• Part AEnter a balanced reaction for the complete combustion of hydrogen.Express your answer as a chemical equation. Identify all of the phases in your answer.2H2(g)+ O2(g)+2H20 (g)SubmitPrevious Answersv CorrectThe balanced combustion equation is2H2(g) + O2(g)–→2H2O(g)• Part BUse standard enthalpies of formation to calculate the amount of heat released per kilogram of hydrogen fuel.Express your answer using four significant figures.amount of heat released = 1.418×105 kJ/kgPrevious AnswersSubmitAll attempts used; correct answer displayedThe enthalpy of formation of water can be used to calculate the amount of energy released per kilogram of fuel. Since only water is present in a nonstandard state, the enthalpy for the reaction is equal to the enthalpy of formation ofwater. Thus1 mol0.002016 kgAH H20 (kJ/mol) ×where 0.002016 kg/molis the molar mass of hydrogen gas.• Part CEnter a balanced reaction for the complete combustion of methanol.Express your answer as a chemical equation. Identify all of the phases in your answer.2CH3OH(1)+ 302(g}>2CO2(g)+ 4H20(g)SubmitPrevious Answersv CorrectThe balanced combustion equation is2CH3OH(1) + 302(g) → 2CO2(g) + 4H20(g) , Part DUse standard enthalpies of formation to calculate the amount of heat released per kilogram of methanol fuel.Express your answer using four significant figures.amount of heat released = 2,267x104 kJ/kgSubmitPrevious Answersv CorrectThe enthalpies of formation of carbon dioxide, water, and methanol can be used to calculate the amount of energy released per kilogram of fuel as follows:AHfxn =npA Hf(products) – nrA Hf(reactants)[(AH? CO2 + 2(A HỆ H20 ) – AH? CH3OH] (kJ/mol)Once you have the enthalpy change for the reaction, divide by the molar mass of the fuel, methanol, in kg/molto find the heat released., Part EWhich fuel contains the most energy in the least mass?hydrogenmethanolPrevious AnswersSubmitv CorrectUsing the results from Parts B and D of the question. Hydrogen contributes almost an order of magnitude more energy per kilogram of mass than does methanol.• Part FTo compare the energy of these fuels to that of octane (CgH19 , calculate the energy released per kilogram of octane.Express your answer using four significant figures.kJ/kgamount of heat released by octane =

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Asked Feb 13, 2020
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please answer part f using the provided information in the images 

• Part A
Enter a balanced reaction for the complete combustion of hydrogen.
Express your answer as a chemical equation. Identify all of the phases in your answer.
2H2(g)+ O2(g)+2H20 (g)
Submit
Previous Answers
v Correct
The balanced combustion equation is
2H2(g) + O2(g)–→2H2O(g)
• Part B
Use standard enthalpies of formation to calculate the amount of heat released per kilogram of hydrogen fuel.
Express your answer using four significant figures.
amount of heat released = 1.418×105 kJ/kg
Previous Answers
Submit
All attempts used; correct answer displayed
The enthalpy of formation of water can be used to calculate the amount of energy released per kilogram of fuel. Since only water is present in a nonstandard state, the enthalpy for the reaction is equal to the enthalpy of formation of
water. Thus
1 mol
0.002016 kg
AH H20 (kJ/mol) ×
where 0.002016 kg/mol
is the molar mass of hydrogen gas.
• Part C
Enter a balanced reaction for the complete combustion of methanol.
Express your answer as a chemical equation. Identify all of the phases in your answer.
2CH3OH(1)+ 302(g}>2CO2(g)+ 4H20(g)
Submit
Previous Answers
v Correct
The balanced combustion equation is
2CH3OH(1) + 302(g) → 2CO2(g) + 4H20(g)
help_outline

Image Transcriptionclose

• Part A Enter a balanced reaction for the complete combustion of hydrogen. Express your answer as a chemical equation. Identify all of the phases in your answer. 2H2(g)+ O2(g)+2H20 (g) Submit Previous Answers v Correct The balanced combustion equation is 2H2(g) + O2(g)–→2H2O(g) • Part B Use standard enthalpies of formation to calculate the amount of heat released per kilogram of hydrogen fuel. Express your answer using four significant figures. amount of heat released = 1.418×105 kJ/kg Previous Answers Submit All attempts used; correct answer displayed The enthalpy of formation of water can be used to calculate the amount of energy released per kilogram of fuel. Since only water is present in a nonstandard state, the enthalpy for the reaction is equal to the enthalpy of formation of water. Thus 1 mol 0.002016 kg AH H20 (kJ/mol) × where 0.002016 kg/mol is the molar mass of hydrogen gas. • Part C Enter a balanced reaction for the complete combustion of methanol. Express your answer as a chemical equation. Identify all of the phases in your answer. 2CH3OH(1)+ 302(g}>2CO2(g)+ 4H20(g) Submit Previous Answers v Correct The balanced combustion equation is 2CH3OH(1) + 302(g) → 2CO2(g) + 4H20(g)

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, Part D
Use standard enthalpies of formation to calculate the amount of heat released per kilogram of methanol fuel.
Express your answer using four significant figures.
amount of heat released = 2,267x104 kJ/kg
Submit
Previous Answers
v Correct
The enthalpies of formation of carbon dioxide, water, and methanol can be used to calculate the amount of energy released per kilogram of fuel as follows:
AHfxn =
npA Hf(products) – nrA Hf(reactants)
[(AH? CO2 + 2(A HỆ H20 ) – AH? CH3OH] (kJ/mol)
Once you have the enthalpy change for the reaction, divide by the molar mass of the fuel, methanol, in kg/mol
to find the heat released.
, Part E
Which fuel contains the most energy in the least mass?
hydrogen
methanol
Previous Answers
Submit
v Correct
Using the results from Parts B and D of the question. Hydrogen contributes almost an order of magnitude more energy per kilogram of mass than does methanol.
• Part F
To compare the energy of these fuels to that of octane (CgH19 , calculate the energy released per kilogram of octane.
Express your answer using four significant figures.
kJ/kg
amount of heat released by octane =
help_outline

Image Transcriptionclose

, Part D Use standard enthalpies of formation to calculate the amount of heat released per kilogram of methanol fuel. Express your answer using four significant figures. amount of heat released = 2,267x104 kJ/kg Submit Previous Answers v Correct The enthalpies of formation of carbon dioxide, water, and methanol can be used to calculate the amount of energy released per kilogram of fuel as follows: AHfxn = npA Hf(products) – nrA Hf(reactants) [(AH? CO2 + 2(A HỆ H20 ) – AH? CH3OH] (kJ/mol) Once you have the enthalpy change for the reaction, divide by the molar mass of the fuel, methanol, in kg/mol to find the heat released. , Part E Which fuel contains the most energy in the least mass? hydrogen methanol Previous Answers Submit v Correct Using the results from Parts B and D of the question. Hydrogen contributes almost an order of magnitude more energy per kilogram of mass than does methanol. • Part F To compare the energy of these fuels to that of octane (CgH19 , calculate the energy released per kilogram of octane. Express your answer using four significant figures. kJ/kg amount of heat released by octane =

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Expert Answer

Energy released per kilogram of octane has to be calculated.

Chemistry homework question answer, step 1, image 1

Enthalpy of combustion is calculated as follows,

Chemistry homework question answer, step 2, image 1

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