ½O2(g) → H2O(l) ΔHorxn = –285.8 kJ/mol Calculate the enthalpy of formation of methanol (CH3OH) from its elements. C(graphite) + 2H2(g) + ½O2(g) → CH3OH(l) Methanol (CH3OH) is an organic solvent and is also used as a fuel in some automobile engines. From...
Time Taken:0:33:09 Brandon Bates: Attempt 1 MULUI PUT Ethanol undergoes combustion in oxygen to produce carbon...
Time Taken:0:33:09 Brandon Bates: Attempt 1 MULUI PUT Ethanol undergoes combustion in oxygen to produce carbon dioxide gas and liquid water. Standard enthalpy formation of [CO2(e)] = -393.5 kJ/mol and [H20(1)] = -285.8 kJ/mol, C,H,OH(1) = -277.6 kJ/mol, what is the standard enthalpy of combustion of ethanol? kJ C,H, OH(1) + 3 02(g) + 2 CO2(g) + 3 H2O(l); A Hex = AH, /mol AH° (ræn) = In A Hfº (products) - In AHF ° (reac tants) +2349 kJ/mol +1366.8...
Assume that a gummy bear consists 100% of glucose, C6H12O6 (MW = 180 g/mol). A gummy...
Assume that a gummy bear consists 100% of glucose, C6H12O6 (MW = 180 g/mol). A gummy bear weighs 228 mg. What is the heat of reaction for the total combustion of one gummy bear in a reaction with molten potassium chlorate, KClO3? 4 KClO3(s) + C6H12O6(s) = 4 KCl(s) + 6 CO2(g) + 6 H2O(g); ΔH0 r = –2726 kJ/mol a. 3.45 kJ b. 34.5 kJ c. 172.5 kJ d. 2726 kJ
Calculate the heat of reaction for the conversion of 1 mole of glucose into formaldehyde, given...
Calculate the heat of reaction for the conversion of 1 mole of glucose into formaldehyde, given the following thermochemical data: H2CO(g)+02(8) Co2(s)+H20(g) AH Comb-572.9 kJ/mol 6C(s)+6H2(g)+302(8)» CH120(s) AH=-1274.4 kJ/mol [C)+0,()Co,() AH-393.5 kJ/mol H()0() ,H20(g) AH=-285.8 kJ/mol What is the AHn for the reaction below? - бн, со (3) Сон20, (3) kJ
If 4.290 g of ethanol C2H5OH(l) is burned completely in a bomb calorimeter at 298.15 K,...
If 4.290 g of ethanol C2H5OH(l) is burned completely in a bomb calorimeter at 298.15 K, the heat produced is 124.34 kJ . Part A Calculate ΔH∘c for ethanol at 298.15 K. Part B Calculate ΔH∘f of ethanol at 298.15 K. The enthalpies of formation of CO2(g) and H2O(l) are −393.5 and −285.8 kJ⋅mol-1, respectively.
A muscle can be thought of as a fuel cell that produces work from the metabolism of glucose CeH12...
thermal physics question
A muscle can be thought of as a fuel cell that produces work from the metabolism of glucose CeH1206 602-6C02 6H20 Relevant data on the reactants and products are tabulated below: H (kJ/mol) -1273 0 | Δ/G (kJ/mol) -910 0 -394.4 237.1 | Glucose O2 (g) CO2 (g393.5 H2O (1) S (J/Knol) 212 205 214 70 -285.8 5. Assuming ideal operation at room temperature, how much work could your muscles 6. Still assuming ideal operation, will heat...
Time Taken:0:33:09 Brandon Bates: Attempt 1 MULUI PUT Ethanol undergoes combustion in oxygen to produce carbon dioxide gas and liquid water. Standard enthalpy formation of [CO2(e)] = -393.5 kJ/mol and [H20(1)] = -285.8 kJ/mol, C,H,OH(1) = -277.6 kJ/mol, what is the standard enthalpy of combustion of ethanol? kJ C,H, OH(1) + 3 02(g) + 2 CO2(g) + 3 H2O(l); A Hex = AH, /mol AH° (ræn) = In A Hfº (products) - In AHF ° (reac tants) +2349 kJ/mol +1366.8...
Calculate the heat of reaction for the conversion of 1 mole of glucose into formaldehyde, given the following thermochemical data: H2CO(g)+02(8) Co2(s)+H20(g) AH Comb-572.9 kJ/mol 6C(s)+6H2(g)+302(8)» CH120(s) AH=-1274.4 kJ/mol [C)+0,()Co,() AH-393.5 kJ/mol H()0() ,H20(g) AH=-285.8 kJ/mol What is the AHn for the reaction below? - бн, со (3) Сон20, (3) kJ
thermal physics question
A muscle can be thought of as a fuel cell that produces work from the metabolism of glucose CeH1206 602-6C02 6H20 Relevant data on the reactants and products are tabulated below: H (kJ/mol) -1273 0 | Δ/G (kJ/mol) -910 0 -394.4 237.1 | Glucose O2 (g) CO2 (g393.5 H2O (1) S (J/Knol) 212 205 214 70 -285.8 5. Assuming ideal operation at room temperature, how much work could your muscles 6. Still assuming ideal operation, will heat...
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