Dynamic equilibrium, equilibria involving physical processes, Henry's law - One Line Questions

1. Consider the reversible reaction A + B <=> C + D. If the system is at equilibrium, which statement is correct? — Rate of forward reaction = Rate of reverse reaction
2. If the Henry's law constant for a gas is 1.25 x 10^5 atm at a certain temperature, and the mole fraction of the gas in the liquid is 0.01, what is the partial pressure of the gas? — 1250 atm
3. The equilibrium that involves changes in physical states, such as melting or boiling, is called: — Physical equilibrium
4. When ice melts at 0°C and 1 atm pressure, the system is in: — Dynamic equilibrium between solid and liquid phases
5. In a saturated solution in contact with excess solute, the process of dissolution and crystallization are in equilibrium. This is a type of: — Physical equilibrium
6. The equilibrium between liquid water and steam at 100°C and 1 atm is an example of: — Phase equilibrium
7. The equilibrium constant for a physical equilibrium involving phase change is typically related to: — Vapor pressures of liquids or solids.
8. Dynamic equilibrium is characterized by: — Constant rates of forward and reverse processes.
9. The equilibrium between a solid and its vapor is characterized by: — Constant vapor pressure at a given temperature.
10. The phenomenon of 'the bends' or decompression sickness is related to the application of which law? — Henry's Law
11. According to Henry's Law, if the mole fraction of a gas in a solution increases, its partial pressure above the solution will: — Increase
12. When a diver ascends from a deep sea dive, the rapid decrease in external pressure causes dissolved gases in the blood to form bubbles. This is a consequence of: — Decreased solubility of gases at lower pressure (Henry's Law).
13. Which of the following is an example of equilibrium involving physical processes? — Dissolving of sugar in water to form a saturated solution
14. Which of the following physical processes is LEAST likely to be described by Henry's Law? — Dissolving ammonia in water.
15. When a gas is dissolved in a liquid, the process is generally: — Exothermic and leads to a decrease in entropy.
16. According to Henry's Law, the solubility of a gas in a liquid is proportional to the partial pressure of the gas above the liquid. If the partial pressure is doubled, the solubility will: — Double
17. If KH for a gas is very high, it means the gas is: — Sparingly soluble in the solvent.
18. Henry's Law is applicable to: — Dilute solutions only
19. For most gases, the value of KH increases with increasing temperature. This implies that the solubility of these gases in liquids: — Decreases with increasing temperature.
20. Henry's Law states that the partial pressure of a gas in equilibrium with a liquid is: — Directly proportional to its mole fraction in the liquid.
21. Which of the following statements about dynamic equilibrium is incorrect? — It means that the reaction has reached completion.
22. Which of the following is a characteristic of a system at equilibrium? — It is dynamic.
23. Carbonated beverages are bottled under high pressure of carbon dioxide. When the bottle is opened, the pressure decreases, and CO2 comes out of solution. This illustrates: — Henry's Law
24. When a liquid is heated to its boiling point at a given pressure, the equilibrium established is between: — Liquid and gas phases
25. At equilibrium, the rate of sublimation of a solid is equal to the rate of: — Deposition
26. Which physical process reaches dynamic equilibrium when the rate of evaporation equals the rate of condensation? — Evaporation of a liquid in a closed container
27. The temperature at which the vapor pressure of a liquid is equal to the external pressure is called the: — Boiling point
28. Which of the following is an example of physical equilibrium? — H2O(l) <=> H2O(g)
29. Which of the following gases is least soluble in water at room temperature and pressure, according to Henry's Law trends? — Nitrogen
30. Which of the following is a consequence of Henry's Law in biological systems? — All of the above
31. The equilibrium between solid iodine and iodine vapor is an example of: — Phase equilibrium
32. The constant KH in Henry's law has units of: — Pressure per mole fraction (e.g., atm/mole fraction)
33. According to Henry's Law, the solubility of gases like O2 and N2 in blood at sea level is sufficient for respiration. However, during deep dives, the increased partial pressure leads to: — Increased solubility of these gases.
34. Henry's Law is an empirical law that describes the behavior of: — Gas-liquid equilibria.
35. The equilibrium established between solid solute and its saturated solution is called: — All of the above
36. The equilibrium between a liquid and its vapor at a constant temperature is known as: — Phase equilibrium
37. Which factor does NOT affect the position of physical equilibrium for a solid-liquid phase transition at constant pressure? — Presence of an inert gas
38. The Henry's law constant (KH) is dependent on: — The nature of the gas and the solvent, and temperature.
39. The solubility of gases in liquids generally decreases with an increase in temperature because: — The dissolution process is usually exothermic.
40. A system is at equilibrium when: — The forward and reverse reaction rates are equal.
41. Mathematically, Henry's Law is expressed as P = KH * X, where P is the partial pressure of the gas, KH is the Henry's law constant, and X is: — The mole fraction of the gas in the liquid.
42. Which statement is NOT true for a system at dynamic equilibrium? — The reaction has stopped.
43. Consider the equilibrium: H2O(l) <=> H2O(g). The vapor pressure of water at a given temperature is: — The partial pressure of H2O(g) at equilibrium.
44. The equilibrium constant for the physical process of sublimation (Solid <=> Gas) is directly related to: — The vapor pressure of the solid.
45. The equilibrium between a solution and undissolved solid is characterized by: — The rate of dissolution being equal to the rate of precipitation.
46. A system is at equilibrium when: — The rates of forward and reverse processes are equal and non-zero.
47. Which of the following best describes dynamic equilibrium in a reversible reaction? — The rate of the forward reaction is equal to the rate of the reverse reaction.
48. Which of the following conditions is necessary for dynamic equilibrium? — The system must be closed.
49. In a system at dynamic equilibrium, what is true about the macroscopic properties? — They remain constant.
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