Sulfuryl chloride (SO2Cl2) is a compound formed by the combination of sulfur dioxide and chlorine. It is used as a reagent in chemical reactions and as a fumigant for pest control.
| IUPAC Name | Sulfuryl chloride |
| Molecular Formula | SO2Cl2 |
| CAS Number | 7791-25-5 |
| Synonyms | Sulfuric dichloride, Sulfur oxychloride, Sulfur dichloride oxide |
| InChI | InChI=1S/Cl2O2S/c1-5(2)6(3)4 |
Sulfuryl Chloride Properties
Sulfuryl Chloride Formula
The chemical formula of sulfuric dichloride is SO2Cl2. It is derived from the combination of one sulfur atom, two oxygen atoms, and two chlorine atoms. This formula represents the composition and arrangement of atoms in a molecule of sulfuric dichloride.
Sulfuryl Chloride Molar Mass
The molar mass of sulfuric dichloride can be calculated by adding up the atomic masses of its constituent elements. Sulfuric dichloride has a molar mass of approximately 134.97 grams per mole. This value is important for various calculations in chemical reactions and stoichiometry.
Sulfuryl Chloride Boiling Point
Sulfuric dichloride has a boiling point of around 69 degrees Celsius. When the temperature rises above this point, sulfuric dichloride undergoes a phase change from a liquid to a gas. The boiling point is a crucial parameter in determining the conditions under which sulfuric dichloride can be used or handled.
Sulfuryl Chloride Melting Point
The melting point of sulfuric dichloride is approximately -54 degrees Celsius. At temperatures below this point, sulfuric dichloride transitions from a solid to a liquid state. The melting point is significant for storing and handling sulfuric dichloride as it indicates the conditions under which it solidifies or liquefies.
Sulfuryl Chloride Density g/mL
The density of sulfuric dichloride is about 1.638 grams per milliliter (g/mL). Density represents the mass of a substance per unit volume and helps determine its physical behavior. The density of sulfuric dichloride is important for understanding its buoyancy, solubility, and compatibility with other substances.
Sulfuryl Chloride Molecular Weight
The molecular weight of sulfuric dichloride is approximately 134.97 atomic mass units (u). It is the sum of the atomic masses of the constituent atoms in a sulfuric dichloride molecule. The molecular weight provides crucial information for various chemical calculations and determining the amount of substance in a given sample.
Sulfuryl Chloride Structure
Sulfuric dichloride features a molecular structure where one sulfur atom is double-bonded to two oxygen atoms and single-bonded to two chlorine atoms. This arrangement forms a central sulfur atom surrounded by oxygen and chlorine atoms, giving sulfuric dichloride its characteristic structure.
Sulfuryl Chloride Solubility
Sulfuric dichloride is sparingly soluble in water. It reacts with water to produce hydrochloric acid and sulfuric acid, making it hydrolytically reactive. However, sulfuric dichloride exhibits some solubility in organic solvents such as chlorinated hydrocarbons and aromatic compounds, which makes them suitable for certain applications.
| Appearance | Colorless liquid |
| Specific Gravity | 1.638 g/mL |
| Color | N/A |
| Odor | Pungent, suffocating |
| Molar Mass | 134.97 g/mol |
| Density | 1.638 g/mL |
| Melting Point | -54 °C |
| Boiling Point | 69 °C |
| Flash Point | N/A |
| Water Solubility | Reacts vigorously |
| Solubility | Soluble in organic solvents such as chlorinated hydrocarbons and aromatic compounds |
| Vapor Pressure | 43.6 mmHg (at 25 °C) |
| Vapor Density | 4.43 (air = 1) |
| pKa | N/A |
| pH | N/A |
Sulfuryl Chloride Safety and Hazards
Sulfuric dichloride poses several safety hazards and precautions should be taken when handling it. It is a corrosive substance that can cause severe burns to the skin, eyes, and respiratory tract upon contact. Direct inhalation of its vapors can lead to respiratory irritation and lung damage. It reacts violently with water, releasing toxic gases and posing a risk of explosion. Therefore, it is important to handle sulfuric dichloride in a well-ventilated area and wear appropriate protective equipment, such as gloves, goggles, and respiratory protection. Spills should be immediately cleaned up using proper procedures, and storage should be in a cool, dry place away from incompatible materials.
| Hazard Symbols | Corrosive (C), Oxidizing (O) |
| Safety Description | Causes severe skin burns and eye damage. Reacts violently with water. |
| UN IDs | UN 1834 (Sulfuric dichloride) |
| HS Code | 28121000 |
| Hazard Class | 8 (Corrosive substances) |
| Packing Group | II (Medium danger) |
| Toxicity | Highly toxic; harmful if swallowed, inhaled, or absorbed through skin. |
Sulfuryl Chloride Synthesis Methods
People commonly use a few methods to synthesize sulfuric dichloride.
