Using the information in Figure 16-2, calculate the values of ∆H° for the following reactions:
(c)

검증된 단계별 안내

Step 1: Identify the reaction type. The given reaction is a hydrogenation reaction where one double bond in cyclohexene is reduced to form cyclohexane using hydrogen gas and a catalyst.

Step 2: Understand the enthalpy change (∆H°) for hydrogenation reactions. Hydrogenation reactions typically release energy, and the enthalpy change is negative. The value of ∆H° for hydrogenation of one double bond can be found in Figure 16-2 or similar reference data.

Step 3: Locate the ∆H° value for the hydrogenation of a single double bond in the reference figure. This value is specific to the reaction of converting cyclohexene to cyclohexane.

Step 4: Write the balanced chemical equation for the reaction:

{C 6 H 10}_{+ H 2 \to C 6 H 12}

. This equation represents the addition of hydrogen to cyclohexene.

Step 5: Use the ∆H° value from the reference figure to calculate the enthalpy change for the reaction. Ensure the units are consistent (e.g., kJ/mol) and interpret the negative sign as energy released during the reaction.

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.

Enthalpy Change (∆H°)

Enthalpy change (∆H°) is a measure of the heat content of a system at constant pressure. It indicates whether a reaction is exothermic (releases heat, ∆H° < 0) or endothermic (absorbs heat, ∆H° > 0). Calculating ∆H° for a reaction involves using standard enthalpies of formation for the reactants and products, allowing chemists to predict energy changes during chemical transformations.

Catalysis

Catalysis refers to the process of increasing the rate of a chemical reaction by adding a substance known as a catalyst. In the reaction shown, a catalyst facilitates the hydrogenation of benzene to cyclohexane, lowering the activation energy required for the reaction to proceed. Catalysts are not consumed in the reaction, allowing them to be used repeatedly in multiple reaction cycles.

Hydrogenation

Hydrogenation is a chemical reaction that involves the addition of hydrogen (H₂) to an unsaturated compound, such as an alkene or an aromatic compound. In this case, benzene, an aromatic compound, reacts with hydrogen in the presence of a catalyst to form cyclohexane, a saturated compound. This process is significant in organic chemistry for converting unsaturated hydrocarbons into more stable saturated forms.

Using the information in Figure 16-2, calculate the values of ∆H° for the following reactions:(c)