Question

Acetic acid is responsible for the sour taste of vinegar. It can be manufactured using the following reaction: ​Acetic acid is responsible for the sour taste of vinegar. It can be manufactured using the following reaction: CH₃OH+CO→CH₃COOH Use tabulated values of bond energies from Table A4.1 in your text to estimate ΔH, in kJ, for this reaction.

Answer 1

Answer: To the estimated enthalpy change (ΔH) for the reaction is approximately −568kJ. This negative value indicates that the reaction is exothermic, meaning it releases heat to the surroundings.
`CH_(3)`

Step-by-step explanation:ΔH=Σbond energies of bonds broken−Σbond energies of bonds formed

step 1 Identify the bonds broken and formed in the reaction:

Bonds broken:

One C-O bond in CH_{3} OH

One C=O bonds in CO

Bonds formed:

One C=O bonds in CH_{3} COOH

Two O-H bonds in CH_{3} COOH

step 2 Find the bond energies from Table A4.1:

Bond energies (in kJ/mol):

C-O single bond: 358

C=O double bond: 799

O-H bond: 463 (approximate average for O-H bonds)

step3 Calculate the energy change for the bonds broken:

Bonds broken:

One C-O bond in CH_{3} OH = 358kJ/mol

One C=O bond in CO = 799kJ/mol

Total energy for bonds broken = 358+799=1157kJ/mol

step 4 Calculate the energy change for the bonds formed:

Bonds formed:

One C=O bond in CH_{3} COOH = 799kJ/mol

Two O-H bonds in CH_{3} COOH = 2×463=926kJ/mol

Total energy for bonds formed = 799+926=1725kJ/mol

step 5 Now, apply the formula for ΔH:

ΔH=Energy of bonds broken−Energy of bonds formed

ΔH=1157kJ/mol−1725kJ/mol=−568kJ/mol

the estimated enthalpy change (ΔH) for the reaction is approximately −568kJ. This negative value indicates that the reaction is exothermic, meaning it releases heat to the surroundings.

Answer 2

The estimated enthalpy change
`($\Delta H$)` for the formation of acetic acid is
`\(208 \, \text{kJ/mol}\).`

The reaction for the formation of acetic acid (CH3COOH) can be broken down into its constituent bond energies:

`\[ \text{CH}_3\text{OH} + (1)/(2)\text{O}_2 \rightarrow \text{CH}_3\text{OOH} \]`

Breaking bonds:

- Breaking the
`$\text{C}-\text{H}$ bonds in CH3OH (methanol): \(4 * 413 \, \text{kJ/mol}\)`

- Breaking the
`$\text{O}-\text{H}$ bond in $(1)/(2)\text{O}_2$: \(1 * 467 \, \text{kJ/mol}\)`

Forming bonds:

- Forming the
`$\text{C}-\text{O}$ bond in CH3OOH (acetic acid): \(2 * 358 \, \text{kJ/mol}\)`

- Forming the
`$\text{C}=\text{O}$ bond in CH3OOH: \(1 * 745 \, \text{kJ/mol}\)`

Now, let's calculate the total bond energies involved:

`\[ \Delta H = \text{Energy of bonds broken} - \text{Energy of bonds formed} \]`

`\[ \Delta H = (4 * 413 \, \text{kJ/mol}) + (1 * 467 \, \text{kJ/mol}) - (2 * 358 \, \text{kJ/mol}) - (1 * 745 \, \text{kJ/mol}) \]`

`\[ \Delta H = 1652 + 467 - 716 - 745 \, \text{kJ/mol} \]`

`\[ \Delta H = 1669 - 1461 \, \text{kJ/mol} \]`

`\[ \Delta H = 208 \, \text{kJ/mol} \]`

Question:

Acetic acid is responsible for the sour taste of vinegar. It can be manufactured using the following reaction: