이산화 황

이산화 황
Skeletal formula sulfur dioxide with assorted dimensions
Spacefill model of sulfur dioxide
The Lewis structure of sulfur dioxide (SO2), showing unshared electron pairs.
이름
IUPAC 이름
Sulfur dioxide
별칭
Sulfurous anhydride
Sulfur(IV) oxide
식별자
3D 모델 (JSmol)
3535237
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.028.359
EC 번호
  • 231-195-2
E 번호 E220 (방부제)
1443
KEGG
MeSH Sulfur+dioxide
RTECS 번호
  • WS4550000
UNII
UN 번호 1079, 2037
  • InChI=1S/O2S/c1-3-2 예
    Key: RAHZWNYVWXNFOC-UHFFFAOYSA-N 예
  • InChI=1/O2S/c1-3-2
    Key: RAHZWNYVWXNFOC-UHFFFAOYAT
  • O=S=O
성질
SO
2
몰 질량 64.066 g mol−1
겉보기 Colorless gas
냄새 Pungent; similar to a just-struck match[1]
밀도 2.6288 kg m−3
녹는점 −72 °C; −98 °F; 201 K
끓는점 −10 °C (14 °F; 263 K)
94 g/L[2]
forms sulfurous acid
증기 압력 237.2 kPa
산성도 (pKa) 1.81
염기도 (pKb) 12.19
−18.2·10−6 cm3/mol
점도 12.82 μPa·s[3]
구조
C2v
Digonal
Dihedral
1.62 D
열화학
248.223 J K−1 mol−1
−296.81 kJ mol−1
위험
GHS 그림문자 GHS05: Corrosive GHS06: Toxic
신호어 위험
H314, H331[4]
NFPA 704 (파이어 다이아몬드)
NFPA 704 four-colored diamondFlammability code 0: Will not burn. E.g. waterHealth code 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
0
3
0
반수 치사량 또는 반수 치사농도 (LD, LC):
3000 ppm (mouse, 30 min)
2520 ppm (rat, 1 hr)[6]
993 ppm (rat, 20 min)
611 ppm (rat, 5 hr)
764 ppm (mouse, 20 min)
1000 ppm (human, 10 min)
3000 ppm (human, 5 min)[6]
NIOSH (미국 건강 노출 한계):
PEL (허용)
TWA 5 ppm (13 mg/m3)[5]
REL (권장)
TWA 2 ppm (5 mg/m3) ST 5 ppm (13 mg/m3)[5]
IDLH (직접적 위험)
100 ppm[5]
관련 화합물
관련 산화물
Sulfur monoxide
Sulfur trioxide
관련 화합물
Ozone

Selenium dioxide
Sulfurous acid
Tellurium dioxide

달리 명시된 경우를 제외하면, 표준상태(25 °C [77 °F], 100 kPa)에서 물질의 정보가 제공됨.
아니오아니오 확인 (관련 정보 예아니오아니오 ?)

이산화 황(二酸化黃, sulfur dioxide)은 화학식 SO2인 무기 화합물이며, 아황산 가스, 무수 아황산이라고도 부른다. 산소 원자 2개와 원자 1개가 결합되어 있다. 색깔이 없으며 자극적인 냄새가 나는 유독성 기체이다. 화산 활동이나 유기 물질이 분해될 때 자연적으로 생긴다. 공업적으로는 황을 태우거나 황을 포함한 금속 화합물을 가열하여 만들며, 실험실에서는 아황산염에 을 가하여 얻는다. 공장이나 발전소에서는 이산화 황이 대기중으로 들어오는데, 이때 공기중에 이산화 황이 기준치보다 높으면 눈에 염증이 생기거나 호흡기 질환이 일어난다. 또한 알레르기를 일으킬 수 있으며, 심하면 사망에 이르기도 한다. 직물의 표백제나 식품 방부제 등으로 쓰인다.

공해 손해배상소송

공장에서 배출된 오염물질(아황산가스)의 농도가 환경보전법에 의하여 허용된 기준치 이내라 하더라도 그 유해의 정도가 통상의 수인한도를 넘어 인근 농장의 관상수를 고사케하는 한 원인이 되었다면 그 배출행위로 인한 손해배상책임을 면치 못한다.[7]

각주

  1. Sulfur dioxide Archived 2019년 12월 30일 - 웨이백 머신, U.S. National Library of Medicine
  2. Lide, David R., 편집. (2006). 《CRC Handbook of Chemistry and Physics》 87판. Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3. 
  3. Miller, J.W. Jr.; Shah, P.N.; Yaws, C.L. (1976). “Correlation constants for chemical compounds”. 《Chemical Engineering》 83 (25): 153–180. ISSN 0009-2460. 
  4. https://echa.europa.eu/information-on-chemicals/cl-inventory-database/-/discli/notification-details/115657/1409763
  5. NIOSH Pocket Guide to Chemical Hazards. “#0575”. 미국 국립 직업안전위생연구소 (NIOSH). 
  6. “Sulfur dioxide”. 《Immediately Dangerous to Life and Health Concentrations (IDLH)》. National Institute for Occupational Safety and Health (NIOSH). 
  7. 대법원 1991.7.23, 선고, 89다카1275, 판결

같이 보기

참고 자료

이 문서에는 다음커뮤니케이션(현 카카오)에서 GFDL 또는 CC-SA 라이선스로 배포한 글로벌 세계대백과사전의 내용을 기초로 작성된 글이 포함되어 있습니다.

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