Sulfur Daily Question, March 27------5 wealth for participation, 10 wealth for correct answers
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This post was last edited by Sulfur-Zinc-Aluminum on 2016-3-28 at 14:50. There’s no need for anyone to hide the answers anymore; I have already set the responses to be visible only to the author. . . Short answer: What are the basic properties of sulfur dioxide?
An extremely pungent smell, almost suffocating~
⑴Physical properties: Typically, SO2 is a colorless, toxic gas with an irritating odor; it has a density greater than that of air, is easy to liquefy, and is soluble in water. ⑵Chemical properties: ① SO2- is an acidic oxide and possesses the general properties of acidic oxides. == ； SO2+CaO=CaSO3 ； SO2+2NaOH=Na2SO3+H2O ； SO2 + NaOH = NaHSO3 (similar to the reaction of CO2 with a base). NH3·H2O or Ca(OH)2 is used to absorb SO2. The acidity of H2SO3 is greater than that of H2CO3; therefore, SO2 reacts with NaHCO3 and Na2CO3. The acidity of H2SO3 is also greater than that of H2S, so SO2 reacts with Na2S. ② Oxidizing property: SO2 + 2H2S = 3S + 2H2O. ③ Reducing property: It can be oxidized by strong oxidizing agents such as Cl2, Br2, I2, Fe3+, KMnO4, and HNO3 to form sulfur in higher oxidation states. SO2+X2+2H2O=H2SO4+2HX
It is usually a colorless, toxic gas with an irritating odor; it has a density greater than that of air, is easily liquefied, and is soluble in water. It is an acidic oxide and possesses the general properties of acidic oxides; it undergoes a hydration reaction to form sulfurous acid, which is then oxidized to sulfuric acid.
When sulfur dioxide dissolves in water, it forms sulfurous acid (the main component of acid rain); if sulfur dioxide is further oxidized, sulfuric acid is produced rapidly and efficiently, usually in the presence of a catalyst. Sulfur dioxide is a colorless and transparent gas with an irritating odor. Soluble in water, ethanol, and ether. At room temperature, moist sulfur dioxide reacts with hydrogen sulfide to precipitate sulfur. Under high temperature and in the presence of a catalyst, it can be reduced to hydrogen sulfide by hydrogen, and to sulfur by carbon monoxide. Strong oxidizing agents can oxidize sulfur dioxide to sulfur trioxide; only in the presence of a catalyst can oxygen oxidize sulfur dioxide to sulfur trioxide.
⑴Physical properties: Typically, SO2 is a colorless, toxic gas with an irritating odor; it has a density greater than that of air, is easy to liquefy, and is soluble in water. ⑵Chemical properties: ① SO2 is an acidic oxide and possesses the general properties of acidic oxides. == ； SO2+CaO=CaSO3 ； SO2+2NaOH=Na2SO3+H2O ； SO2 + NaOH = NaHSO3 (similar to the reaction of CO2 with a base). NH3·H2O or Ca(OH)2 is used to absorb SO2. The acidity of H2SO3 is greater than that of H2CO3; therefore, SO2 reacts with NaHCO3 and Na2CO3. The acidity of H2SO3 is also greater than that of H2S, so SO2 reacts with Na2S. ② Oxidizing property: SO2 + 2H2S = 3S + 2H2O. ③ Reducing property: It can be oxidized by strong oxidizing agents such as Cl2, Br2, I2, Fe3+, KMnO4, and HNO3 to form sulfur in higher oxidation states. SO2+X2+2H2O=H2SO4+2HX
1. Physical properties: Typically, SO2 is a colorless, toxic gas with an irritating odor; it has a density greater than that of air, is easy to liquefy, and soluble in water. 2. Chemical properties: SO2- is an acidic oxide and possesses the general properties of acidic oxides ； Oxidizing property ； Reducing power and bleaching ability
A colorless gas with a sulfurous and acidic odor; its specific gravity is 2.27. It is soluble in water and has a strong irritating effect on the eyes and respiratory organs.
