heat capacity simple experiment

Educating Physics

Determining Specific Heat Capacity Through Experiment

Objectives:

• To understand how to practically determine the specific heat capacity of a substance

Introduction  

A practical for specific heat capacity involves measuring the temperature changes of different materials when they are heated . An investigation involves linking the decrease of one store of one energy store to the increase in thermal energy store. As you would expect, the energy transferrer (work done) will cause a temperature to rise.

As you will have learned on the specific heat capacity page, the temperature rise of a material depends on its specific heat capacity. Materials with a low specific heat capacity (a low capacity to store thermal energy) will have a greater temperature increase than those with a high specific heat capacity.

Apparatus required

• Aluminium block with two holes, one for a thermometer and one for a heater
• 50 W, 12 V heater

• Thermometer
• Beaker (250 cm 3 )

Safety precautions

• The heating element will get very hot, especially if not inside a metal block. Take care not to burn yourself
• Damaged equipment should not be used (e.g. bare wires etc.)
• If you scald yourself with the heater or water then, cool under running cold water immediately for 10 minutes.
• Measure the mass of the aluminium block using the balance, if recorded in grams, this should be converted into kilograms.
• Place the heater and thermometer into the aluminium block

• Measure the  starting temperature of the metal block (you may need to wait for the thermometer to stop changing first).
• Turn the power pack on and up to about 5V, this can be higher for certain heaters (but it will say the maximum on it)
• Record the ammeter and voltmeter readings every 60 seconds in a table like that shown further down this page. These values may vary during the experiment, but they shouldn’t do significantly. Whilst recording the ammeter and voltmeter reading, also record the new temperature of the block at each 60s interval.
• After about 10 minutes turn off the power supply.
• Keep the thermometer in the metal block for a while longer. Record the maximum temperature of the block. The heater will still have some energy after you have turned off the power supply so you want to record any additional temperature rise from this energy.

Examples of results tables you should consider using:

Things to consider before experimenting

• The heating element should fit very snuggly into the metal block, but there may be a small layer of air between the heating element  and the metal block. Add a drop of water before you put the heating element in to improve transfer of energy between the heating element and the metal block.
• Remember to measure the mass of the metal block. These blocks are usually 1kg, but to make sure your calculations are accurate, you should take an accurate mass measurement.
• Make sure you heat the metal block for at least 10 minutes; otherwise you will not be able to draw a graph with a good range of results.
• Don’t forget to use your graph to find the gradient of the line. You will need this and the mass of the block to work out the specific het capacity  of the metal.

Analysing the results

After drawing you line of best and taking your gradient the specific heat capacity can be found by using the following equation:

Exemplar graph and results:

****waiting for a good graph to be drawn from a student ****

• Usually, the value for specific heat capacity found is higher than it should be, this is because more energy is put into the system than that used to heat up the substance. Some energy goes into wasted energy, such as heat loss to the surroundings. To improve the results, an insulation material should be used around the block.
• If you are trying to determine the specific heat capacity of a liquid, then the liquid should be stirred before each measurement to ensure all the water is the same temperature. Additionally, a lid should be used, since heat rises this is one way thermal energy can be lost to the surroundings.

Further reading:

• Specific heat capacity – S-cool

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Specific Heat Capacity Test: The Method of Mixture

1.0 introduction.

The method of mixture is used almost universally by scientists as a quick, easy, and semi-accurate specific heat test for a solid sample, but what makes this method extra special is the fact that it’s so simple that high school students around the world perform it as a hands-on example of how the specific heat capacities of materials are a part of the world around us. This very same experiment can be done with very expensive equipment in a high-tech lab, or in a home kitchen with some glassware, and the only difference will be the accuracy of the results, which can be improved by repeating the experiment and using the average of the results.

The biggest factor in the accuracy of your results will be the quality of calorimeter you are using. Calorimeters are used to measure the heat transfer from a sample into a container of water. Calorimeters can now be found in a few different and very complicated forms in professional labs, but we will be focused on the simple crucible model, as that is what fits the needs of this experiment.

A calorimeter of this sort has a dry inner chamber for the sample, (a crucible), the walls of which are made of a material with a high thermal conductance. The middle chamber is filled with the water that will have its temperature measured with a built-in thermometer probe. Most calorimeters will also have a built-in stir rod to speed up reactions and heat transfers. On the other side of the middle chambers thin walls will be an air gap, and then a thick layer of insulating material.

