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.

검증된 단계별 안내

Identify the standard enthalpies of formation (ΔH°f) for each compound involved in the reaction from Appendix C. You will need the values for NO(g), NO₂(g), and N₂O(g).

Write the balanced chemical equation for the reaction: 3 NO(g) ⇌ NO₂(g) + N₂O(g).

Apply the formula for the standard enthalpy change of the reaction (ΔH°rxn): ΔH°rxn = ΣΔH°f(products) - ΣΔH°f(reactants). Remember to multiply the ΔH°f of each substance by its stoichiometric coefficient in the balanced equation.

Calculate the sum of the standard enthalpies of formation for the products: (1 mole of NO₂(g) × ΔH°f of NO₂(g)) + (1 mole of N₂O(g) × ΔH°f of N₂O(g)).

Calculate the sum of the standard enthalpies of formation for the reactants: 3 moles of NO(g) × ΔH°f of NO(g).

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

주요 개념

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

Hess's Law

Hess's Law states that the total enthalpy change for a chemical reaction is the sum of the enthalpy changes for the individual steps of the reaction, regardless of the pathway taken. This principle allows for the calculation of ΔH° for reactions that may not be easily measured directly by using known enthalpy changes of related reactions.

Standard Enthalpy of Formation (ΔH°f)

The standard enthalpy of formation (ΔH°f) is 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 Hess's Law, as it provides a reference point for the energy content of reactants and products.

Equilibrium Constant (K)

The equilibrium constant (K) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. Understanding K is essential for analyzing the position of equilibrium and how changes in conditions can affect the reaction, which is relevant when considering the enthalpy changes in reactions involving gases.

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.