4.8g of Mg were burn in 3.2g of oxygen. The MgO produced at a mass of 8g what is the equation of the reaction
Mg + heat + O > MgO
Oxygen does not exist as O
2Mg+O2 >> 2MgO
That is the reaction. there may be some reactants left over
when 4.8g of magnesium reacts with 3.2g of oxygen how much magnesium oxide
formed
When 4.8g of magnesium reacts with 3.2g of oxygen, how much magnesium oxide is formed?
To determine the equation of the reaction, we first need to understand the concept of stoichiometry. Stoichiometry is based on the law of conservation of mass, which states that in a chemical reaction, matter cannot be created or destroyed, only rearranged.
In this case, we know that 4.8g of magnesium (Mg) reacted with 3.2g of oxygen (O₂) to produce 8g of magnesium oxide (MgO).
To write the balanced equation, follow these steps:
Step 1: Convert the masses of reactants and products to moles. To do this, divide each mass by the molar mass of the respective substance.
The molar mass of Mg is 24.31 g/mol, the molar mass of O₂ is 32.00 g/mol, and the molar mass of MgO is 40.31 g/mol.
Moles of Mg: 4.8g / 24.31 g/mol ≈ 0.1977 mol
Moles of O₂: 3.2g / 32.00 g/mol ≈ 0.1000 mol
Moles of MgO: 8g / 40.31 g/mol ≈ 0.1985 mol
Step 2: Use the moles of reactants and products to determine the stoichiometric ratio.
From the moles obtained, we can see that the ratio of moles of Mg to moles of MgO is approximately 0.1977 mol: 0.1985 mol.
To simplify this ratio, we can divide all values by 0.1977 to get a whole-number ratio:
0.1977 mol / 0.1977 ≈ 1 mol
0.1985 mol / 0.1977 ≈ 1 mol
Therefore, the simplified ratio is 1:1, indicating that one mole of magnesium reacts with one mole of magnesium oxide.
Step 3: Write the balanced chemical equation using the stoichiometric ratio.
Based on the simplified ratio, we can write the balanced equation as follows:
Mg + O₂ → MgO
This equation represents the reaction between magnesium and oxygen to produce magnesium oxide.