Answers:
Q36 (2); Q37 (2); Q38 (2)
Step-by-step explanation:
Entropy is a measure of the degree of disorder in a system. If the molecules have more freedom to move around, the entropy of the system increases.
Q36.
H₂O(ℓ) + heat ⇌ H₂O(g)
If the temperature is increased, you are adding heat to the system.
According to Le Châtelier's Principle, the system will respond by trying to get rid of the heat.
The position of equilibrium will move to the right, forming more H₂O(g).
Since you are forming more moles of gas, the entropy of the system will increase.
(1) is wrong, because increasing the temperature increases the average kinetic energy of the molecules.
(3) is wrong, because the system forms more moles of H₂O(g).
(4) is wrong, because the position of equilibrium shifts to the right, decreasing the moles of H₂O(ℓ).
Q37.
NaCl(s) ⟶ Na⁺(aq) + Cl⁻(aq)
As NaCl dissolves, the entropy of the system increases, because the ions are free to move throughout the solution instead of being locked in a solid crystal.
Q38.
H₂O(s) ⟶ H₂O(ℓ)
This change results in an increase of entropy, because the water molecules are free to move around instead of being locked in a crystal of ice.
All the other options are wrong, because they result in a decrease of freedom of motion of the molecules.
