CHEM 165
CHM138LL
Lab 5
Stoichiometry Analysis of a Chemical Reaction
Name:
A. Data Tables
Item Measured/Quantity Calculated
Mass (in grams)
Iron nails (before reaction)
7.75g
5.5g
Iron nails (after reaction)
Mass of iron consumed
2.25g
Initial mass of filter paper (before filtration)
0.86g
3.52g
2.66g
Mass of filter paper and solid product
Mass of solid product
Show work below for “mass of iron consumed” and “mass of solid formed” calculations:
7.75g-5.5g=2.25g
3.52g-.086g=2.66g
B. Follow-up Questions
Show all work for questions involving calculations.
1. What color was the 1M CuCl2·2H20 solution before the nails were placed in it? What ion was responsible for this color? (16 pts.) The color was blue and the ion responsible for it is Cu2+.
2. After the nails were allowed to react, did the solution change color? What was responsible for this color change? (16 pts.) Yes, it changed to a green color and the ion responsible for it was Fe2+. Iron atoms were oxidized, giving two electrons to copper ions which were reduced.
3. What type of reaction was this? Why did it take place? Using the activity series of metals, explain why this reaction was possible. (16 pts.) Fe + Cu^+2(aq) ---> Fe^+2(aq)
+ Cu. This was a single displacement reaction. It took place, because the iron atoms gave up two of their electrons to the Cu2+.
4. What was the solid product that formed on the nails? How do you know this? It was rust.
When iron comes in contact with water it corrodes and rust is a byproduct. (16 pts.)
5. Determine the mass of iron consumed in the reaction. Show your work. (16 pts.)
7.75-5.5g=2.25g
6. Calculate the number of moles of iron consumed. Show your work. (16 pts.)
2.25G X 1MOL FE/55.85g= 0.040286 = 0.040286=0.0403 moles Fe
Formula:
Mass Fe used X
1 mol Fe
=
Moles of iron used Molar mass of
Fe
7. Determine the mass of product formed. Show your work. (16 pts.)
3.52g-.086g=2.66g
Formula:
(Mass of
Lab 5
Stoichiometry Analysis of a Chemical Reaction
Name:
A. Data Tables
Item Measured/Quantity Calculated
Mass (in grams)
Iron nails (before reaction)
7.75g
5.5g
Iron nails (after reaction)
Mass of iron consumed
2.25g
Initial mass of filter paper (before filtration)
0.86g
3.52g
2.66g
Mass of filter paper and solid product
Mass of solid product
Show work below for “mass of iron consumed” and “mass of solid formed” calculations:
7.75g-5.5g=2.25g
3.52g-.086g=2.66g
B. Follow-up Questions
Show all work for questions involving calculations.
1. What color was the 1M CuCl2·2H20 solution before the nails were placed in it? What ion was responsible for this color? (16 pts.) The color was blue and the ion responsible for it is Cu2+.
2. After the nails were allowed to react, did the solution change color? What was responsible for this color change? (16 pts.) Yes, it changed to a green color and the ion responsible for it was Fe2+. Iron atoms were oxidized, giving two electrons to copper ions which were reduced.
3. What type of reaction was this? Why did it take place? Using the activity series of metals, explain why this reaction was possible. (16 pts.) Fe + Cu^+2(aq) ---> Fe^+2(aq)
+ Cu. This was a single displacement reaction. It took place, because the iron atoms gave up two of their electrons to the Cu2+.
4. What was the solid product that formed on the nails? How do you know this? It was rust.
When iron comes in contact with water it corrodes and rust is a byproduct. (16 pts.)
5. Determine the mass of iron consumed in the reaction. Show your work. (16 pts.)
7.75-5.5g=2.25g
6. Calculate the number of moles of iron consumed. Show your work. (16 pts.)
2.25G X 1MOL FE/55.85g= 0.040286 = 0.040286=0.0403 moles Fe
Formula:
Mass Fe used X
1 mol Fe
=
Moles of iron used Molar mass of
Fe
7. Determine the mass of product formed. Show your work. (16 pts.)
3.52g-.086g=2.66g
Formula:
(Mass of