Henry의 법칙 (Henry’s law). 기체의 용해도와 압력 효과 ★

Henry의 법칙 (Henry’s law). 기체의 용해도와 압력 효과

 

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Henry’s law is one of the gas laws formulated by William Henry in 1803 and states:

“At a constant temperature, the amount of a given gas that dissolves in a given type and volume of liquid is directly proportional to the partial pressure of that gas in equilibrium with that liquid.”

 

일정 온도에서, 기체의 용해도(C)는 용액 위에 있는 기체의 부분 압력(P_gas)에 비례한다.

 

 

 

An equivalent way of stating the law is that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid:

 

C = k • P_gas

 

where

> C is the solubility of a gas at a fixed temperature in a particular solvent (often in units of M)

> k is Henry’s law constant (often in units of M/atm)

> P_gas is the partial pressure of the gas (often in units of atm)

 

 

 

 

[ 관련 글 https://ywpop.tistory.com/1911 ]

 

 

 

[키워드] Henry 법칙 기준문서, 헨리 법칙 기준문서, 헨리의 법칙 기준문서

 

 

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헨리의 법칙

P_g = k_H × X_g

기체의 부분 압력 = 기체의 헨리 상수 × 기체의 몰분율

( 관련 예제 https://ywpop.tistory.com/12551 )

 

 

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P = k_h • C

where

P = partial pressure of gas

C = concentration of gas

k_h = Henry’s law constant

 

 

The k_h is dependent on the solvent, the gas solute and the temperature.

k_h for some common gases:

> hydrogen (H2): 1228 atm/M (= atm•L/mol)

> carbon dioxide (CO2): 30 atm/M

> oxygen (O2): 757 atm/M

> nitrogen (N2): 1600 atm/M

> helium (He): 2865 atm/M

 

 

 

[ 관련 예제 https://ywpop.tistory.com/16261 ] 25℃ 공기 중 질소기체의 분압은 0.80 atm