The Henry's law constant (K_H) values for N₂ at 293 K and 303 K are 76.48 and 88.84 kbar respectively. This shows that:
AThe solubility of N₂ in water decreases with temperature
BThe solubility of N₂ in water increases with temperature
CN₂ does not obey Henry's law
DK_H is independent of temperature
Answer & Solution
Correct answer: A. The solubility of N₂ in water decreases with temperature
Since p = K_H × x → for the same partial pressure, **larger K_H means smaller x** → **lower solubility**. K_H rising with T → solubility falls with T. This is why warmer waters hold less dissolved oxygen.
Related questions
The mass of NaOH (M = 40 g/mol) required to prepare 500 mL of a 0.20 M NaOH solution isWhich of these solutions will boil at the highest temperature at 1 atm?The molality of a 1 M aqueous NaCl solution (density = 1.04 g/mL, NaCl M = 58.5 g/mol) is Osmotic pressure π of a dilute solution obeys π = C R T. Here C representsVan't Hoff factor i > 1 for a solute indicatesA negative deviation from Raoult law is expected whenIf a solute dimerises in solution, its observed molar mass compared with the calculated vaWhich of the following is NOT a colligative property?