Download Balancing Equations (A visual aid)

Name ___________________________________________________ Date ____________ Period _____
Lab: Balancing Equations (A Visual Aid)
Use Pencil Only!!
PROCEDURE:
I. Obtain a container of colored beads. If your container of beads does not have enough, get them from
the reserve stockpile at the teacher’s desk. The numbers shown below are the minimum for you to be
able to do the equation balancing.
II. For equations (1) - (7) below, complete the following steps:
a. Try to balance the equation first. Then, make a model of the equation using the beads.
b. A pipe cleaner should be used to string beads onto in order to represent formula units or molecules.
Pure elements (atoms) DO NOT need a pipe cleaner.
c. One of the lab partners should use his/her beads to simulate the reactants (left side) of the balanced
equation, and the other person should simulate the products (right side). If you have a third lab
partner, it is that person’s job to check the reactants and products. DO NOT split up molecules or
formula units! This is why they are on a pipe cleaner.
d. Use the index card, (+) and () to correctly show the balanced equation.
e. Make sure that there are the same number of pieces of each kind and color on each side of the
equation. When the equation is balanced, write the coefficient(s). DO NOT use the number one.
f. When you and your lab partner(s) have completed an equation, have Mrs. Pappalardo check the
balanced equation and the bead arrangement to verify that everything is correct.
Mrs. Pappalardo will mark in the space provided so that you will get credit.
(1)
_____ Na + _____ Cl2 → _____ NaCl
Check: _____
(2)
_____ Na + _____ H2O → _____ NaOH + _____ H2
Check: _____
(3)
_____ N2 + _____ H2 → _____ NH3
Check: _____
(4)
_____ Zn + _____ HCl → _____ ZnCl2 + _____ H2
Check: _____
(5)
_____ C + _____ Fe2O3 → _____ CO + _____ Fe
Check: _____
(6)
_____ ZnBr2 + _____ H2CO3 → _____ HBr + _____ ZnCO3
Check: _____
(7)
_____ Fe(OH)2 + _____ NaCl → _____ FeCl2 + _____ NaOH
Check: _____
III. For each of the chemical equations below, use colored pencils to show pictures of the molecules.
Make sure to draw as many reactants and products as you need to balance the reaction. Be sure to
include a color key for each of the elements. Fill in the final coefficient(s) in the blanks in front of the
molecules.
(1)
_____ HgO → _____ Hg + _____ O2
(1) Key:
(2)
_____ Al + _____ O2 → _____ Al2O3
(2) Key:
(3)
_____ Rb + _____ P → _____ Rb3P
(3) Key:
(4)
_____ KI + _____ Cl2 → _____ KCl + _____ I2
(4) Key:
(5)
_____ H2O2 → _____ H2O + _____ O2
(5) Key:
(6)
_____ KIO3 → _____ KI + _____ O2
(6) Key:
(7)
_____ Ca + _____ H2O → _____ Ca(OH)2 + _____ H2
(7) Key:
(8)
_____ CH4 + _____ O2 → _____ CO2 + _____ H2O
(8) Key:
(9)
_____ Na2O2 + _____ H2SO4 → _____ Na2SO4 + _____ H2O2
(9) Key:
(10)
_____ KMnO4 → _____ K2O + _____ MnO + _____ O2
(10) Key:
IV. Balance the following equations.
(1)
_____ AlBr3 + _____ K  _____ KBr + _____ Al
(2)
_____ FeO + _____ PdF2  _____ FeF2 + _____ PdO
(3)
_____ P4 + _____ Br2  _____ PBr3
(4)
_____ LiCl + _____ Br2  _____ LiBr + _____ Cl2
(5)
_____ PbBr2 + _____ HCl  _____ HBr + _____ PbCl2
(6)
_____ CoBr3 + _____ CaSO4  _____ CaBr2 + _____ Co2(SO4)3
(7)
_____ Na3P + _____ CaF2  _____ NaF + _____ Ca3P2
(8)
_____ Mn + _____ HI  _____ H2 + _____ MnI3
(9)
_____ Li3PO4 + _____ NaBr  _____ Na3PO4 + _____ LiBr
(10)
_____ CaF2 + _____ Li2SO4  _____ CaSO4 + _____ LiF
V. On loose leaf paper, write a letter to one of your family members explaining the process of balancing
equations. Use and highlight the following words: reactant, product, subscript, coefficient, and
balance.
1)
1 AlBr3 + 3 K  3 KBr + 1 Al
2)
1 FeO + 1 PdF2  1 FeF2 + 1 PdO
3)
1 P4 + 6 Br2  4 PBr3
4)
2 LiCl + 1 Br2  2 LiBr + 1 Cl2
5)
1 PbBr2 + 2 HCl  2 HBr + 1 PbCl2
6)
2 CoBr3 + 3 CaSO4  3 CaBr2 + 1 Co2(SO4)3
7)
2 Na3P + 3 CaF2  6 NaF + 1 Ca3P2
8)
2 Mn + 6 HI  3 H2 + 2 MnI3
9)
1 Li3PO4 + 3 NaBr  1 Na3PO4 + 3 LiBr
10)
1 CaF2 + 1 Li2SO4  1 CaSO4 + 2 LiF
molecules.
EXTENDED ASSESSMENT
Balance each of the following chemical reactions.
1) ____Fe(OH)3(s)  ____Fe2O3(s) + ____H2O(g)
2) ____Bi(NO3)3(aq) + ____CaI2(aq)  ____BiI3(s) + ____Ca(NO3)2(aq)
3) ____Na2CO3(aq) + ____Ca(OH)2(aq)  ____NaOH(aq) + ____CaCO3(s)
4) ____K3PO4(aq) + ____MgCl2(aq)  ____Mg3(PO4)2(s) + ____KCl(aq)
5) ____Cu(s) + ____H2SO4(aq)  ____CuSO4(aq) + ____H2O(l) ____SO2(g)
Analysis:
1. When a scientists reacts two or more compounds sometimes it forms a precipitate. A precipitate is a
solid substance that forms after a chemical reaction. When you dissolve both magnesium sulfate (Epsom
salt) and sodium carbonate in water you get two clear liquids. When you mix these two clear liquid a
precipitate forms, which means after mixing two liquids you see a solid. According to the Law of
Conservation of Matter does this solid contain different atoms than the two liquids?
Teacher Data Table of Beads
Element
H
O
Cl
N
C
Na
Fe
Zn
Br
Color
white
red
green
purple
black
yellow
blue
orange
pink
Quantity
12
12
8
8
8
8
8
8
8