Concept of Heat:
Prescot Joule first illustrated that heat is the form of energy in the experiment in which mechanical work (energy) was transformed in heat. Other scientists also illustrated that heat from fuel, like gasoline in the engine, may be transformed to mechanical energy when engine is utilized to drive carts, trains and airplanes. In the electric power station, heat from fuel is changed to electrical energy. Unit of energy is Joule (J) that is also unit of estimating mechanical energy and electrical energy. There are larger units like kilojoule (KJ) and megajoule (MJ).
Power is the rate of doing work. It is also stated as rate at which heat energy is given out by the source. For instance, heat energy delivered per second by the gas burner is its power. This power is estimated in watts (W). One watt is hence stated as one joule per second (J/s or Js-1). Other larger units are kilowatt (KW) and megawatt (MW).
Source of heat will transfer heat energy to another body. Source is generally at the high temperature while other body being heated is at the lower temperature. When source and other body are in contact, rise in temperature occurs in colder body.
Let t1oC be initial temperature of body and t2oC be final temperature when Q joules of heat has been supplied. Then change in temperature,
ΔΘ = (t2 - t1)0c
Amount of heat in joules which is capable of changing its temperature through 1oC is
This amount of heat to change temperature of body is explained as heat capacity of body. It is generally represented by symbol H.
By definition, heat (thermal) capacity (H) of the body, is quantity heat (Q) in joules needed to change its temperature by one degree (Celsius or one Kelvin).
Therefore H = QJ/ΔΘ0C Where, ΔΘ = (t2 - t1)
Therefore H = QJ(t2 - t1)oC
Hence unit of heat (thermal capacity is expressed in joules per Celsius or joules per Kelvin (JK-1 or JoC-1).
Values of H for different bodies are not same. They differ from one body to another.
Specific Heat Capacity:
If there are different masses of the substance m1, m2 and m3, it will be seen that to raise their temperatures through 1oC each, they will need different quantities of heat energy Q1, Q2 and Q3. Experiments have illustrated that quantities of heat (Q) needed to change temperature through 1oC is proportional to corresponding masses (m).
Q ∝ m
Though, if we fix mass of substance to 1kg and we transfer different quantities of heat Q to it, there will be different equivalent changes in temperature ΔΘ. Again, it will be found that quantities of heat Q to change temperature of 1kg mass of body will be proportional to corresponding changes in temperature ΔΘ. Therefore we can write
Q ∝ ΔΘ
Joining these two factors, we get
Q ∝ mΔΘ
Q = CmΔΘ
Where C is the constant of proportionality called as specific heat capacity of substance
Hence C = Q/mΔΘ
Specific heat capacity of the substance is thus stated as amount of heat Q (in joules) needed to raise temperature of 1kg mass of substance through unit degree (1oC or 1oK).
Unit of C is J/kgoC or Jkg -10C-1 or Jkg-1K-1. It can also be estimated in cal. g-1 k-1. Value of C varies from one substance to another.
Simple Method of Mixtures:
One body is at high temperature and other is at the low temperature. In simple method of mixtures, observe that at hot and cold substances being mixed without considering container in which they are being mixed. Principle of conservation of heat energy is being seen very closely. Here, very in brief, explain principle of conservation of heat energy.
This principle defines that the heat lost by the hot body is equal to heat gained by cold body in any system given there is no heat exchange between substances involved and their surroundings.
Inclusion of Calorimeter in Method of Mixtures:
Consider calorimeter as one of the main players in heat exchange and principle of conservation of heat energy. Here we have the hot body A at the higher temperature than liquid contained in calorimeter. Therefore, liquid and calorimeter are considered as cold body gaining heat from the hot body.
Let the hot body (A) with mass m1, Specific heat capacity C1 its initial temperature t1 and Final temperature of mixture is = t.