Professional calorimeters are designed this way to prevent heat from escaping as much as possible and they are often very expensive, but amateur, homemade, versions can be accurate enough for some uses. For example, if you nest two Styrofoam cups will make a water chamber followed by an air gap, then an insulating layer, as an inferior version of almost the same design of those that can be purchased.

2.0 Background Information and Relevant Equations

2.1 background information.

It is important to note that in this experiment, the better insulated your calorimeter is, the more accurate your results will be. Loss of heat by conduction is the main cause of error in this experiment.

The theory behind this specific heat test is based on the conservation of energy. Heat is a form of energy , and in this case, it will be transferred between the sample and water. We will be measuring the change in temperature of the water in the calorimeter, which lets us calculate the change in heat of the water in the calorimeter, which we know to be equal and opposite to the change in heat of the sample. It should now be becoming clear how convenient this specific heat capacity test is, because the only thing to do once the experiment is on the way, is to measure is the change in temperature of the water, which is an indirect measurement of the change in heat of the solid.

2.2 Relevant Equations

Change in heat.

Q = change in heat

c = specific heat capacity

ΔT = change in temperature

Conservation of energy

Q w = – Q s

Q w = change in heat of water

Q s = change in heat of sample

3.0 Materials, Experimental Set Up and Procedure

3.1 materials.

• Thermometer
• Glassware stand with a test tube grip arm
• Calorimeter

3.2 Experimental Setup

• Put the sample in a test tube.
• Attach the arm to the stand so it’s capable of gripping the test tube in place vertically, several inches above to tabletop.
• Prepare some distilled water.
• Set your hot plate to around 105 degrees Celsius.

3.3 Procedure

Measure the mass of the sample (m s ), and then weigh a beaker, then mostly fill the beaker with distilled water, weigh it again. Then to find the mass of the volume of distilled water (m w ), subtract the mass of the beaker from the combined mass of the beaker and water. Then pour that water in the calorimeter and set that aside for a time to ensure the water reaches ambient temperature, then measure its temperature (T i w ).

Fill the beaker with water again and set it on a hot plate until it reaches boiling, and keep the temperature steady, at just above boiling, measure that temperature, and record it as the initial temperature of the sample (T i s ).

Set up the glassware stand so that it is holding the test tube with the sample so that the length of the tube containing the sample is completely submerged in the boiling water. Leave this for at least ten minutes so that the sample will be heated evenly. Make sure the tube isn’t touching the sides or bottom of the glass.

When you are confident that the sample is heated evenly, disconnect the test tube from the stand and pour the sample into the calorimeter and shut the lid. Do this as quickly as you can while still being careful as to minimize the time the sample spends in contact with the air. Be sure to prevent any water that was adhering to the test tube from dripping into the calorimeter.

Keep close watch over the temperature in the calorimeter, and when it stops increasing, record it as the final temperature of both the water and the sample (T f w = T f s ).

4.0 Calculations and Comparisons

4.1 calculations.

Combing the equations for the change in heat,

With the principle of conservation of energy,

c w m w ΔT w = c s m s ΔT s

Which we can re-arrange to find the specific heat of the sample

c s = – c w m w ΔT w / (m s ΔT s )

4.2 Comparisons

You can compare the result of the specific heat of your material with our thorough database, generated in our professional laboratory.

https://thermtest.com/materials-database

5.0 Conclusion

This experiment is an extremely quick and relatively precise specific heat capacity test for a solid sample. Anyone with access to a kitchen can do a form of this experiment and become a thermal physicist.

‘Theory of Heat’ – Maxwell, James Clerk – page 57-67 – Westport, Conn., Greenwood Press – 1970 : https://archive.org/details/theoryheat04maxwgoog/page/n77

Talks about conservation of heat, the form and function of calorimeters, Method of Mixture

‘The Edinburgh Encyclopedia Conducted by David Brewster’ , with the assistance of gentlemen eminent in science and literature the first American edition – Published by Joseph and Edward Parker in 1832 – page 294 : http://bit.ly/2Lz2vdN

This is a discussion of Dr Joseph Black’s and Dr William Irvine groundbreaking discovery of specific heat capacity.

