Carbon tetrachloride is a hydrocarbon chemical compound composed of one carbon (C) atom joined to four chlorine (Cl) atoms. It is a colorless, non-flammable liquid and a sweet odor.
Lewis Structure
The Lewis structure of carbon tetrachloride (CCl₄) can be drawn as follows:
C-Cl
|
Cl
|
Cl
|
Cl
The Lewis structure illustrates how the electrons are shared in the molecule, with each line representing a single covalent bond.
Properties
The properties of carbon tetrachloride.
| Density | 1.5867 g/cm³ at 20 °C. |
| Melting point | -22.93 °C |
| Boiling point | 76.72 °C |
| Vapor pressure | 91.4 mmHg at 20 °C |
| Solubility in water | 0.81 g/100 mL |
| Solubility in organic solvents | miscible with most organic solvents |
| Flash point | None |
| Autoignition temperature | None |
| Explosive limits | Not explosive |
Molar Mass
To calculated molar mass of carbon tetrachloride (CCl₄) to adding up the molar masses of it is constituent elements.
Molar Mass of Carbon is 12.01 g/mol.
Molar Mass of Chlorine is 35.45 g/mol.
Molar Mass of CCl₄ = (1 × Molar Mass of Carbon) + (4 × Molar Mass of Chlorine)
= (1 × 12.01) + (4 × 35.45)
≈ 12.01 + 141.80
≈ 153.81 g/mol
The molar mass of carbon tetrachloride (CCl₄) is 153.81 g/mol.
Uses of Carbon Tetrachloride
1. It is a good solvent for soluble many organic substances, such as greases, oils, and tars.
2. It is used in a variety of industries, including metalworking, dry cleaning, and rubber manufacturing etc.
3. It is used as a dry cleaning agent, but it has been largely replaced by less toxic solvents due to it is environmental and health hazards.
4. It is used as a fire extinguisher because it smothers the fire by displacing oxygen.
5. Carbon tetrachloride was once used as a fumigant to control pests in grain and other agricultural products. But it is been banned in many countries due to its environmental and health hazards.
6. It is used as a chemical intermediate in the production of other chemicals, such as chlorofluorocarbons (CFCs). But CFCs have been banned due to their role in ozone depletion.
Intramolecular and Intermolecular Forces Differences
The Mass Percentage of Benzene and Carbon Tetrachloride
To calculate the mass percentage of benzene (C₆H₆) and carbon tetrachloride (CCl₄) in a mixture, you will need to know the masses of each component in the mixture and then use the following formula:
Mass Percentage = (Mass of Component / Total Mass of Mixture) x 100%
Have a mixture containing 40 grams of benzene (C₆H₆) and 60 grams of carbon tetrachloride (CCl₄).
1. Calculate the mass percentage of benzene:
Mass Percentage of Benzene = (40 g / (40 g + 60 g)) x 100%
= (40 g / 100 g) x 100%
= 40%
2. Calculate the mass percentage of carbon tetrachloride:
Mass Percentage of CCl₄ = (60 g / (40 g + 60 g)) x 100%
= (60 g / 100 g) x 100%
= 60%
This mixture, benzene makes up 40% of the total mass, while carbon tetrachloride makes up 60% of the total mass.
The Mole Fraction of Benzene in Solution Containing 30% by Mass in Carbon Tetrachloride
To calculate the mole fraction of benzene (C₆H₆) in a solution containing 30% by mass in carbon tetrachloride (CCl₄), use the following formula:
Mole Fraction = (Number of Moles of Component / Total Number of Moles in Solution)
1. Calculate the number of moles of benzene (C₆H₆):
First find the molar mass of benzene. The molar mass of benzene is the sum of the atomic masses of its constituent atoms:
Molar Mass of C₆H₆ = (6 × Atomic Mass of Carbon) + (6 × Atomic Mass of Hydrogen)
= (6 × 12.01 g/mol) + (6 × 1.01 g/mol) ≈ 78.07 g/mol
Now, calculate the moles of benzene in a 100 g solution (since it is 30% by mass):
Number of Moles of Benzene = (30 g / 78.07 g/mol)
2. Calculate the number of moles of carbon tetrachloride (CCl₄):
To find the moles of CCl₄ in a 100 g solution (since it's 30% by mass), it is molar mass:
Molar Mass of CCl₄ = (1 × Atomic Mass of Carbon) + (4 × Atomic Mass of Chlorine)
= (1 × 12.01 g/mol) + (4 × 35.45 g/mol) ≈ 153.81 g/mol
= (70 g / 153.81 g/mol)
3. Calculate the total number of moles in the solution:
Total Number of Moles in Solution = Number of Moles of Benzene + Number of Moles of CCl₄
= (30 g / 78.07 g/mol) + (70 g / 153.81 g/mol)
= 0.385 + 0.445
= 0.83
4. Calculate the mole fraction of benzene:
Mole Fraction of Benzene = (Number of Moles of Benzene / Total Number of Moles in Solution)
= 0.385/0.83
= 0.452
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