When H2 and CO2 react, acetic acid can be formed spontaneously while the production of formaldehyde requires an input of energy.
Which of the following conclusions may be drawn from this observation?
a. More heat is released when formaldehyde is produced compared to the production of acetic acid.
b. Compared to the reactants from which it is formed, formaldehyde has more potential energy than does acetic acid.
c. Entropy decreases when acetic acid is produced and increases when formaldehyde is produced.
d. The mineral catalyst involved in acetic acid production provides energy to make the reaction spontaneous.
a. More heat is released when formaldehyde is produced compared to the production of acetic acid.
b. Compared to the reactants from which it is formed, formaldehyde has more potential energy than does acetic acid.
c. Entropy decreases when acetic acid is produced and increases when formaldehyde is produced.
d. The mineral catalyst involved in acetic acid production provides energy to make the reaction spontaneous.
1 answer:
Answer:
Compared to the reactants from which it is formed, formaldehyde has more potential energy than does acetic acid.
Explanation:
Some atoms tend to attain a minimum potential energy when atoms interact in certain ways. This interaction lowers the potential energy of the system involving the two atoms. This minimum energy point usually refer to overlap between atoms in a covalent bond. The closer the nuclei of the two atoms, the lower the potential energy of the bonded interaction.
If a specie takes more time to form, then it has a lower potential energy, its minima occurs much lower in the plot shown in the image attached.
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Answer:
a) 79.66 seconds is the half-life of the reaction.
b) It will take seconds for 34% of a sample of an acetone to decompose.
c) It will take seconds for 89% of a sample of an acetone to decompose.
Explanation:
The decomposition of acetone follows first order kinetics
The rate constant of the reaction = k =
a)
Half life of the reaction =
For the first order kinetic half life is related to k by :
79.66 seconds is the half-life of the reaction.
b)
Let the initial concentration of acetone be =
Final concentration of acetone left after t time = [A]
For the first order kinetic :
Solving for t;
It will take 47.76 seconds for 34% of a sample of an acetone to decompose.
c)
Let the initial concentration of acetone be =
Final concentration of acetone left after t time = [A]
For the first order kinetic :
Solving for t;
It will take seconds for 89% of a sample of an acetone to decompose.