Calorimeter - Definition, Uses, Types, Application, Diagram, FAQs

Definition of Calorimetry

The study of the measurement of the changes that occur in the state variable of anybody to find the amount of heat transfer that happens along with state transfer is defined as calorimetry. For example, finding the change of state variable during any phase transitions or other kinds of physical changes. The calorimeter is the instrument used in the study of calorimetry.

Principle of Calorimeter

Consider any two different bodies such as one solid and one liquid in different temperatures. Place the two different bodies such that both are in physical constant. The observations show that the heat transformations occur from the higher temperature body to the lower temperature body. This transformation occurs until both bodies attain thermal equilibrium. The heat is released by the higher-temperature body and the heat is absorbed by the lower-temperature body. Thus the energy is conserved in this process. The calorimeter also works with the same principle. The main principle of the calorimeter is the law of conservation of energy. The heat loss of one body is compensated by the heat gained by another body.

The formula of the Calorimeter with which it works:

From the conservation of the energy, Heat loss = heat gain

q=mcΔt

Where q denotes the measure of the transfer of heat

m denotes the body mass

c denotes the specific heat of the object

Δtdenotes the temperature change

Calorimeter - Explanation in Detail

The physical instrument or device which is used in the measurements of heat-related stuff (that is mainly used in the study of calorimetry). The construction of the calorimeter contains vessels made up of good conductors like metals. The composition of metallic vessels contains copper and aluminium in major. The contents of the metallic vessel are facilitated for stirring with the help of a stirrer. The heat loss in the stirrer is reduced with the help of an insulated jacket around the stirrer. The thermometer is allowed to be inserted through a small opening which is used to measure the thermal change that occurs inside the calorimeter.

In the inner part of the calorimeter, some sample of fuel is used to burn. The metallic vessel contains water, when the fuel inside is burnt, the water gets heated. The heat loss of the fuel is converted into the heat gained by the water. That is, energy is conserved. To increase the accuracy of results, heat loss can be terminated by the insulation of the calorimeter instrument from the environmental conditions. The heat change of the water is measured by using the inserted thermometer. The readings are used to find the heat capacity of the water and the amount of energy conserved inside the fuel.

Calorimetry Uses

A detailed study in the thermodynamic analysis of the substance and environment is required to answer the relationship between the particles, their structure and other properties of that particle.

Calorimeter Types

There are different types of Calorimeters used in practice. Some of the calorimeters are listed below: they are;

• Adiabatic calorimeters
• Constant pressure calorimeter
• Reaction calorimeters
• Differential scanning calorimeter
• Bomb calorimeters

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Solved Examples Based on the Calorimetry Principle

Example 1: Principle of calorimetry is based on

1) conservation of mass

2) conservation of energy

3) conservation of momentum

4) both 1 and 2

Solution:

Calorimetry

Heat lost = Heat gained

wherein

Represents the law of conservation of energy

Hence, the answer is the option 2.

Example 2: An unknown metal of mass 192 g heated to a temperature of 100⁰ C was immersed into a brass calorimeter of mass 128 g containing 240 g of water at a temperature of 8.4⁰C. Calculate the specific heat (in J Kg^-1 K^-1) of the unknown metal if the water temperature stabilises at 21.5⁰ C. (The specific heat of brass is 394 J Kg^-1 K^-1)

1) 458

2) 1232

3) 654

4) 916

Solution:

From the law of conservation of energy

Heat lost = Heat gained

So

192×s(100−21.5)=128×394(21.5−8.4)+240×4200(21.5−8.4)s=916Jkg−1 K−1

Hence, the answer is the option (4).

Example 3: A liquid of mass m and specific heat C is heated to a temperature "2T". Another liquid of mass m/2 and specific heat 2 C is heated to a temperature T . If these two liquids are mixed the resulting temperature of the mixture is

1) 2T/ 3

2) 8T/5

3) 3T/5

4) 3T/2

Solution:

The mixture of two substances
θ_mix=m₁c₁θ₁+m₂c₂θ₂m₁c₁+m₂c₂

wherein
θmix = The temperature of the mixture at equilibrium.

Tmix=m1C1T1+m2C2T2m1C1+m2C2=mc⋅2T+m2⋅2C⋅Tmc+m/2⋅2C=3mCT2mC=3T2

Hence, the answer is the option (4).

Example 4: Ice at −20∘C is added to 50 g of water at 40∘C. When the temperature of the mixture reaches 0∘C, it is found that 20 g of ice is still unmelted. The amount of ice (in gm) added to the water was close to :
(Specific heat of water =4.2 J/g/∘, Specific heat of ice =2.1 J/g/∘C, Heat of fusion of water at 0∘C=334 J/g )

1) 100

2) 50

3) 40

4) 60

Solution:

A mixture of two substances

θmix=m1c1θ1+m2c2θ2m1c1+m2c2 wherein θmix= The temperature of the mixture is at equilibrium. Say the amount of ice =mgm heat taken by ice = heat given by water 20×2.1×m+(m−20)334=50×4.2×40⇒m=40.1≈40

Hence, the answer is 40.

Example 5:5 g of water at 10∘C is mixed with 5 g of water at 40∘C, then final temperature (in celsius) of the mixture is

1) 20

2) 25

3) 30

4) 35

Solution:

If m1=m2 and c1=c2θmix=θ1+θ22θ=θ1+θ22=40+102=25∘C

Hence, the answer is the option (2).

Summary

Calorimetry is the study of heat transfer during physical changes or chemical reactions, governed by the principle of conservation of energy. A calorimeter measures heat exchange between substances, such as the heat lost by a hotter object being equal to the heat gained by a cooler one. This principle has applications in various fields, from everyday activities like boiling water to complex scientific and industrial processes.