Name __________________________________________ Class _______ Date ____________
Lab Partners: ______________________, _____________________, ____________________
Chemical Reactions Lab
Objectives: In performing this experiment, students will
1. predict products of the reaction, mix chemicals, observe reactions, write a representation of the reaction
and balance the chemical equations;
2. identify type of reactions;
3. calculate mass, moles and number of particles (molecules, formula units, ions) in chemical compounds;
4. determine the limiting reactant; and
5. calculate percent yield.
Pre-Lab: Write your predictions when mixing in the table below.
Table 1. Chemical Reactions Predictions
Reactant 1
Reactant 2
Station 1:
Magnesium
Ribbon
Oxygen
in air
Station 2:
Aqueous silver
nitrate solution
Aqueous sodium
chloride solution
Station 3:
Ethyl
Alcohol
Oxygen
in air
Station 4:
Mossy
Zinc
Hydrochloric
Acid
Station 5:
Hydrochloric
acid
Sodium
hydroxide
Station 6:
Copper
sheet/wire
Aqueous sodium
chloride solution
Station 7:
Copper sulfate
pentahydrate heated
no
reaction
solid
Prediction: Reaction produces
gas heat/ different
Other
flame
color
Predictions
Procedure:
NOTE: Record all measurements for all reactions. Write your observations in Table 2.
Mix the chemicals as directed below.
Reaction 1. Measure about 1 inch of magnesium ribbon. Using the electronic balance, measure the mass of the
magnesium ribbon. (Caution: Burning magnesium will produce a very bright light. DO NOT look
directly at the flame as it will hurt your eyes.) Hold one end of the ribbon with a crucible tongs and place it in
the hottest part of the Bunsen burner (inner cone of the burner). If the ribbon is not completely burned, use
forceps to hold the remaining magnesium ribbon so everything is burned completely. Measure the mass of the
white substance produced. Write your observations in Table 2.
Reaction 2. Place 1 mL of aqueous silver nitrate solution (1.0 M; 0.1699 g in 1 mL) in 20 mL of aqueous
sodium chloride solution (50% by mass). Measure the mass of a piece of filter paper. Record the mass: ____ g.
Write your name on the edge of the filter paper. Filter the mixture. Let the filter paper dry and measure its mass
next class period. Write your observations in Table 2.
Reaction 3. (Teacher Demonstration) Place about 5 mL of ethyl alcohol in an evaporating dish. Using a
burning splinter, light up the alcohol until all of it is consumed. Write your observations in Table 2.
Reaction 4. Measure about 1-2 grams of zinc and place it in a test tube. Measure 5 mL of hydrochloric acid
(1.0 M HCl) in a graduated cylinder and place it in a test tube. Add the zinc to the HCl in the test tube.
Observe. Write your observations in Table 2.
Reaction 5. Place 10 mL of hydrochloric acid (0.1 M) in an Erlenmeyer flask. Add 1 drop of phenolphthalein
indicator. Record observation. Read and record the volume of sodium hydroxide in the buret. Using the buret
containing sodium hydroxide, add sodium hydroxide drop by drop until a faint pink color appears. Read and
record the volume of sodium hydroxide remaining in the buret.
Reaction 6. Measure about 5 mL of aqueous sodium chloride solution (50% NaCl solution) and add a small
piece of copper to it. Observe. Write your observations in Table 2.
Reaction 7. Measure 5 grams of copper sulfate pentahydrate. Place it in an evaporating dish and heat it at
325oC on a hot plate until it turns white. Let it cool on the lab table for about 10 minutes. Measure its mass and
record in Table 2.
Table 3. Chemical Reaction Stoichiometry.
For Reaction 1
Name of Reactant 1:
Name of Reactant 2:
Name of Product 1:
Name of Product 2:
Balanced Chemical Equation:
Type of Reaction:
Mass
(g)
Molar Mass
(g/mole)
Moles
No. of Particles/mole
(Avogadro’s No.)
No. of Particles
(Atoms, Molecules, etc.)
Magnesium ribbon
Burnt magnesium
Oxygen
For Reaction 2
Name of Reactant 1:
Name of Reactant 2:
Name of Product 1:
Name of Product 2:
Balanced Chemical Equation:
Type of Reaction:
Mass
(g)
Silver nitrate
Sodium chloride
Greyish white solid
Dissolved substance in H2O
Molar Mass
(g/mole)
Moles
No. of Particles/mole
(Avogadro’s No.)
No. of Particles
(Atoms, Molecules, etc.)
For Reaction 3
Name of Reactant 1:
Name of Reactant 2:
Name of Product 1:
Name of Product 2:
Balanced Chemical Equation:
Type of Reaction:
Mass
(g)
Molar Mass
(g/mole)
Moles
No. of Particles/mole
(Avogadro’s No.)
No. of Particles
(Atoms, Molecules, etc.)
Ethyl alcohol
Oxygen
Gaseous product 1
Gaseous product 2
For Reaction 4
Name of Reactant 1:
Name of Reactant 2:
Name of Product 1:
Name of Product 2:
Balanced Chemical Equation:
Type of Reaction:
Mass
(g)
Zinc metal
Hydrochloric acid (1.0 M)
Gaseous product
Dissolved substance
in water
Molar Mass
(g/mole)
Moles
No. of Particles/mole
(Avogadro’s No.)
No. of Particles
(Atoms, Molecules, etc.)
For Reaction 5
Name of Reactant 1:
Name of Reactant 2:
Name of Product 1 (salt):
Name of Product 2:
Balanced Chemical Equation:
Type of Reaction:
Mass
(g)
Molar Mass
(g/mole)
Moles
No. of Particles/mole
(Avogadro’s No.)
No. of Particles
(Atoms, Molecules, etc.)
Hydrochloric acid (0.1 M)
Sodium hydroxide
Salt dissolved in water
Product 2
For Reaction 6
Name of Reactant 1:
Name of Reactant 2:
Name of Product 1:
Name of Product 2:
Balanced Chemical Equation:
Type of Reaction:
Mass
(g)
Sodium chloride
Copper metal
Product 1
Product 2
Molar Mass
(g/mole)
Moles
No. of Particles/mole
(Avogadro’s No.)
No. of Particles
(Atoms, Molecules, etc.)
For Reaction 7
Name of Reactant 1:
Name of Reactant 2:
Name of Product 1:
Name of Product 2:
Balanced Chemical Equation:
Type of Reaction:
Mass
(g)
Copper (II) sulfate
pentahydrate
White substance
Product causing
the difference in mass
Molar Mass
(g/mole)
Moles
No. of Particles/mole
(Avogadro’s No.)
No. of Particles
(Atoms, Molecules, etc.)