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|
Experiment to measure the Specific
Heat Capacity of Water
| 1.
Preparation: |
a) |
Learn the
definition of specific heat capacity. |
|
b) |
Revise
electrical power and energy. |
|
c) |
Write a list of all
the results you will need to take during the experiment. It is a
good idea to try to write the list in the order that you will
take the results. |
|
d) |
Derive an equation
from which the specific heat capacity of water can be
calculated. |
|
e) |
See part
3 below. |
| 2. |
The diagram below
shows an insulated "calorimeter" suitable for use in
experiments of this type. A calorimeter is simply an aluminium
container for the water, with an aluminium stirrer. |
|
|
|
Measure the quantity
of heat needed to produce a measured temperature change in a
known mass of water. Use the ammeter and voltmeter (together
with a stop-watch) to find the quantity of electrical energy put
into the heater. |
|
| a) |
An
electric heater is 100% efficient. This means that the
quantity of heat energy given out is equal to the
electrical energy put in. |
| b) |
As
you heat the water you are, of course, also heating the
aluminium. Al is a very good conductor so we can assume
that at all times during the experiment, the Al has the
same temperature as the water. |
| c) |
Specific
heat capacity of aluminium = 908 Jkg-1°C-1 |
|
|
Do the experiment as many times as
you can in the time available using different masses of water. |
| 3. |
The temperature changes involved
should not be less than (about) 10°C but not more
than (about) 30°C. Why are there these limitations? |
|
© David
Hoult 2008 |
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Open Door Web Site