Dr. Joseph Black’s and Dr William Irvine’s original work on the concept of heat was published posthumously by the efforts of Dr John Robinso, as Dr. Black did not want to take the time away from his teachings to publish it. Below is a version of that research. Every version I found is behind a paywall.

https://www.tandfonline.com/doi/abs/10.1179/amb.1978.25.3.176 published by Arthur Donovan in 2013

6.0 Save a Few Dollars

The entirety of this experiment can be made at home, save for a thermometer, by switching out the lab equipment with regular kitchen ware.

6.1 Calorimeter

You can make your own calorimeter by nesting two styrofoam cups and crafting a lid out of a third. Notice that nesting the cups will make a water chamber followed by an air gap, then an insulating layer, like in a professional calorimeter. Be sure to include a hole in the lid for the thermometer. You could also use a normal thermos as a calorimeter, as they are also designed to heavily reduce heat transfer of the interior with the surroundings.

6.2 Beaker and hot plate

You can just boil a pot of water on a stovetop, in place of the beaker and the hot plate.

6.3 Test Tube and Stand

You can use a pair of tongs as a replacement for a test tube, (as long as your sample is in one solid piece), preferably made of a plastic that won’t melt, so it won’t absorb to much heat, and the handle won’t get too hot. Be very careful and use thick oven mitts if you plan on holding it submersed in the boiling water for 10 minutes.

7.0 Notes on the Sample

7.1 size and shape.

Note that the more surface area your sample has in relation to its mass, the more likely it will be heated evenly. The more mass your sample is, however, the more heat it will absorb and the give off, meaning the result will be more accurate. One way to account for both traits is for your sample to be in a lot of smaller pieces instead of one big piece.

7.2 Non-homogeneous samples

If your sample is non-homogeneous, then the rule of mixtures can allow you to find the specific heat of one component if you know that of the others, or their relative masses if you know all the specific heats.

Author: Cole Boucher, Junior Technical Writer at Thermtest

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Specific Heat Capacity Experiment

Related Pages Specific Heat Capacity Energy Transfers Mechanical, Potential and Kinetic Energy Elastic Potential Energy Lessons for IGCSE Physics

A series of free GCSE/IGCSE Physics Notes and Lessons .

In these lessons, we will learn to describe a practical that can be used to determine the specific heat capacity of a material.

The specific heat capacity of a substance is the amount of energy required to raise the temperature of 1 kg of the substance by 1°C.

Specific Heat Capacity Practical

Steps to determine the specific heat capacity.

• Place a beaker on a balance and press zero.
• Now add the oil to the beaker and record the mass of the oil.
• Read the starting temperature of the oil.
• Connect a joulemeter to the immersion heater.
• Time for thirty minutes.
• Read the number of joules of energy that passed into the immersion heater.
• Read the final temperature of the oil.
• Use the following formula to calculate the specific heat capacity.

Results and Calculations

0.95 kg of oil was heated from 20°C to 75 °C. 87258J of electrical energy passed into the immersion heater. Calculate the specific heat capacity of the oil.

Sources of inaccuracies

• Thermal energy passing out of the beaker into the air - Use an insulator with a lower thermal conductivity.
• Not all thermal energy passing into the oil - Ensure that immersion heater is fully submerged.
• Incorrect reading of thermometer - Use an electronic temperature probe.
• Thermal energy not being spread through the oil - Stir the oil.

Experiment to show how to find the specific heat capacity of a metal

Specific Heat Capacity - GCSE Science Required Practical

Investigating the specific heat capacity of different metals.

In this practical you will:

• heat up blocks of different metals using an electric heater
• measure the mass and temperature of the block
• calculate the work done by the heater
• plot a graph of temperature change against work done and use the gradient to calculate the specific heat capacity of the metal
• Measure and record the mass of the copper block in kg.
• Wrap the insulation around the block.
• Place the heater in the larger hole in the block.
• Connect the ammeter, power pack and heater in series.
• Connect the voltmeter across the heater.
• Use the pipette to put a small amount of water in the other hole.
• Put the thermometer in this hole.
• Set the power pack to 12 V. Switch on the power pack to turn on the heater.
• Record the ammeter and voltmeter readings. These shouldn’t change during the experiment.
• Measure the temperature and start the stopclock.
• Record the temperature every minute for 10 minutes. Record your results in the table below.
• Calculate the power of the heater in watts. Power in watts = potential difference in volts x current in amps
• Calculate the energy transferred (work done) by the heater. To do this, multiply the time in seconds by the power of the heater. Record these values in your table.

Specific Heat Capacity - GCSE Science Required Practical How to measure the SHC of a material using the graph method?

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