How Many Formula Units Are In 5.50 Grams Of AgNO3
When it comes to understanding the concept of formula units, it is essential to delve into the world of chemistry. In the realm of chemistry, formula units provide valuable information about the number of atoms or ions present in a given compound. In this article, we will explore the calculation of the number of formula units in 5.50 grams of AgNO3, a compound commonly known as silver nitrate.
To comprehend this calculation, it is crucial to have a basic understanding of the concept of a formula unit. A formula unit represents the smallest whole-number ratio of atoms or ions in a compound. Unlike molecules, which are composed of two or more nonmetals, compounds like AgNO3 consist of a metal (Ag) and one or more nonmetals (N and O).
Silver nitrate (AgNO3) is a chemical compound frequently used in the laboratory, particularly in chemistry experiments. To calculate the number of formula units in 5.50 grams of AgNO3, we need to determine the molar mass of AgNO3, which represents the mass of one mole of the compound.
Calculating the Molar Mass of AgNO3
The molar mass of a compound is the sum of the atomic masses of all the atoms present in a formula unit. To find the molar mass of AgNO3, we multiply the number of atoms of each element by its atomic mass and sum them up.
Ag (Silver):
– Atomic Number: 47
– Atomic Mass: 107.87 g/mol
N (Nitrogen):
– Atomic Number: 7
– Atomic Mass: 14.01 g/mol
O (Oxygen):
– Atomic Number: 8
– Atomic Mass: 16.00 g/mol
Therefore, the molar mass of AgNO3 is calculated as follows:
(1 × Ag) + (1 × N) + (3 × O) = (1 × 107.87 g/mol) + (1 × 14.01 g/mol) + (3 × 16.00 g/mol) = 169.87 g/mol
Thus, the molar mass of AgNO3 is 169.87 grams per mole.
Calculating the Number of Moles
Before determining the number of formula units in 5.50 grams of AgNO3, we need to establish the number of moles present in this mass. One mole of any substance contains 6.02 × 10^23 formula units. By calculating the number of moles, we can convert the given mass into a countable unit for further calculations.
To calculate the number of moles in 5.50 grams of AgNO3, we divide the given mass by the molar mass:
Number of moles = Mass (g) / Molar Mass (g/mol)
Number of moles = 5.50 g / 169.87 g/mol
Number of moles = 0.0324 mol (rounded to four decimal places)
Thus, 5.50 grams of AgNO3 contains approximately 0.0324 moles.
Calculating the Number of Formula Units
Now that we have established the number of moles present in 5.50 grams of AgNO3, we can proceed to determine the number of formula units. As mentioned earlier, one mole of any substance contains 6.02 × 10^23 formula units.
To calculate the number of formula units, we multiply the number of moles by Avogadro’s number:
Number of formula units = Number of moles × Avogadro’s Number
Number of formula units = 0.0324 mol × 6.02 × 10^23 formula units/mol
Number of formula units = 1.95 × 10^22 formula units (rounded to two significant figures)
Consequently, in 5.50 grams of AgNO3, there are approximately 1.95 × 10^22 formula units.
In conclusion, to calculate the number of formula units in a given mass of AgNO3, we follow a systematic approach. First, we determine the molar mass of the compound by adding the atomic masses of each element. Then, by dividing the given mass by the molar mass, we find the number of moles. Finally, by multiplying the number of moles by Avogadro’s number, we calculate the number of formula units. Applying this method to 5.50 grams of AgNO3, we find that it contains approximately 1.95 × 10^22 formula units. Understanding these calculations allows us to comprehend the composition and characteristics of chemical compounds in a more precise manner.