Difference between Heat and Temperature

Heat :

1. The energy of hotness and coldness of the body is called the heat

2. Heat is the total kinetic energy of all the particles in a body, i.e., it is the sum of the kinetic energies of each individual particle in the body.

3. Heat is that form of energy which flows from a hot body to a cold body when they are kept in contact.

4. The amount of heat inside the body depends on mass, temperature, and the nature of the body.

5. The body's heat is measured by the principle of calorimetry.

6. Two bodies with the same amount of heat may differ in temperature.

7. When two bodies are placed in contact, the total amount of heat is equal to the sum of the heat of the individual bodies.

8. The heat can only be a positive value.

9. The S.I. unit of heat is $joule (J)$.

Temperature:

1. The measurement of energy (i.e., average energy) of hotness and coldness of the body is called temperature.

2. The body's temperature is equal to the average kinetic energy of all the particles in the body.

3. Temperature is a parameter that determines the direction of the flow of heat while keeping the two bodies at different temperatures in contact.

4. The temperature of a body depends on the average motion of the particles.

5. The thermometer is used to measure the body's temperature.

6. Two bodies at the same temperature may differ in the quantities of heat contained in them.

7. When two bodies having different temperatures are placed in contact, then the resultant temperature is a temperature between the two temperatures.

8. The temperature can be positive or negative value both.

8. The S.I. unit of temperature is $kelvin (K)$.

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Difference between Heat Capacity and Specific Heat Capacity

Heat capacity:

1. Heat capacity is the amount of heat energy required to raise the temperature of the entire body by $1^{\circ}C$.

2. Heat capacity depends on both the nature of the substance and the mass of the body. As the mass of the body increases, the heat capacity of the body also increases.

3. Heat capacity

$C=\frac{Q}{\Delta t}\\ C = mass (m) \times specific \: heat \: capacity (c)$

4. The heat capacity's unit is $J-K^{-1}$.

Specific heat capacity:

1. Specific heat capacity is the amount of heat energy required to raise the temperature of the unit mass of the body by $1^{\circ}C$.

2. Specific heat capacity does not depend on the mass of the body, but it is a characteristic property of the substance of the body.

3. Specific heat capacity

$C=\frac{Q}{m\Delta t} \\ C=\frac{Heat \: Capacity \: (C)}{Mass (m)}$

4. Its unit is $J-kg^{-l}-K^{-1}$.

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Comparison of Isothermal and Adiabatic Processes for an Ideal Gas

Isothermal Process:

1.) In this process temperature remains constant i.e.$(\Delta T= 0)$.

2.) In this process internal energy remains constant i.e. $(\Delta U= 0)$.

3.) This process takes place very slowly.

4.) In this process the system is surrounded by a perfectly conducting material, whose conductivity is infinite.

5.) This process obeys Boyle's law i.e. $(PV= constant)$.

6.) In this process the slope of isothermal curve $=-\frac{P}{V}$

7.) In this process specific heat of gas should be infinite.

Adiabatic Process:

1.) In this process exchange of heat does not take place i.e. $(\Delta Q= 0)$ but temperature changes.

2.) In this process internal energy changes.

3.) This process takes place very rapidly.

4.) In this process the system is surrounded by a perfectly insulating material, whose conductivity is zero.

5.) This process obeys Poisson's law i.e. $(PV^{\gamma} = constant)$.

6.) In this process the slope of adiabatic curve $=- \gamma \frac{P}{V}$

7.) In this process specific heat of gas should be zero.

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