How many moles are contained in 23.5 g of sb2s3

Determining Moles

To find the number of moles in 23.5 g of Sb2S3, we need to use the molar mass of Sb2S3 and the formula:

Calculating Molar Mass

First, calculate the molar mass of Sb2S3:

• Antimony (Sb): Atomic mass = 121.76 g/mol
• Sulfur (S): Atomic mass = 32.06 g/mol

Sb2S3 contains 2 atoms of Sb and 3 atoms of S. Therefore:

Calculating Moles

Now, using the mass of Sb2S3 (23.5 g):

Therefore, 23.5 g of Sb2S3 contain approximately 0.0691 moles.

Understanding Molar Mass Calculation

Molar mass is a fundamental concept in chemistry representing the mass of one mole of a given substance. It allows you to convert between the mass of a material and the number of moles, facilitating a variety of calculations in chemical reactions.

The Concept of Molar Mass

The molar mass of a substance is represented in units of grams per mole (g/mol). To determine the molar mass, you need to sum the atomic masses of all the elements in the molecule, as given on the periodic table.

Calculation Steps

1. Identify the molecular formula of the compound.
2. List the atomic masses of each element (usually found on the periodic table).
3. Multiply each atomic mass by the number of atoms of that element in the molecule.
4. Sum these values to get the total molar mass.

Example: Calculation for Water (H₂O)

1. Molecular formula: $H_2O$
2. Atomic masses:
   • Hydrogen (H): approximately 1 g/mol
   • Oxygen (O): approximately 16 g/mol
3. Multiply:
   • For Hydrogen: $2 \times 1 \, \text{g/mol} = 2 \, \text{g/mol}$
   • For Oxygen: $1 \times 16 \, \text{g/mol} = 16 \, \text{g/mol}$
4. Sum: $$M_{\text{H}_2\text{O}} = 2 \, \text{g/mol (H)} + 16 \, \text{g/mol (O)} = 18 \, \text{g/mol}$$

Multiline LaTeX Formula Example

For a compound like ethane ($C_2H_6$):

Summary

Molar mass calculation is a critical process for quantifying the amount of substances involved in chemical reactions. By following the steps outlined and summing up the atomic masses, you can accurately find the molar mass of any compound.

Understanding the Mole Formula in Chemistry

The mole formula is fundamental in chemistry, as it links the microscopic world of atoms and molecules to the macroscopic world we interact with daily.

The Concept of a Mole

A mole is a unit that measures the amount of substance. One mole contains exactly $6.022 \times 10^{23}$ entities, known as Avogadro's number. This can be atoms, molecules, ions, or other particles.

Mol calculation

To relate the mass of a substance to the number of moles, you use the mole formula:

where:

• $n$ is the number of moles,
• $m$ is the mass of the substance (in grams),
• $M$ is the molar mass of the substance (in g/mol).

Molar Mass

The molar mass is the mass of one mole of a given substance. For elements, it corresponds to the atomic mass found on the periodic table, expressed in grams per mole (g/mol). For example, the molar mass of carbon is $12.01 \ \text{g/mol}$.

Example Calculations

Let's apply the formula with an example. Suppose you have 24 grams of carbon and you want to find out how many moles it represents.

1. Find the molar mass of carbon:

   $M_{\text{carbon}} = 12.01 \ \text{g/mol}$

2. Apply the mole formula:

   $$n = \frac{m}{M} = \frac{24 \ \text{g}}{12.01 \ \text{g/mol}} = 2 \ \text{mol}$$

This shows that 24 grams of carbon is equivalent to 2 moles of carbon atoms.

Importance in Chemical Equations

The mole formula is essential for stoichiometric calculations in chemical reactions, allowing chemists to predict the amounts of reactants needed and products formed. By using the mole ratio derived from balanced chemical equations, one can accurately determine these quantities.

Understanding and applying the mole concept enables chemists to bridge the gap between the atomic scale and observable chemical processes, making it a cornerstone of quantitative chemistry.