CHEMICAL REACTIONS LAB REPORT
OBJECTIVE: This project is designed to assess the students’ ability to identify and evaluate the
five types of chemical reactions that are presented within this unit and justify their findings with
scientific reasoning.
Safety Precaution
List all safety precautions that would apply to the laboratory experiment you performed
this week.
Pre-Lab Question:
SYNTHESIS
Write the balanced equation for the following synthesis reaction. Solid potassium reacts with
chlorine gas to form potassium chloride.
DECOMPOSITION
1. Define Catalyst-A substance, usually used in small amounts relative to the reactants,
that modifies and increases the rate of a reaction without being consumed in the process.
2. Define inhibitor- an agent that slows or interferes with a chemical
SINGLE-REPLACEMENT
Write the single replacement reaction for solid zinc reacts with aqueous hydrochloric acid to
produce aqueous zinc chloride and hydrogen gas.
Zn (S) + 2HCl (L) -> ZnCl2 (L) + H2 (G)
DOUBLE-REPLACEMENT
Write the balanced equation for the following double-replacement reaction. Aqueous lithium iodide
and aqueous silver nitrate react to produce solid silver iodide and aqueous lithium nitrate.
LiI (L) + AgNO3 (L) -> AgI (S) + LiNO3 (L)
Post Lab Analysis:
SYNTHESIS
1. Write the chemical equation from the word equation: solid magnesium reacts with
oxygen gas to produce magnesium oxide. 2Mg (S) + O2 -> Mg2O
2. Balance the chemical equation from #1.
3. Complete the following equations:
Al(s) + O2(g)
Al2O3
SO3(g) + H2O(l)
H2SO4
DECOMPOSITION
1. What happened to the glowing toothpick when it was plunged into the gas above the liquid
in the test tube?
It reignited
2. What must be the gas that is released from the hydrogen peroxide solution? Write an
equation for this decomposition of hydrogen peroxide.
Oxygen.
H2O2 + MnO2 -> H2 + O2 + MnO2
3. Does the manganese dioxide undergo any apparent change during the reaction?
It splits into Manganese and Oxygen Gas
4. What is the role of manganese dioxide in the decomposition reaction?
A Catalyst
SINGLE-REPLACEMENT:
1.) Which metal reacted with the most solutions?
2.) Which metal reacted with the fewest solutions?
3.) Write balanced chemical equations for the following reactions that took place.
Solid copper reacts with aqueous silver nitrate to produce aqueous copper II nitrate and
solid silver
Cu (S) + AgNO3 (L) -> CuNO3 (L) + Ag (S)
Solid magnesium reacts with aqueous copper II nitrate to form solid copper and aqueous
magnesium nitrate
Mg (S) + CuNO3 (L) -> Cu (S) + MgNO3 (L)
Solid magnesium reacts with aqueous silver nitrate to produce solid silver and aqueous
magnesium nitrate
Mg (S) + AgNO3 (L) -> Ag (S) + MgNO3 (L)
Solid zinc reacts with aqueous copper II nitrate to form solid copper and aqueous zinc
nitrate
Zn (S) + CuNO3 (L) -> Cu (S) + ZnNO3 (L)
Solid zinc reacts with aqueous silver nitrate to produce solid silver and aqueous zinc nitrate
Zn (S) + AgNO3 -> Ag (S) + ZnNO3 (L)
DOUBLE-REPLACEMENT
1. Write the chemical equation from the reaction of aqueous lead II nitrate and aqueous potassium
iodide.
2. Balance the chemical equation.
3. Compare and contrast single-replacement reactions and double-placement reactions.