Using data from Appendix 4, calculate ΔH^5, ΔS^∘, and ΔG^∘...

Using data from Appendix 4, calculate $\Delta H^{5}, \Delta S^{\circ}$, and $\Delta G^{\circ}$ for the following reactions that produce acetic acid: Which reaction would you choose as a commercial method for producing acetic acid $\left(\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}\right)$ at standard conditions? What temperature conditions would you choose for the reaction? Assume $\Delta H^{\circ}$ and $\Delta S^{\circ}$ do not depend on temperature.

Using data from Appendix 4, calculate $\Delta H^{5}, \Delta S^{\circ}$, and $\Delta G^{\circ}$ for the following reactions that produce acetic acid:
Which reaction would you choose as a commercial method for producing acetic acid $\left(\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}\right)$ at standard conditions? What temperature conditions would you choose for the reaction? Assume $\Delta H^{\circ}$ and $\Delta S^{\circ}$ do not depend on temperature.

Key Concepts

Standard State Conditions

Standard state conditions, typically defined at 298 K and 1 atm, provide a common baseline for reporting and comparing thermodynamic data. Using these conditions enables the consistent evaluation of reactions, ensuring that decisions such as choosing the most favorable reaction route for producing acetic acid are based on comparable and standardized data.

Relationship Between ?G, ?H, and ?S

The fundamental thermodynamic equation ?G = ?H - T?S connects enthalpy and entropy to the overall free energy change. This relationship explains how temperature can shift the balance between enthalpic and entropic contributions, thereby determining the conditions under which a reaction becomes spontaneous, an essential consideration in process optimization.

Gibbs Free Energy (?G)

Gibbs free energy combines the effects of enthalpy and entropy to determine a reaction's spontaneity under constant temperature and pressure conditions. A negative ?G indicates a thermodynamically favored process, making this a key criterion in selecting an optimal reaction pathway for commercial production.

Enthalpy (?H)

Enthalpy represents the total heat content of a system and indicates whether a reaction is exothermic or endothermic. In reaction analysis, ?H is used to determine the energy change when reactants convert to products, which is crucial for evaluating the feasibility and cost implications of a chemical process.

Entropy (?S)

Entropy is a measure of disorder or randomness within a system. Changes in entropy (?S) during a reaction help in understanding how the molecular arrangement and energy distribution change, which in turn influences the overall spontaneity of the reaction, especially when temperature effects are considered.

Transcript

00:01 In this problem, our first order of business will be to calculate these three entities for the following reactions at standard conditions.

00:23 So let's begin.

00:24 We'll do equation one and equation two.

00:27 For equation one, we will use our delta h will be equal to, are we ready? this is negative 484 and this is 160.

01:11 I should give you a little bit more room here, but you'll be able to tell where they all are.

01:14 Okay, so let's start.

01:15 Negative 484 times 1 minus methane is negative 75 times 1 plus 1 times negative 393 .5.

01:37 So this will equal negative 16 kilojoules.

01:44 For my delta s, this will equal 1 times 160 minus 1 times 186 plus 1 times 214.

02:10 And this will equal negative 240 joules per kelvin.

02:19 And my delta g will equal one times, oh, let's do it this way.

02:31 This will equal my delta h minus my delta h times my delta s t times delta s.

02:52 So this will equal negative 16 kilojoules minus 298 times negative 240 joules per kelvin times 1 ,000 joules per kilojoule.

03:12 And this will equal positive 56 kilojoules.

03:18 So this will be spontaneous below t equals negative h over, excuse me, delta.

03:44 It and that will be 16 divided by 0 .240 that'll equal 67 kelvin that's too cold to be practical oh my pen just fell apart hang on here i captured it i don't want it to fall on the floor that was so weird okay practical okay it's still working that's good now let's do the second reaction, and let's do our delta h.

04:44 Again, it will be 1 times negative 44 minus 1 times, that will be negative 110 .5 plus 1 times negative 201, one and that will equal negative 173 kilojoules...

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