1. If 6.3 g of Fe reacts with 3.1 g of O₂ in a closed container, what mass of product will form?
3.1 g
3.2 g
9.4 g
19.5g
2. The reactant side for an equation is 6A₂B + 5AD₂. How many atoms of A must be on the product side because of the Law of Conservation of Matter?
11
17
12
22
Well, to answer your first question, if 6.3 g of Fe reacts with 3.1 g of O₂, we need to see which element is limiting the reaction. If we convert the masses of Fe and O₂ into moles, we can compare the stoichiometric ratios. The balanced equation is not provided, but let's assume it is:
Fe + O₂ → product
To calculate the moles of Fe, we can divide its mass (6.3 g) by its molar mass. Similarly, we can calculate the moles of O₂ by dividing its mass (3.1 g) by its molar mass. Whichever reactant has the lower number of moles will be the limiting reactant.
Once we determine the limiting reactant, we can use the stoichiometry of the balanced equation to find the mass of the product formed. Unfortunately, since the equation is not provided, we can't give an exact answer. So let's just go with the closest approximation, which is 3.1 g.
Now, let's move on to the second question. The reactant side of the equation is 6A₂B + 5AD₂. To satisfy the Law of Conservation of Matter, we must have the same number of atoms of each element on both sides of the equation. In this case, we have two atoms of "A" on the left side (6 A₂B), but only one atom of "A" on the right side (AD₂). So we need to balance the equation by multiplying the right side by 2, giving us:
6A₂B + 5AD₂ → 10AD₂
Now we have 12 atoms of "A" on the product side. So the answer is 12. Mmm, plenty of "A"s to go around!
1. To determine the mass of the product that will form, we need to determine the limiting reactant. This is the reactant that is completely consumed and determines the maximum amount of product that can form.
To find the limiting reactant, we can compare the moles of each reactant.
First, calculate the moles of Fe:
Molar mass of Fe = 55.845 g/mol
Moles of Fe = mass of Fe / molar mass of Fe = 6.3 g / 55.845 g/mol
Next, calculate the moles of O₂:
Molar mass of O₂ = 32.00 g/mol
Moles of O₂ = mass of O₂ / molar mass of O₂ = 3.1 g / 32.00 g/mol
Now, calculate the mole ratio between Fe and O₂ using the balanced equation. Let's assume the balanced equation is:
4Fe + 3O₂ -> 2Fe₂O₃
The mole ratio between Fe and O₂ is 4:3.
Now, compare the moles of Fe and O₂ using the mole ratio:
Moles of Fe / Mole ratio = 6.3 g / 55.845 g/mol / 4/3 ≈ 0.0798 mol
Moles of O₂ / Mole ratio = 3.1 g / 32.00 g/mol / 3/4 ≈ 0.1615 mol
Since the moles of Fe are smaller than the moles of O₂, Fe is the limiting reactant.
Finally, we need to calculate the mass of the product formed using the mole ratio from the balanced equation:
Molar mass of Fe₂O₃ = (Molar mass of Fe x 2) + (Molar mass of O x 3) = (55.845 g/mol x 2) + (16.00 g/mol x 3) = 159.69 g/mol
Mass of Fe₂O₃ = Moles of Fe x Molar mass of Fe₂O₃ = 0.0798 mol x 159.69 g/mol ≈ 12.72 g
Therefore, the mass of the product that will form is approximately 12.72 g.
2. According to the Law of Conservation of Matter, the total number of atoms of each element must be the same on both sides of a balanced chemical equation.
In the given equation 6A₂B + 5AD₂, we have 6 atoms of A on the reactant side and 2 atoms of A on the product side. To satisfy the Law of Conservation of Matter, we need to have a total of 6 atoms of A on the product side as well.
Since there are already 2 atoms of A on the product side, we need to add 4 more atoms. Therefore, the correct answer is 6 atoms of A.
1. To determine the mass of the product that will form, we need to determine the limiting reactant. This is the reactant that is completely consumed in the reaction and determines the maximum amount of product that can be formed.
To do this, we need to calculate the number of moles for each reactant by dividing the given mass by their respective molar masses.
Molar mass of Fe: 55.85 g/mol
Molar mass of O₂: 32.00 g/mol
Moles of Fe = 6.3 g / 55.85 g/mol ≈ 0.1126 mol
Moles of O₂ = 3.1 g / 32.00 g/mol ≈ 0.0969 mol
According to the balanced chemical equation, the stoichiometry between Fe and O₂ is 4:1. This means that for every 4 moles of Fe, 1 mole of O₂ is required.
Comparing the moles of Fe and O₂, we see that there is an excess of Fe and it will be the limiting reactant. Therefore, the mass of the product formed will be the mass of O₂.
Mass of O₂ = 3.1 g
So the correct answer is 3.1 g.
2. To determine the number of atoms of A on the product side, we need to consider the stoichiometry of the balanced chemical equation.
The reactant side of the equation is 6A₂B + 5AD₂. From this equation, we can see that there are 6 atoms of A in each molecule of A₂B.
Therefore, the number of atoms of A on the product side is given by:
6 atoms of A * 2 molecules = 12 atoms of A
So the correct answer is 12.