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Beaches are such a beauty of nature, aren’t they? This is really what we need when we are in the mood to relax. We love watching water meeting the sand and the sunset at the horizon.
The sand on the beach is hot when the sun is beating down, but what about the water in the sea? Well! It's much cooler! Have you ever wondered why the water is cooler than the sand even though they are heated by the same source up there? Let’s look at what is happening here.
Table of contents
e and a wooden spoon in the second. The metal spoon gets heated quite quickly in terms of temperature rie. For the same amount of heat, the temperature of the metal spoon increases a lot in comparison with the wooden spoon. If we were to observe a onedegree temperature increase in the
Let’s assume that both the land surface near to the sea and water are at the same temperature, say 20^{0}C Both got exposed to the sun till noon, due to this the temperature of the land surface has been raised to 40^{o}C but the temperature of the water is still pleasant, 25^{o}C. We can see that despite being exposed to the same amount of heat, the rise in temperature of land and water is not the same.
Clearly, both have shown different sensitivities to heat in regards to temperature, isn’t it?
Let’s substantiate the above claim with some facts. It takes about 78,000 joules of heat to increase the temperature of a kilogram of seawater from 20^{o}C to 40^{o}C. Whereas it takes only about 15,000 joules for the same mass of sand to increase its temperature from 20^{o}C to 40^{o}C.
So we can clearly see that different substances require different amounts of heat to raise the temperature by the same amount. Alternatively, it can be said that some substances show a higher temperature rise than others for the same amount of heat they absorb. By knowing how much heat a given substance needs to raise its temperature by a particular amount is something of relevance to us in thermodynamics. The property that specifically tells us about this is called heat capacity.
The heat capacity of a substance can be defined as the amount of heat required to raise the temperature of a given amount of substance by onedegree celsius.
Mathematically, heat capacity can be expressed as:
Where,q is the heat energy required to bring about a temperature change of and C is the heat capacity of the substance.
Similarly, it can be written as:
dq = cdT (for a very small change in the temperature)
Integrating both the sides,
Heat capacity for a given matter depends on its size or quantity and hence it is an extensive property. The unit of heat capacity isJ K^{1} or J^{0}C^{1}.
Scientists defined specific heat capacity as a quantity that was independent of the quantity or size of the material being studied for thermodynamic investigations. Since it is unaffected by the size or quantity of the matter, it is an intensive quality.
Specific heat capacity of a substance can be defined as the amount of heat energy required to raise the temperature of one kilogram of a substance by onedegree celsius.
Mathematically, specific heat capacity can be expressed as:
Where Q is the amount of heat transfer, is the change in the temperature, m is the mass of the substance and C_{s} is the specific heat capacity.
The unit of specific heat capacity (C_{S}) is K Kg^{1}K^{1}
Similarly it can be written as:
dq = mC_{s}dT (for a very small change in the temperature)
Integrating both the sides,
Molar heat capacity of a substance can be defined as the amount of heat energy required to raise the temperature of one mole of a substance by onedegree celsius.
Mathematically, molar heat capacity can be expressed as:
Where Q is the amount of heat transfer, is the change in the temperature, n is the no. of moles of the substance and C_{s }is the specific heat capacity.
Similarly it can be written as:
dq = nC_{m}dT (for a very small change in the temperature)
Integrating both the sides,
The unit of C_{m} is J mol^{1}K^{1}
The molar heat capacity is an intensive property of a substance, that does not depend on the amount and size of the substance.
Molar heat capacity (C_{m}) is the product of the specific heat capacity (C_{s}) and the molar mass of the substance (M).
Mathematically,
Where, M is the molar mass of the substance
The heat required to raise the temperature of one mole of gas by 1 °C (or 1 K) at constant
volume is called heat capacity at constant volume (C_{v}).
Where, n is no. of moles of the gas, dq_{v} is heat transfer at constant volume, dT is a small change in the temperature.
The heat required to raise the temperature of one mole of gas by 1 °C (or 1 K) at constant
pressure is called heat capacity at constant pressure (C_{p}).
Where, n is no. of moles of the gas, dp_{q} is heat transfer at constant pressure, dT is a small change in the temperature.
Consider an ideal gas. Let dq be the amount of heat given to the system to raise the temperature of an ideal gas by dT, and change in internal energy be du. Then, According to the first law of thermodynamics;
Note: The above relation between C_{p}&C_{v} is true only for an ideal gas.
Q 1. (C_{p}  C_{v}) = R is for n moles of a gas. If we consider 1 mol of the gas. The correct formula among the following is:
Answer: (A)
We know;
Equation (a) is derived from the first law of thermodynamicsfor n moles of a gas.
If we consider n = 1 mol putting the value of n in equation (a), we get;
Q 2. The amount of heat required to raise the temperature of the unit mass of a gas by onedegree Celcius at constant pressure is:
A) C_{v}
B) C_{p}
C) C_{s}
D) None of the above
Answer: (B)
The heat required to raise the temperature of one mole of gas by 1 °C (or 1 K) at constant
pressure is called heat capacity at constant pressure (C_{p}).
Q 3. 10 g piece of a metal absorbs 300 J of energy in the form of heat. The temperature of the metal got raised from 27^{0}C to 47^{0}C. The specific heat of the metal would be:
Answer: Option (A)
Given,
q = 300 j
m = 10 g
We know that,
Where,
q = heat energy,
C_{s} = specific heat capacity
m = ass of a substance
Then, specific heat capacity,
Q 4. 550 j of heat was absorbed by a sample of CaCO_{3} when its temperature was increased by 5K . If the molar heat capacity of CaCO_{3} is 82 J mol^{1}K^{1}, then the number of moles of CaCO_{3} will be:
a. 2.50 mol
b. 3.45 mol
c. 1.34 mol
d. 1.70 mol
Answer: Option (C)
Given,
Where,
q = heat energy
C_{m} = molar heat capacity
n = number of moles
On rearranging the equation, we get,
Substituting the values in the equation, we get,
n = 1.34 mol
Q 1. Can the heat capacity of any substance be zero?
Answer: Zero heat capacity of any substance means an infinitesimally small amount of heat will increase the temperature by an infinitely large amount because it has very less internal degrees of freedom into which it can channel the absorbed energy or heat. The smaller the heat capacity, the lesser the number of internal degrees of freedom and vice versa.
Q 2. What is the importance of heat capacity?
Answer: Larger the heat capacity, the more the heat a substance can store, even with a slight increment in the temperature. For example; water has high heat capacity, so even to increase the slightest of temperature it would need a large amount of heat energy.
That’s why water's high heat capacity makes it ideal for central heating systems since it can transfer a lot of energy even with a slight change in temperature.
Q 3. Is specific heat capacity an intensive or extensive property?
Answer: Specific heat is an intensive property. Its magnitude does not depend upon the amount of matter present in the system.
Q 4. What factors affect heat capacity?
Answer: Experiments show that the transferred heat depends on the following factors:
Q 5. How do we measure heat capacity?
Answer: Start with the object at a known uniform temperature, add a known amount of heat energy, wait for the temperature to become uniform, and measure the change in temperature and then by using the formula of heat transfer; , calculate the heat capacity of a substance (C).
Isothermal Process  Thermodynamic Terms 
Thermodynamic Processes  Degrees of Freedom 
Isobaric Process 
Zeroth Law of Thermodynamics

Second Law of Thermodynamics

Third Law of Thermodynamics
