CHM1020 Week 5
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Chemistry
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Jan 9, 2024
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Name(s): ____Casey Zufall
______________
CHM 1020 W5
Week 5 Assignment Objective
In today’s lab, we will demonstrate a few different types of chemical reactions and be able to observe whether a chemical reaction has taken place. We will also learn how to use chemical equations to describe chemical reactions.
Background/Theory
The Periodic Table shows over 100 elements. The chemical literature describes millions of compounds that are known—some isolated from natural sources, some synthesized by laboratory workers. The combination of chemicals, in the natural environment or the laboratory setting, involves chemical reactions. The change in the way that matter is composed is a chemical reaction
, a process wherein reactants (or starting materials) are converted into products. The new products often have properties and characteristics that are entirely different from those of the starting materials.
Four ways in which chemical reactions may be classified are combination, decomposition, single replacement (substitution), and double replacement (metathesis).
Two elements reacting to form a compound is a combination reaction
. This process may be described by
the general formula:
A + B ⟶
AB
The rusting of iron or the combination of iron and sulfur are good examples.
4Fe(s) + 3O
2
(g) ⟶
2Fe
2
O
3
(s) (rust)
Fe(s) + S(s)
⟶
FeS(s)
Two compounds reacting together as in the example below also is a combination reaction.
CaO(s) + CO
2
(g) ⟶
CaCO
3
(s)
A compound which breaks down into elements or simpler components typifies the decomposition reaction
. This reaction has the general formula: AB ⟶
A + B
Some examples of this type of reaction are the electrolysis of water into hydrogen and oxygen:
2H
2
O(l) ⟶
2H
2
(g) + O
2
(g)
and the decomposition of potassium iodate into potassium iodide and oxygen: 2KIO
3
(s) ⟶
2KI(s) + 3O
2
(g)
The replacement of one component in a compound by another describes the single replacement
(or substitution
) reaction. This reaction has the general formula: AB + C ⟶
CB + A
Page 1
of 7
Name(s): ____Casey Zufall
______________
CHM 1020 W5
Processes which involve oxidation (the loss of electrons or the gain of relative positive charge) and reduction (the gain of electrons or the loss of relative positive charge) are typical of these reactions. Use of Table 1, the activity series of common metals, enables chemists to predict which oxidation-reduction reactions are possible. A more active metal, one higher in the table, is able to displace a less active metal, one listed lower in the table, from its aqueous salt. Thus aluminum metal displaces copper metal from an aqueous solution of copper(II) chloride; but copper metal will not displace aluminum from an aqueous solution of aluminum(III) chloride.
2Al(s) + 3CuCl
2
(aq) ⟶
3Cu(s) + 2AlCl
3
(aq)
Cu(s) + AlCl
3
(aq) ⟶
No Reaction
(
Note that Al is oxidized to Al
3+ and Cu
2+ is reduced to Cu.
)
Hydrogen may be displaced from water by a very active metal. Alkali metals are particularly reactive with water, and the reaction of sodium with water often is exothermic enough to ignite the hydrogen gas released.
2Na(s) + 2HOH(l) ⟶
2NaOH(aq) + H
2
(g) + heat
(Note that Na is oxidized to Na
+ and H
+ is reduced to H
2
.)
Active metals, those above hydrogen in the series, are capable of displacing hydrogen from aqueous mineral acids such as HCl or H
2
SO
4
; however, metals below hydrogen will not replace hydrogen. Thus zinc reacts with aqueous solutions of HCl and H
2
SO
4 to release hydrogen gas, but copper will not.
Zn(s) + 2HCl(aq) ⟶
ZnCl
2
(aq) + H
2
(g) Cu(s) + H
2
SO
4
(aq) ⟶
No reaction
Two compounds reacting with each other to form two different compounds describes double replacement reactions. This process has the general formula: AB + CD ⟶
AD + CB
There are two replacements in the sense that A replaces C in CD and C replaces A in AB. This type of reaction generally involves ions which form in solution either from the dissociation of ionic compounds or the ionization of molecular compounds. The reaction of an aqueous solution of silver nitrate with an aqueous solution of sodium chloride is a good example. The products are sodium nitrate and silver chloride. We know a reaction has taken place since the insoluble precipitate silver chloride forms and separates from solution.
