Answer:
a) Nor Mg, neither I2 is the limiting reactant.
b) I2 is the limiting reactant
c) <u>Mg is the limiting reactant</u>
<u>d) Mg is the limiting reactant</u>
<u>e) Nor Mg, neither I2 is the limiting reactant.</u>
<u>f) I2 is the limiting reactant</u>
<u>g) Nor Mg, neither I2 is the limiting reactant.</u>
<u>h) I2 is the limiting reactant</u>
<u>i) Mg is the limiting reactant</u>
Explanation:
Step 1: The balanced equation:
Mg(s) + I2(s) → MgI2(s)
For 1 mol of Mg we need 1 mol of I2 to produce 1 mol of MgI2
a. 100 atoms of Mg and 100 molecules of I2
We'll have the following equation:
100 Mg(s) + 100 I2(s) → 100MgI2(s)
This is a stoichiometric mixture. <u>Nor Mg, neither I2 is the limiting reactant.</u>
b. 150 atoms of Mg and 100 molecules of I2
We'll have the following equation:
150 Mg(s) + 100 I2(s) → 100 MgI2(s)
<u>I2 is the limiting reactant</u>, and will be completely consumed. There will be consumed 100 Mg atoms. There will remain 50 Mg atoms.
There will be produced 100 MgI2 molecules.
c. 200 atoms of Mg and 300 molecules of I2
We'll have the following equation:
200 Mg(s) + 300 I2(s) →200 MgI2(s)
<u>Mg is the limiting reactant</u>, and will be completely consumed. There will be consumed 200 I2 molecules. There will remain 100 I2 molecules.
There will be produced 200 MgI2 molecules.
d. 0.16 mol Mg and 0.25 mol I2
We'll have the following equation:
Mg(s) + I2(s) → MgI2(s)
<u>Mg is the limiting reactant</u>, and will be completely consumed. There will be consumed 0.16 mol of I2. There will remain 0.09 mol of I2.
There will be produced 0.16 mol of MgI2.
e. 0.14 mol Mg and 0.14 mol I2
We'll have the following equation:
Mg(s) + I2(s) → MgI2(s)
This is a stoichiometric mixture. <u>Nor Mg, neither I2 is the limiting reactant.</u>
There will be consumed 0.14 mol of Mg and 0.14 mol of I2. there will be produced 0.14 mol of MgI2
f. 0.12 mol Mg and 0.08 mol I2
We'll have the following equation:
Mg(s) + I2(s) → MgI2(s)
<u>I2 is the limiting reactant</u>, and will be completely consumed. There will be consumed 0.08 moles of Mg. There will remain 0.04 moles of Mg.
There will be produced 0.08 moles of MgI2.
g. 6.078 g Mg and 63.455 g I2
We'll have the following equation:
Mg(s) + I2(s) → MgI2(s)
Number of moles of Mg = 6.078 grams / 24.31 g/mol = 0.250 moles
Number of moles I2 = 63.455 grams/ 253.8 g/mol = 0.250 moles
This is a stoichiometric mixture. <u>Nor Mg, neither I2 is the limiting reactant.</u>
There will be consumed 0.250 mol of Mg and 0.250 mol of I2. there will be produced 0.250 mol of MgI2
h. 1.00 g Mg and 2.00 g I2
We'll have the following equation:
Mg(s) + I2(s) → MgI2(s)
Number of moles of Mg = 1.00 grams / 24.31 g/mol = 0.0411 moles
Number of moles I2 = 2.00 grams/ 253.8 g/mol = 0.00788 moles
<u>I2 is the limiting reactant</u>, and will be completely consumed. There will be consumed 0.00788 moles of Mg. There will remain 0.03322 moles of Mg.
There will be produced 0.00788 moles of MgI2.
i. 1.00 g Mg and 2.00 g I2
We'll have the following equation:
Mg(s) + I2(s) → MgI2(s)
Number of moles of Mg = 1.00 grams / 24.31 g/mol = 0.0411 moles
Number of moles I2 = 20.00 grams/ 253.8 g/mol = 0.0788 moles
<u>Mg is the limiting reactant</u>, and will be completely consumed. There will be consumed 0.0411 moles of Mg. There will remain 0.0377 moles of I2.
There will be produced 0.0411 moles of MgI2.