⑴Physical properties: Typically, SO2 is a colorless, toxic gas with an irritating odor; it has a density greater than that of air, is easy to liquefy, and is soluble in water. ⑵Chemical properties: ① SO2- is an acidic oxide and possesses the general properties of acidic oxides. == ； SO2+CaO=CaSO3 ； SO2+2NaOH=Na2SO3+H2O ； SO2 + NaOH = NaHSO3 (similar to the reaction of CO2 with a base). NH3·H2O or Ca(OH)2 is used to absorb SO2. The acidity of H2SO3 is greater than that of H2CO3; therefore, SO2 reacts with NaHCO3 and Na2CO3. The acidity of H2SO3 is also greater than that of H2S, so SO2 reacts with Na2S. ② Oxidizing property: SO2 + 2H2S = 3S + 2H2O. ③ Reducing property: It can be oxidized by strong oxidizing agents such as Cl2, Br2, I2, Fe3+, KMnO4, and HNO3 to form sulfur in higher oxidation states. SO2+X2+2H2O=H2SO4+2HX
Physical properties: Density and state – 2.551 g/L, gas (under standard conditions). Solubility – 9.4 g/mL (at 25 degrees Celsius). Color and appearance – colorless at room temperature. Melting point – -72.4 degrees Celsius (200.75 K). Boiling point – -10 degrees Celsius (263 K).
Chemical properties: Sulfur dioxide can be produced when sulfur burns: S(s) + O2(g) → SO2(g). Hydrogen sulfide can also burn to produce sulfur dioxide: 2H2S(g) + 3O2(g) → 2H2O(g) + 2SO2(g). Heating pyrite, sphalerite, and mercury sulfide can yield sulfur dioxide as well: 4FeS2(s) + 11O2(g) → 2Fe2O3(s) + 8SO2(g); 2ZnS(s) + 3O2(g) → 2ZnO(s) + 2SO2(g).
Applications: Sulfur dioxide is particularly useful as a preservative for alcohol and dried fruits; it helps to prevent microbial growth and improves the taste of fruits. It is also an effective reducing agent – in the presence of water, it can cause items to fade in color, making it useful as a bleaching agent. It is commonly used to bleach paper and other materials that are soft like cloth
Chemical properties: Sulfur dioxide can be produced when sulfur burns: S(s) + O2(g) → SO2(g). Hydrogen sulfide can also burn to produce sulfur dioxide: 2H2S(g) + 3O2(g) → 2H2O(g) + 2SO2(g). Heating pyrite, sphalerite, and mercury sulfide can yield sulfur dioxide as well: 4FeS2(s) + 11O2(g) → 2Fe2O3(s) + 8SO2(g); 2ZnS(s) + 3O2(g) → 2ZnO(s) + 2SO2(g).
Applications: Sulfur dioxide is particularly useful as a preservative for alcohol and dried fruits; it helps to prevent microbial growth and improves the taste of fruits. It is also an effective reducing agent – in the presence of water, it can cause items to fade in color, making it useful as a bleaching agent. It is commonly used to bleach paper and other materials that are soft like cloth
【Physical properties of SO2】 Also known as sulfurous anhydride, it is a colorless, flammable-free, toxic gas with a strong pungent odor. Molecular weight 64.07, density 2.3 g/L, melting point -72.7°C, boiling point -10°C. Soluble in water, methanol, ethanol, sulfuric acid, acetic acid, chloroform, and ether. It mixes easily with water to form sulfurous acid (H2SO3), which is then converted into sulfuric acid. At room temperature and pressures of 392.266–490.3325 kPa (4–5 kg/cm2), it is a colorless flowing liquid. 【Chemical properties of SO2】 1. Reaction with water: Sulfur dioxide reacts chemically with water to produce acidic substances. Sulfur dioxide is an acidic oxide. SO2 + H2O = H2SO3 2. Weak oxidizing property: 2H2S + SO2 = 3S + 2H2O 3. Reducing property: 2SO2 + O2 = 2SO3; 5SO2 + 2H2O + 2KMnO4 = 2MnSO4 + 2K2SO4; 2SO2 + Cl2 = H2SO4 + 2HCl 4. Bleaching property: Sulfur dioxide can cause red phenol red solution to fade, and the solution turns red again when heated.