Substances that can eat through metals and other containers are classified as _____. radioactive wastes toxic wastes corrosive w
2 answers:
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Answer:
I. Kindly, see the attached image.
II. The reaction is exothermic.
III. - 51.88 kJ/mol.
IV. The reaction is spontaneous.
Explanation:
I. Draw a possible potential energy diagram of the reaction. Label the enthalpy of the reaction.
- Since the sign of ΔH is negative, the reaction is exothermic reaction.
In an exothermic reaction, the energy of the reactants is higher than that of the products.
<u><em>Kindly see the attached image to show you the potential energy diagram of the reaction.</em></u>
<em>II. Is the reaction endothermic or exothermic? Explain your answer.</em>
- The reaction is exothermic reaction.
- The sign of ΔH indicates wither the reaction is endothermic or exothermic one:
If the sign is positive, the reaction is endothermic.
If the sign is negative, the reaction is exothermic.
Herein, <em>ΔH = - 33.1 kJ/mol, </em>so the reaction is exothermic.
<em>III. What is the Gibbs free energy of the reaction at 25°C? </em>
∵ ΔG = ΔH - TΔS.
Where, ΔG is the Gibbs free energy change (J/mol).
ΔH is the enthalpy change (ΔH = - 33.1 kJ/mol).
T is the temperature (T = 25°C + 273 = 298 K).
ΔS is the entorpy change (ΔS = 63.02 J/mol.K = 0.06302 J/mol.K).
<em>∴ ΔG = ΔH - TΔS</em> = (- 33.1 kJ/mol) - (298 K)(0.06302 J/mol.K) = <em>- 51.88 kJ/mol.</em>
IV. Is the reaction spontaneous or nonspontaneous at 25°C?
The sign of ΔG indicates the spontaneity of the reaction:
If ΔG < 0, the reaction is spontaneous.
If ΔG = 0, the reaction is at equilibrium.
If ΔG > 0, the reaction is nonspontaneous.
Herein, <em>ΔG = - 51.88 kJ/mol, </em>so the reaction is spontaneous.
Answer:
Lower
Explanation:
Surface tension occurs because molecules at the surface do not have molecules above them, so they cohere more strongly to their neighbours.
The stronger cohesive forces make it more difficult to move an object through the surface than when it is beneath the surface.
The attractive forces in water are strong because of hydrogen bonding.
A hexane molecule is nonpolar, so the only attractions are the weak London dispersion forces.
The cohesive forces at the surface are much lower than those in water, so the surface tension of hexane is lower than that of water at the sane temperature.
