Calculate the mass in grams of 1.1 mol of magnesium fluoride.
The following molar masses can be used: Magnesium: 24.21 g/mol;
Fluorine: 19.00 g/mol
The Correct Answer and Explanation is :
The correct answer is: 68.43 grams.
To calculate the mass of 1.1 moles of magnesium fluoride (MgF₂), we first need to determine its molar mass. Magnesium fluoride consists of one magnesium atom and two fluorine atoms.
Step 1: Calculate the Molar Mass of MgF₂
- Molar Mass of Magnesium (Mg):
- ( \text{Molar mass of Mg} = 24.21 \, \text{g/mol} )
- Molar Mass of Fluorine (F):
- Since there are two fluorine atoms in magnesium fluoride, we calculate:
[
\text{Molar mass of F} = 2 \times 19.00 \, \text{g/mol} = 38.00 \, \text{g/mol}
]
- Total Molar Mass of MgF₂:
- Combine the molar masses of magnesium and fluorine:
[
\text{Molar mass of MgF₂} = \text{Molar mass of Mg} + \text{Molar mass of F} = 24.21 \, \text{g/mol} + 38.00 \, \text{g/mol} = 62.21 \, \text{g/mol}
]
Step 2: Calculate the Mass of 1.1 moles of MgF₂
To find the mass, use the formula:
[
\text{Mass} = \text{Moles} \times \text{Molar Mass}
]
Plugging in the values:
[
\text{Mass} = 1.1 \, \text{mol} \times 62.21 \, \text{g/mol} = 68.431 \, \text{g}
]
Conclusion
The mass of 1.1 moles of magnesium fluoride is approximately 68.43 grams.
Explanation
Understanding how to calculate the mass of a compound from its moles is fundamental in chemistry, especially in stoichiometry. The concept of the mole is central to chemical calculations, allowing chemists to relate quantities of reactants and products in chemical reactions. The molar mass acts as a bridge between the atomic or molecular scale and the macroscopic scale we observe in the laboratory. By determining the molar mass, we can efficiently convert moles into grams, which is crucial for preparing solutions, conducting reactions, or analyzing substances. This knowledge is also applicable in various fields, including pharmaceuticals, environmental science, and materials science, where precise measurements of compounds are vital.