AgNO
3
(aq) + NaCl(aq) ⟶
NaNO
3
(aq) + AgCl(s) (White precipitate)
In general, a double replacement results if one combination of ions leads to a precipitate, a gas or an un-
ionized or very slightly ionized species such as water. In all of these reaction classes, it is very often possible to use your physical senses to observe whether a chemical reaction has occurred. The qualitative criteria may involve the formation of a gaseous product, the formation of a precipitate, a change in color, or a transfer of energy.
In the next section, you will practice identifying which of the four classes or classification of chemical reactions mentioned above does each chemical reaction represent. Note, in addition to combination, decomposition, single replacement and double replacement reactions, we also have combustion reactions, which you will explore in later assignments. For now, each reaction listed will fall into one of the four categories described here.
Page 2
of 7
Name(s): ____Casey Zufall
______________
CHM 1020 W5
Practice determining reaction classification
For each of the reactions below, classify as a combination, decomposition, single replacement, or double
replacement.
1.
Ca(s) + Cl
2
(g) ⟶
CaCl
2
(s)
Combination
2.
2Cu(s) + O
2
(g) ⟶
2CuO(s)
Combination
3.
Ca(NO
3
)
2
(aq) + H
2
SO
4
(aq)
⟶
2HNO
3
(aq)
+ CaSO
4
(s)
Double displacement
4.
NH
3
(aq) + HCl(aq) ⟶
NH
4
Cl(aq)
Combination
5.
Hg(NO
3
)
2
(aq) + 2NaI(aq) ⟶
HgI
2
(s) + 2NaNO
3
(aq)
Double displacement
6.
AgNO
3
(aq) + NaCl(aq) ⟶
AgCl(s) + NaNO
3
(aq)
Double displacement
7.
Zn(s) + H
2
SO
4
(aq) ⟶
ZnSO
4
(aq) + H
2
(g)
Single displacement
8.
H
2
CO
3
(aq) ⟶
CO
2
(g) + H
2
O(l)
Decomposition
9.
2H
2
O(l) ⟶
2H
2
(g) + 2O
2
(g)
Decomposition
10.
2Li(s) + 2H
2
O(l) ⟶
2LiOH(aq) + H
2
(g)
Combination
Page 3
of 7
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Related Questions
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Using a balance, mass between 1.50 – 2.00 grams of sodium carbonate in a pre-massed 150mL beaker.
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Pour the calcium chloride solution into the 150mL beaker containing the sodium carbonate solution and stir.
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Slowly pour the mixture from the beaker into the funnel and collect the filtrate into a 125mL erlenmeyer flask. Do not allow the mixture to rise above the edge of the filter paper.
Rinse the beaker with about 10 mL of distilled water.…
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read the Procedure and answer the post lab questions below:
Using a balance, mass between 1.50 – 2.00 grams of sodium carbonate in a pre-massed 150mL beaker.
Add 20 mL of distilled water and stir thoroughly to make sure all the crystals are dissolved. Rinse the stirring rod with a little distilled water after stirring.
Using a balance, mass between 1.50 – 2.00 grams of calcium chloride dihydrate in a pre-massed 50 mL beaker.
Repeat Step 2 for the solution in the 50 mL beaker.
Pour the calcium chloride solution into the 150mL beaker containing the sodium carbonate solution and stir.
Mass a piece of filter paper. Fold the filter paper and place it into the funnel. Wet it with a little distilled water to ensure that it is stuck to the sides of the funnel.
Slowly pour the mixture from the beaker into the funnel and collect the filtrate into a 125mL erlenmeyer flask. Do not allow the mixture to rise above the edge of the filter paper.
Rinse the beaker with about 10 mL of distilled water.…
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c. Collect the glass and throw it in the sharps bin and let the spill air-dry.
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