How Many Moles Of Aluminium Sulphate Will Contain 0.24 Mole Of Oxygen Atom

Have you ever wondered how many moles of aluminium sulphate would be needed to contain 0.24 moles of oxygen atoms? Well, in this video, we will break down the process for you in a simple and easy-to-understand way.

First of all, let’s understand the chemical formula for aluminium sulphate, which is Al2(SO4)3. This means that one molecule of aluminium sulphate contains 2 atoms of aluminium (Al), 3 atoms of sulphur (S), and 12 atoms of oxygen (O).

Now, if we want to find out how many moles of aluminium sulphate are needed to contain 0.24 moles of oxygen atoms, we first need to calculate the molar mass of aluminium sulphate.

The molar mass of aluminium sulphate can be calculated by adding up the atomic masses of each element in the formula. The atomic mass of aluminium is 26.98 g/mol, the atomic mass of sulphur is 32.06 g/mol, and the atomic mass of oxygen is 16.00 g/mol.

So, the molar mass of aluminium sulphate is:
2(26.98) + 3(32.06) + 12(16.00) = 246.16 g/mol

Next, we need to calculate the number of moles of oxygen atoms in one mole of aluminium sulphate. Since there are 12 oxygen atoms in one mole of aluminium sulphate, the number of moles of oxygen atoms is:
(12)(0.24) = 2.88 moles

Now, to find out how many moles of aluminium sulphate are needed to contain 0.24 moles of oxygen atoms, we simply divide the number of moles of oxygen atoms by the number of moles of oxygen atoms in one mole of aluminium sulphate:
0.24 / 2.88 = 0.0833 moles

Therefore, 0.0833 moles of aluminium sulphate would be needed to contain 0.24 moles of oxygen atoms.

In conclusion, understanding the molar mass of a compound and the number of atoms of each element in the compound is essential in determining the number of moles of a substance needed to contain a certain number of atoms. This simple calculation can be applied to various chemical reactions and experiments, helping scientists and researchers in their work.

So, the next time you come across a similar question or problem, remember to calculate the molar mass and number of moles of each element to find the solution. Chemistry may seem complex, but with a little practice and understanding, you can easily master it.

Thank you for watching this video and we hope you found this explanation helpful. Stay curious and keep learning!

Aluminium sulphate is a chemical compound with the formula Al2(SO4)3. It is commonly used in water treatment plants to clarify water by removing impurities. In this article, we will delve into the calculation of how many moles of aluminium sulphate will contain 0.24 moles of oxygen atoms. This calculation involves stoichiometry, which is the relationship between the amounts of reactants and products in a chemical reaction.

What is Aluminium Sulphate?

Aluminium sulphate, also known as alum, is a white crystalline solid that is soluble in water. It is commonly used in the purification of drinking water and wastewater treatment. Aluminium sulphate is a coagulant that binds with impurities in the water, allowing them to settle out. This process is known as flocculation.

What is Stoichiometry?

Stoichiometry is the calculation of quantities of reactants and products in a chemical reaction. It is based on the principle of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. Stoichiometry allows chemists to predict how much product will be formed from a given amount of reactant, or vice versa.

How Many Moles of Aluminium Sulphate Will Contain 0.24 Moles of Oxygen Atoms?

To calculate how many moles of aluminium sulphate will contain 0.24 moles of oxygen atoms, we need to consider the balanced chemical equation for the reaction. The formula for aluminium sulphate is Al2(SO4)3, which means that each molecule contains two aluminium atoms, three sulphur atoms, and twelve oxygen atoms.

Step-by-Step Explanation:

1. Start by writing down the balanced chemical equation for the reaction involving aluminium sulphate and oxygen. The reaction can be written as:

   2Al2(SO4)3 + 3O2 → 2Al2O3 + 3SO3

2. From the equation, we can see that 3 moles of oxygen react with 2 moles of aluminium sulphate to produce 2 moles of aluminium oxide and 3 moles of sulphur trioxide.
3. Calculate the molar mass of aluminium sulphate (Al2(SO4)3) by adding the atomic masses of aluminium, sulfur, and oxygen. The atomic masses are: Al = 27 g/mol, S = 32 g/mol, O = 16 g/mol.
4. The molar mass of aluminium sulphate is:
   2(27) + 3(32) + 12(16) = 2(27) + 96 + 192 = 54 + 96 + 192 = 342 g/mol

5. Calculate the number of moles of oxygen atoms in 0.24 moles of oxygen. Since each oxygen molecule (O2) contains 2 oxygen atoms, the number of moles of oxygen atoms is half of the number of moles of oxygen molecules.
6. The number of moles of oxygen atoms is:
   0.24 moles / 2 = 0.12 moles

7. Use the stoichiometry of the balanced chemical equation to determine the number of moles of aluminium sulphate needed to react with 0.12 moles of oxygen atoms.
8. From the balanced chemical equation, we know that 3 moles of oxygen react with 2 moles of aluminium sulphate. Therefore, the ratio of moles of oxygen to moles of aluminium sulphate is 3:2.
9. Set up a proportion to find the number of moles of aluminium sulphate:
   0.12 moles O / 3 moles O = x moles Al2(SO4)3 / 2 moles Al2(SO4)3

10. Solve for x:
    x = (0.12 moles O * 2 moles Al2(SO4)3) / 3 moles O
    x = 0.08 moles Al2(SO4)3

    Therefore, 0.08 moles of aluminium sulphate will contain 0.24 moles of oxygen atoms.

    Conclusion
    

    In conclusion, the calculation of how many moles of aluminium sulphate will contain 0.24 moles of oxygen atoms involves stoichiometry and the balanced chemical equation for the reaction. By following the step-by-step explanation provided in this article, you can easily determine the amount of aluminium sulphate needed to react with a given number of oxygen atoms. Aluminium sulphate plays a crucial role in water treatment processes, and understanding its chemistry is essential for efficient purification of water sources.

    Sources:

    • Chemistry LibreTexts
    • Royal Society of Chemistry

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