Calculate ∆ H ° for the following reactions. (c) CH 3 CH 3 + HOOH → CH 3 CH 2 OH + H 2 O

Hello everyone. Today we have a following problem. What does he change in for the reaction given below to calculate for the change of entropy? We will use the following equation that states that the change in our entropy is equal to the bond dissociation energies of our bonds broken or BB subtracted by our bond association energies of our bonds formed. Or BF if we look at our reaction, we see that we have a hidden hydrogen attached to that met carbon on the left, we see that this was broken and this carbon oxygen bond was formed. Moreover, we see that this bond between these two oxygens was broken and a new bond between an oxygen and hydrogen was formed. So plugging in our values for our bonds broken, we see that we broke essentially a secondary carbon hydrogen bond. So we have three 97 kill the jules promo add it to the other bone that was broken the two between the bond between the two oxygens, which is 213 kilojoules per mole. And then we subtracted by the bonds associated energies of the bonds that were formed. We formed a carbon oxygen bond. So that's 381 kilojoules per month. And then we add that to the other bond that was formed or the oxygen hydrogen bond, which is 498 kilojoules per mole. Solving the math for the answer, we arrive at an answer of negative 269 kilojoules per mole or enter choice D overall. I hope this helped. And until next time.

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6. Thermodynamics and Kinetics

Enthalpy

Organic Chemistry

6. Thermodynamics and Kinetics

Enthalpy

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Problem 37c

Textbook Question

Calculate ∆H° for the following reactions.
(c) CH₃CH₃ + HOOH → CH₃CH₂OH + H₂O

Verified step by step guidance

Step 1: Understand the problem. The goal is to calculate the enthalpy change (∆H°) for the given reaction. This involves using bond dissociation energies (BDEs) to determine the energy required to break bonds in the reactants and the energy released when bonds are formed in the products.

Step 2: Write out the bonds involved in the reactants and products. In the reactants, CH3CH3 contains C-H and C-C bonds, and HOOH contains O-H and O-O bonds. In the products, CH3CH2OH contains C-H, C-C, C-O, and O-H bonds, and H2O contains O-H bonds.

Step 3: Use a table of bond dissociation energies to find the BDE values for each bond type. For example, the BDE for a C-H bond is approximately 412 kJ/mol, for a C-C bond is 348 kJ/mol, for an O-H bond is 463 kJ/mol, and for an O-O bond is 146 kJ/mol. Ensure you have accurate values for all bonds involved.

Step 4: Calculate the total energy required to break all bonds in the reactants. Multiply the BDE of each bond by the number of such bonds in the reactants and sum them up. For example, if CH3CH3 has 6 C-H bonds and 1 C-C bond, calculate the energy for breaking all these bonds.

Step 5: Calculate the total energy released when bonds are formed in the products. Multiply the BDE of each bond by the number of such bonds in the products and sum them up. Subtract the energy released from the energy required to break bonds to find ∆H° for the reaction.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Enthalpy Change (∆H°)

Enthalpy change (∆H°) refers to the heat content change of a system at constant pressure during a chemical reaction. It indicates whether a reaction is exothermic (releases heat, ∆H° < 0) or endothermic (absorbs heat, ∆H° > 0). Understanding how to calculate ∆H° is crucial for predicting the energy changes associated with chemical reactions.

Hess's Law

Hess's Law states that the total enthalpy change for a reaction is the sum of the enthalpy changes for the individual steps of the reaction, regardless of the pathway taken. This principle allows chemists to calculate ∆H° for reactions that may be difficult to measure directly by using known enthalpy changes of related reactions.

Standard State Conditions

Standard state conditions refer to the specific set of conditions (usually 1 atm pressure and 25°C) under which the enthalpy values are measured. It is essential to use standard state values when calculating ∆H° to ensure consistency and comparability of thermodynamic data across different reactions.

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