− = .4kg. . . Heat capacity and specific heat capacity Take equal amount of water and oil at temperature °C and heat both of them till they reach the temperature °C.
Note down the time taken by the water and oil to reach the temperature °C. Obviously these times are not same. We can see that water takes more time to reach °C than oil. It implies that water requires more heat energy to raise its temperature than oil.
Now take twice the amount of water at °C and heat it up to °C , note the time taken for this rise in temperature. The time taken by the water is now twice compared to the previous case. We can define ‘heat capacity’ as the amount of heat energy required to raise the temperature of the given body from T to T + ∆T . Heat capacity S = D D Q Specific heat capacity of a substance is defined as the amount of heat energy required to raise the temperature of 1kg of a substance by Kelvin or °C Solution: Here STP means standard temperature (T=273K or °C) and Pressure (P= atm or .
kPa) We can use ideal gas equation V RT = µ Here µ = mol and R = . J/mol.K. By substituting the values V = ( )( . )( ) mol J mol K K Nm = .
× – m We know that Litre (L) = = – m . So we can conclude that mole of any ideal gas has volume . L. By multiplying .4L by K K we get the volume of one mole of gas at room temperature.
It is . L. EXAMPLE . Estimate the mass of air in your class room at NTP.
Here NTP implies normal temperature (room temperature) and atmospheric pressure. Solution The average size of a class is 6m length, m breadth and m height. The volume of the room V = × ×