Correct Answer: C

Rationale: Henry's Law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. The equation P = kC represents Henry's Law, where P is the partial pressure of the gas, C is the concentration of the gas in the liquid, and k is a constant. This law is applicable to dilute solutions where the gas does not significantly affect the liquid's volume. Therefore, in the context of gas solubility in liquids, Henry's Law is the appropriate principle that describes the relationship between solubility and partial pressure. Boyle's Law relates the pressure and volume of a gas at constant temperature, Gay-Lussac's Law deals with the pressure and temperature relationship of a gas at constant volume, and Charles' Law describes the relationship between the volume and temperature of a gas at constant pressure. These laws are not directly related to the solubility of gases in liquids, making them incorrect choices for this question.

Correct Answer: D

Rationale: Boyle's law describes the relationship between the pressure and volume of an ideal gas when the temperature and amount of gas are constant. According to Boyle's law, if the pressure of a gas increases, its volume decreases proportionally, and vice versa. This law is expressed by the equation P1V1 = P2V2, where P1 and V1 represent the initial pressure and volume, while P2 and V2 represent the final pressure and volume when the temperature and amount of gas remain unchanged. Understanding Boyle's law is essential in comprehending the behavior of gases under varying conditions and is fundamental in the study of thermodynamics. The other choices are incorrect: - Henry's law deals with the solubility of gases in liquids, not the relationship between pressure and volume of gases. - Dalton's law states that the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of individual gases, not the pressure-volume relationship. - Brown's law is a fabricated concept and does not exist in the context of gas laws.

Correct Answer: B

Rationale: Oxygen typically has an oxidation number of -2 in compounds because it tends to gain electrons. This is due to its high electronegativity, which leads to oxygen attracting electrons towards itself in a chemical bond. Choice A (2) is incorrect because oxygen doesn't have a +2 oxidation number in compounds. Choice C (0) is incorrect as oxygen rarely has an oxidation number of 0 in compounds. Choice D (-1) is incorrect as oxygen's oxidation number in compounds is typically -2, not -1.

Correct Answer: A

Rationale: In the periodic table, the elements are arranged in order of increasing atomic number. This organization is based on the number of protons in the nucleus of each element. It provides a systematic way to classify elements and predict their properties. Knowing the atomic number of an element helps determine its placement in the periodic table and its characteristics. Therefore, the correct answer is the order of increasing atomic number as it is fundamental to the structure and properties of the elements. Choices B, C, and D are incorrect. Alphabetical order does not reflect any underlying property of the elements, metallic properties vary across the table, and neutron content alone is not the basis for the arrangement in the periodic table.

Correct Answer: B

Rationale: Water boils at 212°F under standard atmospheric pressure. This is the point at which water changes from a liquid to a gas phase. Choice A (210°F) is incorrect as it is below the boiling point of water. Choice C (215°F) and Choice D (220°F) are also incorrect as they are above the boiling point of water.