A 100 milliliters (mL) sample of a liquid is poured from a beaker into a graduated cylinder. Which of the following best explain
1 answer:
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Answer:
For A: The change in free energy for the reaction is -5339.76 J/mol
For B: Free energy change is expressed in kJ/mol
For C: The forward reaction favors progression, while the reverse reaction does not.
Explanation:
Regarding the specified chemical reaction:
- For A:
The relationship between standard Gibbs free energy and equilibrium constant is as follows:
The free energy change can be calculated using the following equation:
Or,
where,
= Change in free energy
R = Gas constant =
= standard temperature =
T = temperature of the cell =
= equilibrium constant =
Q = reaction quotient =
= 0.06 M
[DHAP] = 0.125 M
Substituting the values into the equation yields:
Thus, the change in free energy for the reaction is -5339.76 J/mol
- For B:
To convert the free energy change to kilojoules, we apply the conversion factor:
1 kJ = 1000 J
So,
Consequently, the free energy change's units are kJ/mol
- For C:
For spontaneity in the reaction, the Gibbs free energy must be negative. However, the calculations indicate a positive Gibbs free energy, leading to the conclusion that the reaction is not spontaneous.
The free energy change of the reaction is negative.
Consequently, the forward reaction is favored and the reverse reaction is not favored.