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factors affecting the quantity of heat absorbed to increase the temperature of a body

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factors affecting the quantity of heat absorbed to increase the temperature of a body

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The factors are:-

the body's mass-

objects with different mass made from the same substance absorb different amounts of heat energy to raise their temperature by the same amount.

The amount of heat energy absorbed is directly proportional to the object's mass.

the increase in temperature of the body-

objects with equal mass made from the same substance absorb different amounts of heat energy to increase their temperatures by different amounts.

The amount of heat energy absorbed is directly proportional to the rise in temperature.

the material of the body-

objects of the same mass but different materials need different amounts of heat energy to raise their temperature by the same amount.

The amount of heat energy absorbed depends on the substance of the object

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difference between heat capacity and specific heat capacity

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difference between heat capacity and specific heat capacity

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Units of Heat Energy

S.I. Unit is joule ( J )
Other Units are calorie and kilocalorie

One calore = 4.2 J
1000 Calorie= 4200 J or
One kcal = 4200 J

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Consequences of specific heat capacity of water

1)     Moderate climate near coastal areas

Water has a high specific heat capacity of 4200 J kg⁻¹ K⁻¹. It is neither gets heated quickly, nor does it cool quickly. During the day, land gets heated up quickly and hot air above the land rises up and cool air from the sea moves towards the land causing sea breeze. During night, land cools down quickly, so hot air above the sea rises up and cool air from the land moves towards the sea causing land breeze. This makes coastal climate moderate.

2)     In cold countries, farmers fill their fields on a cold winter night

This is because crops are majorly constituted of water, and the water in their bodies tends to freeze and expand, causing failure of the crops. But if the field is filled with water, heat is not lost as quickly to the surroundings, and hence prevents crop failure.

Applications of high and low thermal capacity

1)     Base of cooking pans are made thick

This is to increase the heat capacity of the cooking pan and so it imparts sufficient heat energy at a low temperature. This results in uniform cooking.

2)     Bae of electrical iron is made thick and heavy

This increases the thermal capacity of the base and so the iron remains hot for a longer time even after switching off the current.

Natural Consequence of high specific latent of ice

1)     Drinks get cooled more quickly by adding pieces of ice at 0°C than ice cold water at 0°C

The latent heat of fusion of ice is 336 J g⁻¹. This implies that energy per per gram of ice absorbs 336 J of heat energy from juice to melt into water which is additional heat energy lost by the juice to ice than what it loses to 1 g of ice-cold water.

2)     Snow on mountains does not melt all at once

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Differences between Heat and Temperature

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

Temperature is a quantity/parameter which determines the direction of flow of heat on keeping two bodies at different temperatures in contact.

The amount of heat contained in a body depends on the mass, temperature and substance of that body.

The temperature of a body depends on the average kinetic energy of its molecules due to random motion.

Heat is measured by using the principle of calorimetry.

Temperature of a body is measured by using a thermometer.

Differences between Heat Capacity and Specific Heat Capacity

Heat Capacity is the amount of heat energy required to raise the temperature of the entire body by 1OC .

Specific Heat Capacity  is the amount of heat energy required to raise the temperature of unit mass of the body by 1OC.

Heat Capacity depends on the mass of the body.

Specific Heat Capacity  is independent of the mass of the body.

The S.I. Unit of Heat Capacity is J K⁻¹.

The S.I. Unit of Specific Heat Capacity is J kg⁻¹ K⁻¹.

Differences between Evaporation and Vaporisation.

Evaporation is the change from liquid state to gaseous state due to absorption of heat from the surroundings. [No external heat provided]

Vaporisation is the change from liquid state to gaseous state, due to absorption of heat at a constant temperature known as the substance's boiling point. [External heat is provided.]

Evaporation is a surface phenomenon i.e. it occurs only on the surface of the liquid.

Vaporisation occurs throughout the liquid.

Evaporation occurs at temperatures below the boiling point of the substance.

Vaporisation occurs at the boiling point of the substance

Evaporation causes cooling effect as heat is absorbed [removed] from the surroundings.

Vaporisation doesn't cause any cooling effect.

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Core Definitions and Concepts in Calorimetry

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Core Definitions and Concepts in Calorimetry

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Definition.  The Kinetic Energy due to random motion of the molecules of a substance is known as its heat energy.

Definition.  The average internal kinetic energy of molecules of a substance is a measure of temperature of that substance.

From the very nature of these definitions it is clear that there must exist some direct correlation between the quantities such that a slight change in one reflects as a proportionate change in the other. Therefore, there must exist some quantity which can be defined on the nature of  variation of Heat with respect to Temperature or vice versa.

Definition. The amount of heat energy required to raise the temperature of a body by 1K is called the heat capacity of the body.

Or eqiuvalently, assuming non-linearity - it is the change in heat with respect to change in temperature.

Intuitively, it is apparent that more massive bodies must require greater amount of heat energy to show an equivalent rise in temperature when compared to less massive bodies. This once again, implies that it must be possible to define a quantity that is indpendent of the mass of a body, i.e, it is intrinsic to the nature of the material of the body by scaling against the mass apropriately.

Definition.  The amount of heat energy required to raise the temperature of unit mass of that substance by 1K is the specific heat capacity of the body.

Or equivalently, the mass-averaged thermal capacity of the body.

Assuming linearity, the definitions of thermal capacity and specific heat capacity take the following form mathematically:

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The standard unit of specific hear capacity is joule per kilogram per kelvin ( J/kg/K)
the convenient unit is joule per kilogram per degree celcius (J/kg/°C)
1 J/kg/K =1 J/kg/°C
The cgs unit of specific heat capacity is joules/ gram/ kelvin.
1 J/g/K =1000 J/kg/K
1 J/kg/k =  10⁻³  J/kg/K

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Latent heat, when expressed for unit mass of substance, is called the specific latent heat.
Thus, specific latent heat is : the heat absorbed or liberated for the change of phase/mass or L=Q/M.

Specific latent heat of a phase is the quantity of heat energy absorbed or liberated by the unit mass of the substance for the change in its phase at a constant temperature.

Units of specific latent heat:
SI unit: J/kg
Other units: cal/g and kcal/kg
1 kcal/kg=1 cal/g
1 cal/g=4.2 J/g
or 1 cal/g=4.2*10³ J/kg

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Latent heat, when expressed for unit mass of substance, is called the specific latent heat.
Thus, specific latent heat is : the heat absorbed or liberated for the change of phase/mass or L=Q/M.

Specific latent heat of a phase is the quantity of heat energy absorbed or liberated by the unit mass of the substance for the change in its phase at a constant temperature.

Units of specific latent heat:
SI unit: J/kg
Other units: cal/g and kcal/kg
1 kcal/kg=1 cal/g
1 cal/g=4.2 J/g
or 1 cal/g=4.2*10³ J/kg

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Units of heat energy: SI unit- The SI unit of heat energy is joule (J)The other commonly used units of heat energy are calorie (cal) and kilocalorie (kcal). They are related to the SI unit of heat as follows
1 cal = 4.18J ≈ 4.2 J
1 kcal = 4180 J ≈ 4200 J

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In most situations, adding heat to an object or system causes an increase in temperature, but this is not always the case. Sometimes, the supplied energy instead undertakes some other form of thermodynamic ‘work’ while temperature remains constant. The energy absorbed during such a process( and released when it is reversed ) is known as Latent heat, or its ENTHALPY.