Then, Heat lost by hot body:
Q1 = m1c1ΔΘ1
Q1 = m1c1(t1 - t)
Again let cold liquid (B) with mass m2, specific heat capacity C2 with initial temperature t2. Final temperature of mixture is t. Heat gained by cold liquid (B) = Q2
Q2 = m2C2ΔΘ2
Q2 = m2C2 (t - t2)
Let the cold calorimeter (C) with mass m3, specific heat capacity C3, Specific heat capacity = C3 Initial temperature t3 and Final temperature of mixture t. Heat gained by cold calorimeter C is Q3.
Q3 = m3C3ΔΘ3
Q3 = m3C3 (t - t3)
It can be noted here that liquid (B) and calorimeter (C) are both gaining heat. Thus their changes in temperature will be same.
θ2 = Δθ3
(t - t2) = (t - t3)
In most cases, m3 and C3 may not be given for you in heat exchange. Rather, the property of container that is calorimeter may be given in form of thermal capacity (H) of calorimeter. Therefore, quantity of heat gained by calorimeter is stated as
Q3 = HΔθ3 = m3C3Δθ3
Q3 = H(t - t2)
By applying the principle of conversation of heat energy, relation between quantities Q1, Q2 and Q3 is
Heat lost = Heat gained
Q1 = Q2 + Q3
m1C1 (t1 - t) = m2C2 (t - t2) + m3C3 (t - t2)
Or m1C1 (t - t1) = m2C2 (t - t2) + H (t - t2)
Specific Latent Heat of Fusion:
A solid comprises of atoms or molecules held in fixed structure by forces of attraction between them. Such atoms or molecules vibrate about the mean position. When heat is thus supplied to solid kinetic energy of vibration increases hence increasing temperature of solid. Heat supplied is estimate by mCΔθ . At melting point, heat given to solid is utilized to overcome forces of attraction between atoms or molecules that keep solid in its rigid form, and then solid melts.
At this point we state specific latent heat of fusion (LF) as quantity of heat needed to change 1kg mass of a solid at the melting point to liquid at same temperature.
Specific Latent Heat of Vaporization:
Unlike solids, the liquid has no definite form; it generally takes shape of its container. It molecules move in random manner inside though molecules are close enough to attract each other. Some molecules, that have greatest kinetic energy, are able to escape through surface. They then exist as vapor outside the liquid. This procedure is known as evaporation and it occurs at all temperatures. Though, boiling occurs at the definite temperature, boiling point that depends on external pressure. Water for instance boils at 100oC and at the pressure 760mmHg. It does so at the lower temperature when external pressure is lower like boiling point of water at top of the mountain is less than 100oC. Boiling takes place throughout whole volume of liquid while evaporation is the surface phenomenon.
At this point, we would state specify latent heat of vaporization as quantity of heat needed to change 1kg mass of liquid at boiling point to vapor at same temperature.
Latent Heat and Internal Energy:
When the liquid reaches boiling point, energy required to change it to vapor is: (i) energy or work required to separate liquid molecules from the mutual attraction until they are comparatively far apart in gaseous state. (ii) Energy or work required to push back external pressure so that molecules can escape from the liquid. Latent heat of vaporization is utilized in point (i) that is required to change internal energy of liquid while point (ii) is external work done against external pressure. Work done in this case is stated as
W = pΔV
Where, p is external pressure and ΔV is change in volume 1g of water changes to approx 1672cm3 of steam
Hence ΔV = (1672 - )cm3
= (1671 X 10-6)cm3
Assume external pressure P = 1.013 x 105 Nm-2
The work done (W) = pΔV is hence
= 1.0 pΔV 13 x 105N/m2 X 1671 X 10-6m3
Latent heat of vaporization per gram of water = 2260J
Therefore internal energy part of latent heat of vaporization
= (2260 - 169.3)J
This is much greater than external work done. Latent heat of fusion is approx 340J. So energy required to overcome bonds between molecules in solid state is much less than energy to form the gaseous molecules from the liquid state.
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