Phenol, c6h5oh, is a stronger acid than methanol, ch3oh, even though both contain an o]h bond. Draw the structures of the anions
resulting from loss of h1 from phenol and methanol, and use resonance structures to explain the difference in acidity.
1 answer:
In resonance structures, the chemical connectivity in the molecule is same but the distribution of electrons are different around the structure. They are created by moving electrons in double or triple bonds, and not atoms.
Phenol, and methanol,
both are alcohols that contain an
group attached to carbon atom.
Due to loss of 1 from phenol, it forms phenoxide anion and due to presence of double bond in the benzene ring the negative charge on the oxygen atom (which represents electrons) will resonate with double bonds of benzene ring as shown in the image. The resonance-stabilized phenoxide ion is more stable. Whereas when methanol lose 1
it forms methoxide anion and there are no such electrons present in the structure of methoxide that will result in the movement of electron. Since, due to resonance-stabilized phenoxide ion is more stable than methoxide ion, so it is a stronger acid.
The structures of the anions resulting from loss of 1 from phenol and methanol is shown in the image.
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Answer : The value of is, 11.2
The value of is -9.04 kJ/mol
Explanation :
The relation between the equilibrium constant and standard Gibbs free energy is:
where,
= standard Gibbs free energy = -5.980 kJ/mol = -5980 J/mol
R = gas constant = 8.314 J/K.mol
T = temperature =
= equilibrium constant = ?
Now put all the given values in the above formula, we get:
Thus, the value of is, 11.2
Now we have to calculate the .
The formula used for is:
The given reaction is:
............(1)
where,
= Gibbs free energy for the reaction = ?
= standard Gibbs free energy = -30.5 kJ/mol
R = gas constant =
T = temperature =
Q = reaction quotient
[A] = concentration of A = 1.8 M
[B] = concentration of B = 0.55 M
Now put all the given values in the above formula 1, we get:
Therefore, the value of is -9.04 kJ/mol
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