Oxidation-Reduction Reactions Chemistry Worksheet Page 18
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41224
Chapter 6
Oxidation-Reduction Reactions
∆
(g) + 2PbO(s) + O
c. 2Pb(NO
)
(s)
4NO
(g)
3
2
2
2
Because one substance is being converted into more than one substance,
this is a decomposition reaction
.
SH(l ) + 9O
(g) → 5CO
(g) + 6H
O(l ) + SO
d. C
H
(g)
5
11
2
2
2
2
Because a substance combines with oxygen, and because we see carbon
in that substance going to CO
, hydrogen going to H
O, and sulfur
2
2
going to SO
, we classify this reaction as a combustion reaction. The
2
compound C
H
SH is 3‑methyl‑1‑butanethiol, a component of the
5
11
spray produced by skunks.
e
6.3 - Classification of Chemical Reactions
xerCise
Classify each of these reactions with respect to the following categories: combination
O
7
bjeCtive
reaction, decomposition reaction, combustion reaction, and single‑displacement
reaction.
∆
2Hg(l ) + O
a. 2HgO(s)
(g)
2
(s) + 12O
(g) → 12CO
(g) + 11H
b. C
H
O
O(l )
12
22
11
2
2
2
∆
(s) + 3Mg(s)
2B(s) + 3MgO(s)
c. B
O
2
3
(g) + H
(g) → C
d. C
H
H
( g)
2
4
2
2
6
6.4
Voltaic Cells
We’re people on the go…with laptop computers, portable drills, and electronic games
that kids can play in the car. To keep all of these tools and toys working, we need
batteries, and because the newer electronic devices require more power in smaller
packages, scientists are constantly searching for stronger and more efficient batteries.
The goal of this section is to help you understand how batteries work and to describe
some that may be familiar to you and some that may be new.
A battery is a device that converts chemical energy into electrical energy using redox
reactions. To discover what this means and how batteries work, let’s examine a simple
system that generates an electric current using the reaction between zinc metal and
copper(II) ions described in Figure 6.4. In this redox reaction, uncharged zinc atoms
are oxidized to zinc ions, and copper(II) ions are reduced to uncharged copper atoms.
2+
2+
Zn(s) + Cu
(aq) → Zn
(aq) + Cu(s)
Zn(s) → Zn
2+
(aq) + 2e
‒
oxidation:
2+
‒
(aq) + 2e
→ Cu(s)
reduction:
Cu
The last section showed how this reaction takes place when zinc metal is added to
2+
a solution of copper(II) sulfate. When a Cu
ion collides with the zinc metal, two
electrons are transferred from a zinc atom directly to the copper(II) ion.
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