Skip to main content
Ch.10 - Chemical Bonding I: The Lewis Model
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Tro 6th EditionCh.10 - Chemical Bonding I: The Lewis Model문제 89
10장, 문제 89

Ethane burns in air to form carbon dixode and water vapor.
2 H3C¬CH3( g) + 7 O2( g)¡4 CO2( g) + 6 H2O( g)
Use average bond energies to calculate ΔHrxn for the reaction.

검증된 단계별 안내
1
Identify the bonds broken in the reactants: In ethane (C2H6), there are C-C and C-H bonds. In O2, there are O=O bonds.
Identify the bonds formed in the products: In CO2, there are C=O bonds. In H2O, there are O-H bonds.
Use the average bond energies to calculate the total energy required to break the bonds in the reactants. This involves multiplying the number of each type of bond by its bond energy and summing them up.
Use the average bond energies to calculate the total energy released when the bonds in the products are formed. Again, multiply the number of each type of bond by its bond energy and sum them up.
Calculate the enthalpy change (ΔH_rxn) for the reaction using the formula: ΔH_rxn = (Total energy of bonds broken) - (Total energy of bonds formed).

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

주요 개념

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

Bond Energies

Bond energies refer to the amount of energy required to break a bond between two atoms in a molecule. In chemical reactions, the total energy required to break the bonds in the reactants is compared to the energy released when new bonds are formed in the products. This concept is crucial for calculating the enthalpy change (ΔHrxn) of a reaction, as it allows us to estimate the energy changes associated with bond breaking and forming.
추천 영상:
가이드 코스
01:50
Bond Energy

Enthalpy Change (ΔHrxn)

The enthalpy change (ΔHrxn) of a reaction is the difference in energy between the products and the reactants, indicating whether a reaction is exothermic (releases heat) or endothermic (absorbs heat). It can be calculated using the formula ΔHrxn = Σ(Bond Energies of Reactants) - Σ(Bond Energies of Products). Understanding this concept is essential for predicting the energy dynamics of the combustion of ethane.
추천 영상:
가이드 코스
02:34
Enthalpy of Formation

Combustion Reaction

A combustion reaction is a chemical reaction that typically involves a hydrocarbon reacting with oxygen to produce carbon dioxide and water, releasing energy in the form of heat and light. In the case of ethane, the balanced equation shows that it reacts with oxygen to produce carbon dioxide and water vapor. Recognizing the characteristics of combustion reactions is important for applying bond energy calculations to determine the overall energy change.
추천 영상:
가이드 코스
02:24
Combustion Apparatus
관련 실천
교과서 질문

Ethanol is a possible fuel. Use average bond energies to calculate ΔHrxn for the combustion of ethanol. CH3CH2OH(g) + 3 O2(g) → 2 CO2(g) + 3 H2O(g)

2906
views
교과서 질문

Write an appropriate Lewis structure for each compound. Make certain to distinguish between ionic and molecular compounds. b. ClF5

586
views
교과서 질문

In the Chemistry and the Environment box on free radicals in this chapter, we discussed the importance of the hydroxyl radical in reacting with and eliminating many atmospheric pollutants. However, the hydroxyl radical does not clean up everything. For example, chlorofluorocarbons—which destroy stratospheric ozone—are not attacked by the hydroxyl radical. Consider the hypothetical reaction by which the hydroxyl radical might react with a chlorofluorocarbon: OH(g) + CF2Cl2(g) → HOF(g) + CFCl2(g) Use bond energies to explain why this reaction is improbable. (The C–F bond energy is 552 kJ/mol.)

734
views
교과서 질문

Hydrogenation reactions are used to add hydrogen across double bonds in hydrocarbons and other organic compounds. Use average bond energies to calculate ΔHrxn for the hydrogenation reaction. H2C=CH2(g) + H2(g) → H3C–CH3(g)

2669
views
1
rank
교과서 질문

Which of the two compounds, H2NNH2 and HNNH, has the strongest nitrogen-nitrogen bond, and which has the shorter nitrogen-nitrogen bond.

1937
views