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: 17.2 g
Explanation:
To calculate the moles :
The balanced chemical equation is:
According to stoichiometry :
4 moles of produce = 4 moles of
Thus 0.085 moles of will require=
of
Mass of
Thus 17.2 g of will be produced form 20.0 g of HgS.