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Ch.9 - Chemical Bonding I: The Lewis Model
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Tro 4th EditionCh.9 - Chemical Bonding I: The Lewis Model문제 105d
9장, 문제 105d

If hydrogen were used as a fuel, it could be burned according to this reaction: H2(g) + 1/2 O2(g) → H2O(g) Which fuel yields more energy per gram?

검증된 단계별 안내
1
Identify the enthalpy change (\( \Delta H \)) for the combustion of hydrogen gas (\( \text{H}_2 \)) using standard enthalpy of formation values.
Calculate the molar mass of hydrogen gas (\( \text{H}_2 \)) to convert the energy per mole to energy per gram.
Compare the energy yield per gram of hydrogen with other common fuels, such as gasoline, by calculating their energy yield per gram using their respective combustion reactions and enthalpy changes.
Consider the energy density (energy per unit mass) of hydrogen and compare it with other fuels to determine which has a higher energy yield per gram.
Discuss the implications of using hydrogen as a fuel in terms of energy efficiency and environmental impact.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Combustion Reaction

A combustion reaction is a chemical process in which a substance reacts rapidly with oxygen, releasing energy in the form of heat and light. In the case of hydrogen, it reacts with oxygen to form water, producing a significant amount of energy. Understanding the stoichiometry of this reaction is essential for calculating energy yields.
추천 영상:
가이드 코스
02:24
Combustion Apparatus

Energy Density

Energy density refers to the amount of energy stored in a given system or region of space per unit volume or mass. For fuels, it is typically expressed in joules per gram or kilojoules per liter. Comparing the energy density of hydrogen with other fuels helps determine which fuel is more efficient for energy production.
추천 영상:
가이드 코스
01:56
Density Concepts

Enthalpy of Combustion

The enthalpy of combustion is the heat released when one mole of a substance is completely burned in oxygen. It is a crucial concept for evaluating the energy output of different fuels. For hydrogen, the enthalpy of combustion is high, indicating that it releases a large amount of energy per gram when combusted, making it a potent fuel source.
추천 영상:
가이드 코스
02:24
Combustion Apparatus
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교과서 질문

If hydrogen were used as a fuel, it could be burned according to this reaction: H2(g) + 1/2 O2(g) → H2O(g) Use average bond energies to calculate ΔHrxn for this reaction.

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교과서 질문

If hydrogen were used as a fuel, it could be burned according to this reaction: H2(g) + 1/2 O2(g) → H2O(g) Which fuel yields more energy per mole?

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교과서 질문

Calculate ΔHrxn for the combustion of octane (C8H18), a component of gasoline, by using average bond energies and then calculate it using enthalpies of formation from Appendix IIB. What is the percent difference between your results? Which result would you expect to be more accurate?

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교과서 질문

If hydrogen were used as a fuel, it could be burned according to this reaction: H2(g) + 1/2 O2(g) → H2O(g) Use average bond energies to calculate ΔHrxn for the combustion of methane (CH4).

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교과서 질문

Draw the Lewis structure for each compound. b. H3PO3 (two OH bonds)

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