1) Mg + F2 = MgF2
10.00 grams of magnesium reacted with fluorine to produce MgF2
Find :
a) Balance the reaction
b) How many grams of fluorine reacted with magnesium. Answer:____________
c) How many grams of MgF2 were formed in the reaction. Answer:____________
a) The reaction is balanced as is.
b) mols Mg = grams/molar mass.
Use the coefficients in the balanced equation to convert mols Mg to mols F2.
Convert mols F2 to grams. g = mols x molar mass.
c) You have grams Mg and grams F2, The totals will be grams MgF2.
a) To balance the reaction, we need to ensure that we have an equal number of atoms on both sides of the equation. Let's start by counting the number of atoms of each element on both sides:
On the left-hand side:
- Magnesium (Mg): 1 atom
- Fluorine (F): 2 atoms
On the right-hand side (after balancing):
- Magnesium (Mg): 1 atom
- Fluorine (F): 2 atoms
Since we already have one atom of Mg on both sides, we can focus on balancing the fluorine. We need to have the same number of fluorine atoms on both sides, which is currently 2 on the left side and 2 on the right side. So, the balanced equation is:
Mg + F2 → MgF2
b) To determine the number of grams of fluorine that reacted with magnesium, we need to use the given information that 10.00 grams of magnesium reacted.
From the balanced equation, we can see that the mole ratio of magnesium to fluorine is 1:1. This means that for every 1 mole of magnesium that reacts, 1 mole of fluorine is consumed.
To calculate the number of moles of magnesium, we can use its molar mass. The molar mass of magnesium (Mg) is approximately 24.31 g/mol. Therefore,
Number of moles of magnesium = mass of magnesium / molar mass of magnesium
= 10.00 g / 24.31 g/mol
≈ 0.411 moles
Since the mole ratio of magnesium to fluorine is 1:1, the number of moles of fluorine that reacted is also 0.411 moles.
To convert moles of fluorine to grams, we need to multiply by its molar mass. The molar mass of fluorine (F2) is approximately 38.00 g/mol. Therefore,
Mass of fluorine = number of moles of fluorine × molar mass of fluorine
= 0.411 moles × 38.00 g/mol
≈ 15.64 grams
Therefore, approximately 15.64 grams of fluorine reacted with magnesium.
c) To determine the number of grams of MgF2 formed in the reaction, we can use the same approach as before.
From the balanced equation, we can see that the mole ratio of magnesium to MgF2 is 1:1. This means that for every 1 mole of magnesium that reacts, 1 mole of MgF2 is formed.
Since we already know the number of moles of magnesium (0.411 moles) that reacted, we can directly say that the number of moles of MgF2 formed is also 0.411 moles.
To convert moles of MgF2 to grams, we need to multiply by its molar mass. The molar mass of MgF2 is approximately 62.30 g/mol. Therefore,
Mass of MgF2 = number of moles of MgF2 × molar mass of MgF2
= 0.411 moles × 62.30 g/mol
≈ 25.58 grams
Therefore, approximately 25.58 grams of MgF2 were formed in the reaction.