How many grams of magnesium nitride are formed from 45.1 moles of magnesium?
3Mg + N2 ==> Mg3N2
mols Mg = 45.1
mols Mg3N2 = 45.1 x (1 mol Mg3N2/3 mols mg) = 45.1 x (1/3) = ? mols.
g = mols x molar mass.
To determine the number of grams of magnesium nitride formed from 45.1 moles of magnesium, you'll need to use stoichiometry.
First, we need to write a balanced chemical equation for the reaction between magnesium and nitrogen to form magnesium nitride:
3Mg + N2 -> Mg3N2
From the balanced equation, we can see that 3 moles of magnesium react to form 1 mole of magnesium nitride.
So, we'll set up a conversion factor as follows:
1 mole Mg3N2 / 3 moles Mg
This conversion factor allows us to convert moles of magnesium to moles of magnesium nitride.
To find the number of moles of magnesium nitride, we'll use the following calculation:
moles of Mg3N2 = (45.1 moles Mg) * (1 mole Mg3N2 / 3 moles Mg)
moles of Mg3N2 = (45.1 / 3) moles Mg3N2
moles of Mg3N2 = 15.03 moles Mg3N2
Now, to convert moles of magnesium nitride to grams, we'll need to use its molar mass. The molar mass of magnesium nitride (Mg3N2) is the sum of the atomic masses of its constituent atoms:
Molar mass of Mg3N2 = (3 x atomic mass of Mg) + (2 x atomic mass of N)
Molar mass of Mg3N2 = (3 x 24.31 g/mol) + (2 x 14.01 g/mol)
Molar mass of Mg3N2 = 72.93 g/mol + 28.02 g/mol
Molar mass of Mg3N2 = 100.95 g/mol
To convert moles of magnesium nitride to grams, we'll use the following calculation:
grams of Mg3N2 = (moles of Mg3N2) * (molar mass of Mg3N2)
grams of Mg3N2 = (15.03 moles) * (100.95 g/mol)
grams of Mg3N2 = 1519.78 grams
Therefore, approximately 1519.78 grams of magnesium nitride are formed from 45.1 moles of magnesium.
To determine how many grams of magnesium nitride are formed from 45.1 moles of magnesium, you first need to understand the balanced chemical equation for the reaction between magnesium and nitrogen to form magnesium nitride.
The balanced chemical equation for this reaction is:
3Mg + N2 -> Mg3N2
From the balanced chemical equation, we can see that 3 moles of magnesium react with 1 mole of nitrogen to produce 1 mole of magnesium nitride.
In this case, we have 45.1 moles of magnesium, so we need to determine the moles of magnesium nitride formed using the mole ratio from the balanced chemical equation.
Using the mole ratio, we can calculate the moles of magnesium nitride formed:
45.1 moles Mg * (1 mole Mg3N2 / 3 moles Mg) = 15.03 moles Mg3N2
Now, to determine the mass of magnesium nitride formed, we need to use the molar mass of magnesium nitride, which can be calculated by summing the atomic masses of its constituent elements.
Molar mass of Mg3N2 = (3 x atomic mass of Mg) + (2 x atomic mass of N)
The atomic masses of magnesium (Mg) and nitrogen (N) are approximately 24.31 g/mol and 14.01 g/mol, respectively. Plugging these values into the equation:
Molar mass of Mg3N2 = (3 x 24.31 g/mol) + (2 x 14.01 g/mol) = 100.94 g/mol
Finally, to calculate the mass of magnesium nitride formed, we multiply the moles of magnesium nitride by its molar mass:
15.03 moles Mg3N2 * (100.94 g Mg3N2 / 1 mol Mg3N2) = 1518.78 g
Therefore, approximately 1518.78 grams of magnesium nitride are formed from 45.1 moles of magnesium.