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First law thermodynamics states that
Heat always refers to energy in transit from one body to another because of temperature difference.
A thermo-dynamical system is changed from state (P1, V1) to (P2, V2) by two different process. The quantity which will remain same will be
Change in internal energy does not depend upon path so remain constant.
If 150 J of heat is added to a system and the work done by the system is 110 J, then change in internal energy will be
If ΔQ and ΔW represent the heat supplied to the system and the work done on the system respectively, then the first law of thermodynamics can be written as
∵ Heat supplied to the system so ΔQ → Positive
and work is done on the system so ΔW → Negative
Hence +ΔQ = ΔU – ΔW
Which of the following can not determine the state of a thermodynamic system
State of a thermodynamic state cannot determine by a single variable (P or V or T)
Which of the following is not a thermodynamics co-ordinate ?
R is the universal gas constant.
In a given process for an ideal gas, dW = 0 and dQ < 0. Then for the gas -
From FLOT
⇒
So temperature will decrease.
Which of the following statements is correct for any thermodynamic system ?
The internal energy and entropy depend only on the initial and final states of the system and not on the path followed to attain that state.
In a thermodynamic process, pressure of a fixed mass of a gas is changed in such a manner that the gas molecules absorb 30 J of heat and 10 J of work is done by the gas. If the initial internal energy of the gas was 40 J, then the final internal energy will be -
⇒ ⇒
First law of thermodynamics is a special case of
Heat supplied to a gas raise its internal energy and does some work against expansion, so it is a special case of law of conservation of energy.
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