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Ch.15 - Chemical Equilibrium
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 14th EditionCh.15 - Chemical Equilibrium문제 66a
15장, 문제 66a

Methanol (CH3OH) can be made by the reaction of CO with H2: CO(𝑔) + 2 H2(𝑔) ⇌ CH3OH(𝑔) (a) Use thermochemical data in Appendix C to calculate ΔH° for this reaction.

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1
Identify the standard enthalpy of formation (ΔH_f°) for each compound involved in the reaction from Appendix C.
Write the balanced chemical equation for the reaction: CO(g) + 2 H_2(g) ⇌ CH_3OH(g).
Use the formula for the standard enthalpy change of the reaction: ΔH° = Σ(ΔH_f° of products) - Σ(ΔH_f° of reactants).
Substitute the ΔH_f° values for CH_3OH(g), CO(g), and H_2(g) into the formula. Remember that the ΔH_f° for elements in their standard state, like H_2(g), is zero.
Calculate the sum of the enthalpies for the products and the reactants separately, then find the difference to determine ΔH° for the reaction.

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주요 개념

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Thermochemical Data

Thermochemical data includes information about the enthalpy changes associated with chemical reactions. This data is often found in tables and can provide standard enthalpy of formation values (ΔH°f) for various substances. By using these values, one can calculate the overall enthalpy change (ΔH°) for a reaction by applying Hess's law, which states that the total enthalpy change is the sum of the enthalpy changes for individual steps.
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가이드 코스
01:13
Thermochemical Equations

Hess's Law

Hess's Law states that the total enthalpy change for a chemical reaction is the same, regardless of the number of steps or the pathway taken. This principle allows chemists to calculate the enthalpy change of a reaction by summing the enthalpy changes of individual reactions that lead to the same products. It is particularly useful when direct measurement of ΔH° is difficult or impossible.
추천 영상:
가이드 코스
02:03
Hess's Law

Standard Enthalpy of Formation (ΔH°f)

The standard enthalpy of formation (ΔH°f) is defined as the change in enthalpy when one mole of a compound is formed from its elements in their standard states. This value is crucial for calculating the enthalpy change of a reaction using the formula ΔH° = ΣΔH°f(products) - ΣΔH°f(reactants). Understanding how to use ΔH°f values allows for the determination of the energy changes involved in chemical reactions.
추천 영상:
가이드 코스
02:34
Enthalpy of Formation
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교과서 질문

Consider the following equilibrium between oxides of nitrogen 3 NO(g) ⇌ NO2(g) + N2O(g) (a) Use data in Appendix C to calculate ΔH° for this reaction.

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교과서 질문

Consider the following equilibrium between oxides of nitrogen

3 NO(g) ⇌ NO2(g) + N2O(g)

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교과서 질문

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