Question

The molar mass of barium nitrate ( $ Ba{(N{O_3})_2} $ ) is $ 261.35g.mo{l^{ - 1}} $ . What is the mass of $ 5.30 \times {10^{22}} $ formula units of $ Ba{(N{O_3})_2} $ ?

Answer 1

Hint : In order to this question, first we will rewrite the given facts of the question, and then we will find the molar mass, as the molar mass of a chemical compound is defined as the mass of a sample of that compound divided by the amount of substance in that sample, measured in moles.

Complete Step By Step Answer:
It is a fact that $ 6.023 \times {10^{23}} $ formula units of barium nitrate have a mass of $ 261.35g $ .
When we talk about molar mass, we mean this.
The quotient multiplied by the molar mass equals the mass of $ 5.30 \times {10^{22}} $ formula units of barium nitrate:
 $ \dfrac{{5.30 \times {{10}^{22}}}}{{6.023 \times {{10}^{23}}}} \times 261.35g.mo{l^{ - 1}} = 22.99g.mo{l^{ - 1}} $
Hence, the required molar mass of $ 5.30 \times {10^{22}} $ .

Additional Information:
The mass of a sample of a chemical compound divided by the amount of material in that sample, measured in moles, is the molar mass of that compound in chemistry. In gram, it is the mass of 1 mole of the substance, or $ 6.023 \times {10^{23}} $ particles. The molar mass of a substance is a bulk attribute, not a molecular property. The molar mass is a weighted average of many different instances of the compound, which can vary in mass due to isotopes. The molar mass is most usually calculated from standard atomic weights, and is thus a terrestrial average and a function of the relative abundance of the constituent atoms on Earth.
For bulk quantities, the molar mass is ideal for converting between the mass of a substance and the amount of a substance.

Note :
This constant is used to determine the number of atoms contained in one mole of any substance, and the mass of one mole of a substance is known as its molar mass. Understand the concept of molar mass. The mass (in grammes) of one mole of a substance is referred to as molar mass.