Lab 5 Report
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name section date
EXPERIMENT: Chemical Reactions
Fill in all the information in boxes highlighted !
Data Table 1: Observations of reactions mixtures: (c/c = clear and colorless liquid)
Rxn
Reactants
Initial Observation of
Reactants
Observation After Reactants
Are Mixed Together
How Do You Know a
Reaction Has Occurred?
a
NaHCO3
+
HCl
b
HCl
+
blue dye
c
Blue dye
+
NaOCl
Then HCl
d
NaOCl
+
KI
Then starch
e
KI
+
Pb(NO3)2
f
Pb(NO3)2
+
CaCl2
Lab 5 Report
g
CaCl2
+
NaHSO4
h
NaHSO4
+
Na2CO3
i
Na2CO3
+
phen
j
Phen
+
NaOH
k
NaOH
+
AgNO3
l*
AgNO3
+
NH3
**Paper:
m*
NH3
+
CuSO4
n
CuSO4
+
NaHCO3
Lab 5 Report
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WORKSHEET: Chemical Equations
1. Fill in the products of the following combustion reactions in
and coefficients in
. If a coefficient is “1,” leave the green box blank. Also, remember what the
combustion products are when compounds containing only carbon, hydrogen, and oxygen are
burned (see p. 280 of the Guinn textbook for more details).
2. Using the information on p. 92 of the lab manual, predict which three of the following five
aqueous solutions should react with solid aluminum metal (the elemental form of aluminum):
AgNO3, Na2CO3, CuSO4, CaCl2, Pb(NO3)2. (HINT: This would be a single replacement reaction!)
State your prediction below and explain on what basis you are saying this.
3. Write the chemical equation for the three solutions above that reacted with pure aluminum
metal. Fill in the reactants and products in and coefficients in . If a
coefficient is “1,” leave the green box blank. Assuming that the aqueous product is an ionic
compound and the solid product is an element (by itself) in each case, use the “X rule” for
figuring out the formula unit of each product!
C
3
H
8
(g) +
O
2
(g) →
C
4
H
10
(g) +
O
2
(g) →
(g)
+
(g)
+
(g)
(g)
O2(g) →
(g) +
(g)
Al(s) +
(s) +
(aq)
Al(s) +
(s) +
(aq)
Al(s) +
(s) +
(aq)
(aq) →
(aq) →
(aq) →
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Lab 5 Report
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4. Balance the following equations, placing the coefficients in . If a coefficient is “1,”
leave the green box blank. In indicate reaction type: “C” for combination reactions,
“D” for decomposition, “SR” for single replacement, or “DR” for double replacement reactions.
Pb(NO3)2(aq) +
KI(aq) →
PbI2(s) +
KNO3(aq)
(NH
4
)
2
CO
3
(s) →
CO2(g) +
NH3(g) +
H2O(g)
K(s) +
B2O3(s) →
K2O(s) +
B(s)
N2(g) +
O2(g) →
N2O5(g)
NH3(g) +
HCl(g) →
NH4Cl(g)
NH3(g) +
O2(g) →
N2(g) +
H2O(g)
Pb(NO3)2(aq) +
CaCl2(aq) →
PbCl2(s) +
Ca(NO3)2(aq)
Fe(s) +
AgNO3(g) →
Ag(s) +
Fe(NO3)3(aq)
Mg(OH)2(s) +
HCl(aq) →
MgCl2(aq) +
HOH(g)
H2CO3(aq) →
H2O(l) +
CO2(g)
AgNO3(aq) +
NaCl(aq) →
AgCl(s) +
NaNO3(aq)
Lab 5 Report
Post-Laboratory Questions
A.
Why do chemical equations need to be balanced? Explain briefly!
B.
Which of the equations in Part 4 of the Worksheet were reactions that you did in the
experiment?
C.
In the reactions from question B above, identify the change in color or appearance with one of
the products. (HINT: Think about what cloudy appearance usually means!)