One method involves the reaction between sulfur dioxide (SO2) and chlorine gas (Cl2). In the presence of a catalyst, such as activated carbon or aluminum chloride, the gases react to form sulfuric dichloride (SO2Cl2). This reaction typically occurs at elevated temperatures, around 100-200°C.
Another method for sulfuric dichloride synthesis involves the reaction of sulfur trioxide (SO3) with hydrogen chloride (HCl). Under controlled conditions, these two compounds combine to produce sulfuric dichloride. This reaction is exothermic and typically occurs in the gas phase.
The Thionyl chloride process generates sulfuric dichloride by the room temperature reaction of sulfuric acid (H2SO4) with phosphorus pentachloride (PCl5). This reaction generates sulfuric dichloride as well as byproducts such as phosphoric acid (H3PO4) and hydrogen chloride (HCl). Industrial settings commonly employ this method.
It is important to note that these synthesis methods require careful handling of the reactants and consideration of safety precautions due to the reactivity and hazardous nature of the involved substances.
Furthermore, chemists often utilize suitable equipment, such as condensers and reflux systems, to exert control over the reaction conditions and guarantee a successful synthesis of sulfuric dichloride.
Sulfuryl Chloride Uses
Sulfuric dichloride (SO2Cl2) finds various applications across different industries due to its unique properties. Here are some key uses of sulfuric dichloride:
- Chemical Reagent: Organic synthesis commonly employs sulfuric dichloride as a versatile chemical reagent, where it actively participates in various reactions, including chlorination, sulfonation, and esterification, enabling the introduction of chlorine, sulfur, or acid functionalities into organic compounds.
- Pesticide and Fumigant: Sulfuric dichloride acts as a potent fumigant for pest control in stored grains, flour mills, and food processing facilities, actively eliminating insects, larvae, and pests that can cause damage to stored agricultural products due to its strong biocidal properties.
- Polymerization: In the polymerization of specific monomers, such as vinyl chloride, sulfuric dichloride serves as an active catalyst or initiator, facilitating the production of polyvinyl chloride (PVC), a widely used thermoplastic polymer with applications in construction, automotive, and electrical industries.
- Pharmaceuticals: Sulfuric dichloride actively plays a crucial role in synthesizing pharmaceutical compounds, particularly sulfonamides, which are vital antibiotics and therapeutic agents utilized for treating diverse infections.
- Dye Manufacturing: Sulfuric dichloride actively participates in the production of dyes, particularly those containing sulfur or chlorine. It actively introduces desired functional groups and enhances the colorfastness and stability of dyes.
- Chemical Intermediates: Sulfuric dichloride serves as an active intermediate in the synthesis of other chemicals, including sulfur dioxide, sulfuric acid, and sulfonyl chlorides, which find applications in numerous industries such as detergent production, plastics manufacturing, and pharmaceuticals.
- Water Treatment: For water purification and disinfection, sulfuric dichloride actively neutralizes and eliminates harmful bacteria, viruses, and other microorganisms present in water sources.
- Laboratory Applications: Various laboratory procedures actively employ sulfuric dichloride, such as for the detection and determination of primary and secondary amines. It actively reacts with amines to form stable sulfonamides, aiding in their analysis and characterization.
Questions:
Q: What is the total number of gram-molecules of SO2Cl2 in 13.5 g of sulfuryl chloride?
A: The total number of gram-molecules of SO2Cl2 in 13.5 g of sulfuryl chloride can be calculated by dividing the given mass by the molar mass of SO2Cl2.
Q: Is SO2Cl2 polar or nonpolar?
A: SO2Cl2 is a polar molecule due to the presence of polar bonds and an asymmetrical molecular geometry.
Q: At what time will the pressure of SO2Cl2 decline?
A: The decline in the pressure of SO2Cl2 depends on various factors such as temperature, volume, and reaction conditions. It cannot be determined solely based on time.
Q: What is the partial pressure of SO2Cl2 in this mixture?
A: The partial pressure of SO2Cl2 in a mixture can be determined using the ideal gas law, given the temperature, volume, and the mole fraction or concentration of SO2Cl2.
Q: What type(s) of intermolecular forces are expected between SO2Cl2 molecules?
A: The intermolecular forces expected between SO2Cl2 molecules include dipole-dipole interactions and London dispersion forces.
Q: At what time will the partial pressure of SO2Cl2 decline to one-tenth its initial value?
A: The time required for the partial pressure of SO2Cl2 to decline to one-tenth of its initial value depends on the specific conditions of the system and the rate of the chemical reaction involved.
Q: What is the molar mass of SO2Cl2?
A: The molar mass of SO2Cl2 is approximately 134.97 grams per mole.
Q: What is the molecular geometry of SO2Cl2?
A: The molecular geometry of SO2Cl2 is bent or V-shaped, with a sulfur atom in the center bonded to two oxygen atoms and two chlorine atoms.
Q: What is the Lewis structure of SO2Cl2?
A: The Lewis structure of SO2Cl2 consists of a sulfur atom double-bonded to one oxygen atom and single-bonded to another oxygen atom, with two chlorine atoms bonded to the sulfur atom.