WS/G.Sci/2
Ls. 4 Current Electricity and Magnetism
C) Look at the following diagram and answer the questions below
STD V111
Load
Resistance
- Cathode
Anode +
РЬО,
→ H,SO
Pb
2H
SO,
Lead Acid Cells
1. State the positive, negative terminal.
2. The electrolyte solution is of
3. Any 2 uses of the cell
4. State advantage
5. Can you extend battery life by storing batteries at low temperature?
Answers
Answer:
In electricity, a battery is a device consisting of one or more electrochemical cells that convert stored chemical energy into electrical energy. The dry cell is one of many general types of electrochemical cells.
A dry cell has the electrolyte immobilized as a paste, with only enough moisture in it to allow current to flow. Unlike a wet cell, a dry cell can operate in any orientation without spilling, as it contains no free liquid. This versatility makes it suitable for portable equipment. By comparison, the first wet-cell batteries were typically fragile glass containers with lead rods hanging from an open top. They, therefore, needed careful handling to avoid spillage. The development of the dry-cell battery allowed for a major advance in battery safety and portability.
A common dry-cell battery is the zinc-carbon battery, which uses a cell that is sometimes called the Leclanché cell. The cell is made up of an outer zinc container, which acts as the anode. The cathode is a central carbon rod, surrounded by a mixture of carbon and manganese(IV) dioxide (MnO2). The electrolyte is a paste of ammonium chloride (NH4Cl). A fibrous fabric separates the two electrodes, and a brass pin in the center of the cell conducts electricity to the outside circuit.
image
A zinc-carbon dry-cell battery: An illustration of a zinc-carbon dry cell. In it, a zinc casing acts as the anode, surrounding a carbon rod, which acts as a cathode. Between them, the electrolyte paste works as the battery.
Chemical reactions occur in every part of the battery to allow for energy storage; the reactions can be described using balanced chemical equations that delineate the electron flow. The paste of ammonium chloride reacts according to the following half-reaction:
2
NH
4
(
aq
)
+
2
e
−
→
2
NH
3
(
g
)
+
H
2
(
g
)
The manganese(IV) oxide in the cell removes the hydrogen produced by the ammonium chloride, according to the following reaction:
2
MnO
2
(
s
)
+
H
2
(
g
)
→
Mn
2
O
3
(
s
)
+
H
2
O
(
l
)
The combined result of these two reactions takes place at the cathode. Adding these two reactions together, we get:
Answer:
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